Answer:
7.16 × 10⁻³ M
Explanation:
Let's consider the reduction reaction of copper during the electroplating.
Cu²⁺(aq) + 2 e⁻ ⇒ Cu(s)
We can calculate the moles of Cu²⁺ present in the solution using the following relations.
1 A = 1 C/s.1 min = 60 s.1 mole of electrons has a charge of 96486 C (Faraday's constant).1 mole of Cu²⁺ is reduced when 2 moles of electrons are gained.The moles of Cu²⁺ reduced are:
[tex]2.30 min \times \frac{60s}{1min} \times \frac{3.00C}{s} \times \frac{1mole^{-} }{96486C} \times \frac{1molCu^{2+} }{2mole^{-} } = 2.15 \times 10^{-3} molCu^{2+}[/tex]
[tex]2.15 \times 10^{-3} moles[/tex] of Cu²⁺ are in 0.300 L of solution.
[Cu²⁺] = 2.15 × 10⁻³ mol/0.300 L = 7.16 × 10⁻³ M
What's 2+7 hehdhenbeidbnejdbdbdbdi
Answer:
Answer
9......
Explanation:
Explaination:
Copper metal has a specific heat of 0.385 J/g.C. calculate the amount of heat required to raise the temperature of 22.8g of copper metal from 20.0C to 875°C
Answer:
7505.19 J
Explanation:
We'll begin by calculating the change in the temperature of copper. This can be obtained as follow:
Initial temperature (T₁) = 20 °C
Final temperature (T₂) = 875 °C
Change in temperature (ΔT) =?
ΔT = T₂ – T₁
ΔT = 875 – 20
ΔT = 855 °C
Finally, we shall determine the heat required. This can be obtained as follow:
Specific heat capacity (C) = 0.385 J/gºC
Change in temperature (ΔT) = 855 °C
Mass (M) = 22.8 g
Heat (Q) required =?
Q = MCΔT
Q = 22.8 × 0.385 × 855
Q = 7505.19 J
Thus, 7505.19 J of heat energy is required.
what elements don't form bonds
Answer:
Noble gases are a set of elements in the periodic table because they don't naturally bond with other elements. *Examples ...Helium; Neon; Radon; Xenon; Argon etc
Explanation:
theyre noble gases.
Fire a single electron towards the hydrogen atom. Describe what happens in a step by step fashion. [N.B. - It may be helpful to utilize the Run in Slow Motion option for this part.]
Answer:
The electrons will be added by the hydrogen.
Explanation:
If we fire a single electron towards the hydrogen atom, the hydrogen atoms added the electron to its shell by applying force of attraction and becomes stable as well as non reactive in nature because the hydrogen attains the electronic configuration of helium which is a noble gas and have completed its outermost shell. The proton that is present in the nucleus attracts this electron and compel it to add in the electron.
Name the subatomic parts of the atom, their charges and where they are located.
Answer:
protons: positively charged, located in the nucleus
electrons: negatively charged, located outside the nucleus
neutrons: no charge, located in the nucleus
8. What does the term 'sustainable mean? *
Answer:
something that can be maintained over a period of time
Answer:
a balance between meeