Answer:
=> 0.10 moles
Explanation:
The question is asking us to find the moles of NaCl cid formed.
We have been provided with;
0.10 L of 1.0 M NaOH.
We know that mole ratio of the reaction is 1:1 and also the molarity of a solution is contained in 1 L or 1000 mL or 1000 cm³.
This means that;
1.0 M is contained in 1.0 L.
X mol is contained in 0.10 L
[tex] x \: mol \: = \frac{0.1 \times 1.0}{1.0} \\ = 0.10 \: mol[/tex]
= 0.10 moles of NaCl formed
A sample of helium gas inside a closed but flexible container occupies a volume of 355mL at 23°C. If the pressure is held constant, to what temperature must the He be raised to cause the container to expand to a final volume of 1.50 L?
Answer:
978.19° C
Explanation:
P1V1/T1 =P2V2/T2 Since the pressure is constant, this can be written as
V1/T1 = V2/T2 RE-ARRANGE TO
V2 * T1/V1 = T2 Note: T must be in Kelvin!!
1.5 L * (273.15 + 23) / (.355 L ) = T2 = 1251.338 K =978.19 C
a compound with a molar mass of 92g/mol contains 0.3955g of nitrogen and 0.904g of oxygen. Determine the empirical and molecular formula
Answer:
Empirical: NO2. Molecular: N2O4
Explanation:
In order to determine the empirical formula, we divide each element's mass by their respective molar mass:
N: 0.3955g/14.01 g/mol = 0.02823 mol
O: 0.904g/16.00 g/mol = 0.0565 mol
Next, we take the smallest value and multiply it till it is close enough to an integer:
0.02823 x 40 = 1.12 Close enough to 1.
0.0565 x 40 = 2.26. Close enough to 2.
Therefore, the Empirical Formula is: NO2
Next, we determine how much the Empirical formula weighs and see if it matches 92g/mol:
14.01 g/mol + 2(16.00 g/mol) = 46.01 g/mol
We can assume this is roughly half of 92 g/mol so we can multiply each subscript by 2 to match the weight.
Therefore, the Molecular formula is N2O4
Hope this helped!
In a constant‑pressure calorimeter, 55.0 mL of 0.310 M Ba(OH)2 was added to 55.0 mL of 0.620 M HCl.
The reaction caused the temperature of the solution to rise from 24.25 ∘C to 28.47 ∘C. If the solution has the same density and specific heat as water ( 1.00 g/mL and 4.184J/g⋅°C,) respectively), what is Δ for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes.
The enthalpy change (ΔH) for the reaction (per mole H₂O produced) is 56.96 KJ/mol
How to determine the mass of the solutionVolume = 55 + 55 = 110 mLDensity = 1 g/mLMass = ?Mass = density × volume
Mass = 1 × 110
Mass = 110 g
How to determine the heat Mass (M) = 110 gInitial temperature (T₁) = 24.25 °C Final temperature (T₂) = 28.47 °CChange in temperature (ΔT) = 28.47 – 24.25 = 4.22 °C Specific heat capacity (C) = 4.184 J/gºC Heat (Q) =?Q = MCΔT
Q = 110 × 4.184 × 4.22
Q = 1942.2128 J
How to determine the mole of H₂O producedBa(OH)₂ + 2HCl --> BaCl₂ + 2H₂O
Since the reaction occurs in a constant‑pressure calorimeter, it means both reactants are sufficient enough for the reaction.
Mole of Ba(OH)₂ = molarity × volume
Mole of Ba(OH)₂ = 0.310 × (55 / 1000)
Mole of Ba(OH)₂ = 0.01705 mole
From the balanced equation above,
1 mole of Ba(OH)₂ reacted to produce 2 moles of H₂O.
Therefore,
0.01705 mole of Ba(OH)₂ will react to produce = 0.01705 × 2 = 0.0341 mole of H₂O.
How to determine the enthalpy change ΔH per mole of H₂O producedHeat (Q) = 1942.2128 JMole of H₂O (n) = 0.0341 moleEnthalpy change (ΔH) =?ΔH = Q / n
ΔH = 1942.2128 / 0.0341
ΔH = 56956.29 J/mol
Divide by 1000 to express in KJ/mol
ΔH = 56956.29 / 1000
ΔH = 56.96 KJ/mol
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The compound HgO can be decomposed to form Hg and O2. This can be represented at the atomic level by a chemical equation:
2HgO 2Hg + O2
According to the law of conservation of mass, if 23.5 grams of HgO decomposes and 21.8 grams of Hg is formed, how many grams of O2 must simultaneously be formed?
According to the law of conservation of mass 1.7 grams of [tex]O_2[/tex] will be formed.
What are moles?A mole is defined as 6.02214076 × 1[tex]0^{23}[/tex]of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
[tex]2HgO[/tex]→ [tex]2Hg + O_2[/tex]
According to the laws of conservation mass of reactants should be equal to the mass of products.
23.5 grams - 21.8 grams
1.7 grams of [tex]O_2[/tex] will be formed.
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Determine the number of moles of H in each sample
The number of mole of H in NH₃, given the data is 23.85 moles
Data obtained from the questionMole of NH₃ = 7.95 molesMole of H in NH₃ =?How to determine the mole of H in 7.95 moles of NH₃1 mole of NH₃ contains 3 moles of H
Therefore,
7.95 moles of NH₃ will contain = 7.95 × 3 = 23.85 mole of H
Thus, 23.85 mole of H is present in 7.95 moles of NH₃
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When 25.0 g of ch4 reacts completely with excess chlorine yielding 45.0 g of ch3cl, what is the percentage yield, according to ch4(g) + cl2(g) → ch3cl(g) + hcl(g)?
*
Taking into account definition of percent yield, the percent yield for the reaction is 57.08%.
Reaction stoichiometryIn first place, the balanced reaction is:
CH₄ + Cl₂ → CH₃Cl + HCl
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
CH₄: 1 mole Cl₂: 1 moleCH₃Cl: 1 moleHCl: 1 moleThe molar mass of the compounds is:
CH₄: 16 g/moleCl₂: 70.9 g/moleCH₃Cl: 50.45 g/moleHCl: 36.45 g/moleThen, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
CH₄: 1 mole ×16 g/mole= 16 gramsCl₂: 1 mole ×70.9 g/mole= 70.9 gramsCH₃Cl: 1 mole ×50.45 g/mole= 50.45 gramsHCl: 1 mole ×36.45 g/mole= 36.45 gramsMass of CH₃Cl formed
The following rule of three can be applied: if by reaction stoichiometry 16 grams of CH₄ form 50.45 grams of CH₃Cl, 25 grams of CH₄ form how much mass of CH₃Cl?
[tex]mass of CH_{3} Cl=\frac{25 grams of CH_{4}x 50.45grams of CH₃Cl }{16 grams of CH_{4}}[/tex]
mass of CH₃Cl= 78.83 grams
Then, 78.83 grams of CH₃Cl can be produced from 25 grams of CH₄.
Percent yieldThe percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.
The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:
[tex]percent yield=\frac{actual yield}{theorical yield}x100[/tex]
where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.
Percent yield for the reaction in this case
In this case, you know:
actual yield= 45 gramstheorical yield= 78.83 gramsReplacing in the definition of percent yields:
[tex]percent yield=\frac{45 grams}{78.83 grams}x100[/tex]
Solving:
percent yield= 57.08%
Finally, the percent yield for the reaction is 57.08%.
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How much does 2.3 moles of Mg(NO2)2 weigh?
Answer:
mass = 266.8 g
Explanation:
mass = no. of moles x molar mass ([tex]M_r[/tex])
[tex]M_r \space\ \space\ of[/tex] [tex]Mg(NO_2)_2[/tex] = 24 + 2[14 + 2(16)]
= 116
∴ mass = 2.3 x 116
= 266.8 g
What is hypotheses
?
Answer:
is an assumption , in an idea that is proposed for the sake of argument so that it can be tested to see if it might be true.
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What is the molality, m, of a solution made by adding 8.21 g of solid naphthalene, C10H8, to 27.92 g of liquid benzene, C6H6? The molar mass of naphthalene = 128.2 g/mol and benzene = 78.1 g/mol.
4.21×[tex]10^{-4}[/tex] Molal is the molality, m, of a solution made by adding 8.21 g of solid naphthalene, [tex]C_{10}H_8[/tex], to 27.92 g of liquid benzene,[tex]C_6H_6[/tex].
What are moles?A mole is defined as 6.02214076 × [tex]10^{23}[/tex]of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
[tex]Molality = \frac{Moles \;solute}{Solvent \;in \;kg}[/tex]
Moles of naphthalene=[tex]\frac{mass}{molar \;mass}[/tex]
Moles of naphthalene[tex]=\frac{8.21 g}{128.2 g/mol}[/tex]
=0.064
Moles of benzene[tex]=\frac{mass}{molar \;mass}[/tex]
Moles of benzene[tex]=\frac{27.92 g}{78.1 g/mol}[/tex]
=0.357
Total mole of solute= 0.064+0.357=0.421
[tex]Molality = \frac{Moles \;solute}{Solvent \;in \;kg}[/tex]
[tex]Molality = \frac{0.421 }{1000}[/tex]
Molality = 4.21×[tex]10^{-4}[/tex] Molal
Hence, 4.21×[tex]10^{-4}[/tex] Molal is the molality, m, of a solution made by adding 8.21 g of solid naphthalene, [tex]C_{10}H_8[/tex], to 27.92 g of liquid benzene, [tex]C_6H_6[/tex].
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Using what you learned in this lab, how could you determine the polarity of other common household substances?
It is possible to determine the polarity of common household substances by dissolving them into water.
What are polar molecules?Polar molecules are those that may form hydrogen chemical bonds with water molecules, which contain positive and negative regions.
Polar molecules depend on the unsymmetrical distribution of negative electrons in their atoms.
In conclusion, the polarity of common substances can be determined by dissolving them into water.
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In the preparation of the soap above, a student dissolved 5 g of NaOH in 25 mL water and added 10 mL palm kernel oil (density: 0.997 g/cm3). The mixture was heated and boiled with 20 mL of water, followed by addition of NaCl to the soap solution. At the end of the experiment, the student obtained 6.2 g of soap What is the percentage yield of the soap?
The Percent yield of soap is 17.8%
What is the percent yield of soap?Percent yield is given as follows:
Percent yield = actual yield/expected yield * 100%The actual yield of soap = 6.2 g
The expected yield is determined from the equation of the reaction.
The equation of the reaction is given as follows:
NaOH + CH₃(CH₂)₁₄COOH ----> CH₃(CH₂)₁₄COONa + H₂O
Molar mass of (palm kernel oil) CH₃(CH₂)₁₄COOH = 256 g/mol
Molar mass of NaOH = 40 g/mol
Molar mass of (soap) CH₃(CH₂)₁₄COONa = 278 g/mol
Mass of palm kernel oil = 9.9 g
Expected mass of soap = 5/40 * 278 = 34.75 g
Percent yield = 6.2/34.75 * 100 = 17.8%
Therefore, the Percent yield of soap is 17.8%
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2FeCl + 3Na2CO2= Fe2 (CO3)3 + 6NaCl
If you begin a reaction with 127.490 g of Na2CO3, how many moles of NaCl can you theoretically produce, assuming an excess of FeCl3 is present?
I need help
Taking into account the reaction stoichiometry, 2.405 moles of NaCl are formed when 127.49 grams of Na₂CO₂ reacts with excess of FeCl₃.
Reaction stoichiometryIn first place, the balanced reaction is:
2 FeCl+ 3 Na₂CO₂ → Fe₂(CO₃)₃ + 6 NaCl
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
FeCl: 2 moles Na₂CO₂: 3 molesFe₂(CO₃)₃: 1 moleNaCl: 6 molesThe molar mass of the compounds is:
FeCl: 91.3 g/moleNa₂CO₂: 106 g/moleFe₂(CO₃)₃: 291.7 g/moleNaCl: 58.45 g/moleThen, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
FeCl: 2 moles ×91.3 g/mole= 182.6 gramsNa₂CO₂: 3 moles ×106 g/mole= 318 gramsFe₂(CO₃)₃: 1 mole ×291.7 g/mole= 291.7 gramsNaCl: 6 moles ×58.45 g/mole= 350.7 gramsMass of NaCl producedThe following rule of three can be applied: if by reaction stoichiometry 318 grams of Na₂CO₂ form 6 moles of NaCl, 127.49 grams of Na₂CO₂ form how many moles of NaCl?
[tex]moles of NaCl=\frac{127.49 grams of Na_{2} CO_{2} x6 moles of NaCl }{318grams of Na_{2} CO_{2} }[/tex]
moles of NaCl= 2.405 moles
Then, 2.405 moles of NaCl are formed when 127.49 grams of Na₂CO₂ reacts with excess of FeCl₃.
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A solid is 5 cm tall, 3 am wide, and 2 cm thick. It has a mass of 135 g. What is the solid's density?
Answer:
density of solid = 4.5 g/cm³
Explanation:
density = mass ÷ volume
• We know the mass of the object (135 g). We need to calculate the volume:
Volume = length × width × thickness
= 5 cm × 3 cm × 2 cm
= 30 cm³
• Now we can calculate the solid's density:
density = 135 g ÷ 30 cm³
= 4.5 g/cm³
A space shuttle gaining speed as it travels through earth's atmosphere? A) 1st Law B) 2nd Law C) 3rd Law
If 5.00 L of argon gas is at 0.460 atm and -123°C, what is the volume at STP?
Answer:
4.27 L
Explanation:
STP = 0 C and 1 atm
P1V1/T1 = P2V2/T2 where T is in Kelvin
P1 V1 / T1 *T2/P2 = V2
.469 * 5 / ( 273.15-123) * 273.15/1 = V2 = 4.27 L
when 1 mol of glucose is burned, 2802.5kj of energy is released. calculate rhe quantity of energy released to a person by eating 5.00g of glucose in a candy
77.78 kJ of energy is released when 1 mol of glucose is burned, 2802.5 kJ of energy is released.
What are moles?A mole is defined as 6.02214076 ×[tex]10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
Calculate the moles of 5.00g of glucose.
Given mass = 5.00g
The molar mass of glucose = 180.156 g/mol
[tex]Moles = \frac{mass}{molar \;mass}[/tex]
[tex]Moles = \frac{5.00g}{180.156 g/mol}[/tex]
Moles =0.02775372455
The quantity of energy released to a person by eating 5.00g of glucose in a candy.
0.02775372455 x 2802.5 kJ
77.77981305 kJ =77.78 kJ
Hence, 777.78 kJ of energy is released.
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Consider the following chemical reaction:
2 Cr(OH)3(aq) ------------> Cr2O3(s) + 3H2O(l)
12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced.
From the calculation, the moles of water produced is 18 moles of water.
What is a decomposition reaction?A decomposition reaction is one in which a substance is split up into smaller parts.
We have the reaction; 2 Cr(OH)3(aq) ------------> Cr2O3(s) + 3H2O(l)
From this reaction;
2 moles of Cr(OH)3 produced 3 moles of water
12 moles of Cr(OH)3 will produce;
12 moles * 3 moles / 2moles
= 18 moles of water
Hence, 12 moles of chromium (III) hydroxide produces 18 moles of water.
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How much would a 55 kg person weigh on venus
Answer:
109.988623 Pounds or 49.89kg
Explanation:
Solve this whole experiment,
I'll be so glad . thanks
●do the above experiment
●give detailed answers
THANKS
In Part A, we saw that the theoretical yield of aluminum oxide is 1.60 mol . Calculate the percent yield if the actual yield of aluminum oxide is 1.22 mol .
Taking into account definition of percent yield, the percent yield for the reaction is 76.25%.
Percent yieldThe percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.
The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:
[tex]percent yield=\frac{actual yield}{theorical yield}x100[/tex]
where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.
Percent yield in this caseIn this case, you know:
actual yield= 1.22 moltheorical yield= 1.60 molReplacing in the definition of percent yields:
[tex]percent yield=\frac{1.22 mol}{1.60 mol}x100[/tex]
Solving:
percent yield= 76.25%
Finally, the percent yield for the reaction is 76.25%.
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Determine the molar mass of a gas that moves 1.25 times as fast as CO2.
The molar mass of a gas that moves 1.25 times as fast as CO2 is 28.16 g.
Molar mass of the gas
The molar mass of the gas is determined by applying Graham's law of diffusion.
R₁√M₁ = R₂√M₂
R₁/R₂ = √M₂/√M₁
R₁/R₂ = √(M₂/M₁)
where;
R₁ is rate of the CO2 gasM₁ is molar mass of CO2 gasR₂ is rate of the second gasM₂ is the molar mass of the second gasR₁/1.25R₁ = √(M₂/44)
1/1.25 = √(M₂/44)
0.8 = √(M₂/44)
0.8² = M₂/44
M₂ = 0.8² x 44
M₂ = 28.16 g
Thus, the molar mass of a gas that moves 1.25 times as fast as CO2 is 28.16 g.
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Which of the following equations is correct for coffee-cup calorimeter?
q reaction = q calorimeter
q reaction = -q calorimeter
The equation that is correct for coffee-cup calorimeter is q reaction = -q calorimeter. Details about coffee-cup calorimeter.
What is a calorimeter?A calorimeter is an apparatus for measuring the heat generated or absorbed by either a chemical reaction, change of phase or some other physical change.
A coffee-cup calorimeter is a specific type of calorimeter that involves the absorption of heat of a reaction by water when a reaction occurs.
The enthalpy change of the reaction is equal in magnitude but opposite in sign to the heat flow for the water:
qreaction = -(qwater)
Therefore, the equation that is correct for coffee-cup calorimeter is q reaction = -q calorimeter.
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Discuss why the solubility of CaCO33(s) would be greater in distilled water than in tap water that contains 50 mg/L of calcium ions (Ksp CaCO3 = 8.7x10-9).
Answer:
mitxtitsixitdkgxgxmhhxlyfuldyooyddryodyoodyyodroydgodydout70r9ryiryogiustoydotsixulslysrluhsro6rh zpyrqujs7t7wiyidiey9ye9yd96d9ydoydoydodyoydoydoyydgkxyodigggoydyoydyyo
Explanation:
uodigdoydoydohhxoydoydodkgdyodisirs85ssto toutuset8itgxotteotsmvtieksititsgie8e85t8upfgtjwdujhftisnfvoyxuvfgkrtj57lhmdkhflfheogkhptufsjfxocljhflhfoydllbxoydoggsigxitieoyurreifosuuluprohgsjtgjzffgfhcpzfjchzjfcg gsjiggdoydogxlhd6oxhx9yfljf
The greater, the ionic property, the greater will be solubility. water is a covalent compound where calcium carbonate is ionic that's why the solubility of [tex]CaCO_{3}[/tex](s) would be greater.
What is solubility?The capability of a substance, the solvent, to combine with another substance, the solvent, has been known as solubility. Insolubility, or just the solute's inability to create that kind of a solution, would be the opposite attribute.
How does solubility depend on the ionic compound?Ionic chemicals dissolve readily in just about any liquid that has the ability to rupture the ionic link present in them. Since water itself has a stronger ionic bond and is still polar in nature, water disrupts the ionic link by hydrogen bonding. Several other solvents, like kerosene and gasoline, are unable to dissolve the ionic bond.
The greater, the ionic property, the greater will be solubility. water is a covalent compound where calcium carbonate is ionic that's why the solubility of [tex]CaCO_{3}[/tex](s) would be greater in distilled water than in tap water that contains 50 mg/L of calcium ions
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How much pure alcohol is in a 316 mL bottle of a "wine cooler" that is 4.8 percent alcohol by volume?
Answer:
15.17 ml
Explanation:
4.8 % is .048 in decimal
316 ml * .048 = 15.17 ml ( about 1/2 ounce)
1. Balance the equation below: Fe(s) + Cl₂(g) → FeCl3(aq) 2. Calculate the moles of FeCl3 that will form if 2.0 moles of Fe react with sufficient Cl₂. 3. Calculate the moles of FeCl3 that will form if 1.0 moles of each reactant mix together. 4. How many grams of FeCl3 that will form if 1.0 g of each reactant mix?
Answer:
1.) 2 Fe (s) + 3 Cl₂ (g) ---> 2 FeCl₃ (aq)
2.) 2.0 moles FeCl₃
3.) 0.67 moles FeCl₃
4.) 1.5 g FeCl₃
Explanation:
1.)
The unbalanced reaction:
Fe (s) + Cl₂ (g) ---> FeCl₃ (aq)
Reactants: 1 iron, 2 chlorine
Products: 1 iron, 3 chlorine
The balanced reaction:
2 Fe (s) + 3 Cl₂ (g) ---> 2 FeCl₃ (aq)
Reactants: 2 iron, 6 chlorine
Products: 2 iron, 6 chlorine
2.)
To find moles FeCl₃, you need to multiply the given value by the mole-to-mole ratio of Fe to FeCl₃. This ratio is constructed via the coefficients from the balanced equation.
2.0 moles Fe 2 moles FeCl₃
--------------------- x ------------------------ = 2.0 moles FeCl₃
2 moles Fe
3.)
To determine how much FeCl₃ is produced, you need to identify the limiting reagent. To find it, you need to convert both reactants to the product then identify which reactant gives you the smallest amount of product. This reactant is the limiting reagent and will give you your actual answer.
1.0 mole Fe 2 moles FeCl₃
------------------- x ----------------------- = 1.0 moles FeCl₃
2 moles Fe
1.0 mole Cl₂ 2 moles FeCl₃
------------------- x ------------------------ = 0.67 moles FeCl₃
3 moles Cl₂
4.)
Because Cl₂ is the limiting reagent, we need to convert grams Cl₂ to grams FeCl₃. This can be done using the molar masses of both compounds and the mole-to-mole ratio.
Molar Mass (Cl₂): 2(35.453 g/mol)
Molar Mass (Cl₂): 70.906 g/mol
Molar Mass (FeCl₃): 55.845 g/mol + 3(35.453 g/mol)
Molar Mass (FeCl₃): 162.204 g/mol
1.0 g Cl₂ 1 mole 2 moles FeCl₃ 162.204 g
------------- x ----------------- x ----------------------- x ------------------ = 1.5 g FeCl₃
70.906 g 3 moles Cl₂ 1 mole
A student performs the following lead extraction to test the stoichiometric method and to determine the efficiency of the reaction. In the reaction 49.5 g of lead(II) nitrate is reacted with excess zinc in a single displacement reaction.
a. Calculate the theoretical yield of lead in the experiment.
b. After separating the lead by filtration and allowing it to dry, the student obtains 19.8g of lead. What is the percent yield of the experiment?
Theoretical yield produced is 31.8 gram and the percentage yield is 62.27%.
The zinc (Zn) is more reactive than lead (Pb). So that zinc loses electrons more easily than lead .
And the electrons of Zn are transfer to lead in this reaction .
This question is a limiting reactant question .
And For limiting reactant questions so that we need to determine that how much product can be produced by all reactant .
Zinc and Lead (II) nitrate react to form Zinc Nitrate and Lead.
Zn + Pb(NO₃)₂ → Zn(NO₃)₂ + Pb
Now we have- Weight of Pb(NO₃)₂ = 49.5 g
molar mass of Pb(NO₃)₂ = 331.2 g
now moles of Pb(NO₃)₂ = 49.5 ÷ 331.2 = 0.15 moles
Moles of Pb consumed = 1 × 0.15 = 0.15
moles mass of Pb consumed = 0.15 × 207.2 = 31.8 gm
Here Zn is in excess so that lead(II) nitrate is a limiting reactant.
(a) Theoretical yield of lead -
moles of Pb produced = 0.15 × 1 = 0.15 moles
molar mass of Pb = 207.2g
mass of Pb produced in reaction = 0.15 × 207.2 = 31.08 g
theoretical yield = 31.8 gram
(b) After separating the lead by filtration -
obtained lead = 19.8gm
Percentage yield = 19.8 ÷ 31.8 ×100 = 62.27%
so that after separating the lead the percentage yield is 62.27%.
So, After applying the concepts of stoichiometric method the theoretical yield produced came out to be 31.8 gram and the percentage yield came out to be 62.27%.
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Consider the following balanced chemical reaction: 2 H2(g) + CO (g) -> CH4O (1). If
6.12 g of H₂ reacts with excess CO, how many grams of CH4O can be produced?
Select one:
a. 16.5g
b. 27.29
c. 64.5g
d. 48.6 g
e. 75.8 g
Answer:
d
Explanation:
2H₂(g) +CO(g) → CH₄O (l)
Since H₂ was reacted with excess CO, H₂ is the limiting reagent. This means that the amount of product formed is dependent on the amount, i.e. the number of moles, of H₂.
The number of moles of H₂ can be calculated by taking the mass divided by its Mr (relative molecular mass).
Mr of H₂= 2(1)= 2
Moles of H₂ (g)
= 6.12 ÷2
= 3.06 mol
From the balanced equation, 2 moles of H₂(g) produces 1 mole of CH₄O(g).
Since we have 3.06 moles of H₂(g),
Moles of CH₄O (l) produced
= 3.06 ÷2
= 1.53 mol
Mr of CH₄O
= 12 +4 +16
= 32
Mass= mole ×Mr
Mass of CH₄O (l) produced
= 1.53(32)
= 48.96 g
Thus, d would be the best option.
what substances dissociate into ions when dissolved in water
Polar or ionic substances dissociate into ions when dissolved in water.
What substances dissociate into ions when dissolved in water?Ionic substances dissociate into ions when dissolved in water because water is also a polar by nature. We know that like dissolve like so polar substances dissolve in water and dissociate into ions i.e. positive an negative ions.
So we can conclude that polar or ionic substances dissociate into ions when dissolved in water.
Learn more about ions here: https://brainly.com/question/14511468
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Which of the following chemical reactions is a decomposition reaction?
2 HgO → 2 Hg + O2
Al + 3 CuCl → AlCl3 + 3 Cu
2 H2 + O2 → 2 H2O
HCl + NaOH → NaCl + H2O
Answer:
2 HgO → 2 Hg + O2
Explanation:
Decomposition is when one reactant breaks down into two or more products due to heat, light or electricity
Here mercury (II) oxide goes through thermal decomposition to make mercury and oxygen
Answer:
2HgO—»2Hg+O_2
Explanation:
The decomposition reaction
It's reaction in which a single reactant gives two or more than two productsHere Mercury oxide gives mercury and oxygen
so option A is decomposition
How many moles of H2SO4 are needed in 0.500m³ of a 0.150M tetraoxosulphate solution?
Answer:
0.015 moles
Explanation:
0.500 m³ of a 0.150 M tetraoxosulphate solution contains 0.075 moles of tetraoxosulphate ions. Since 1 mole of H2SO4 is needed for every 2 moles of tetraoxosulphate ions, then 0.015 moles of H2SO4 are needed.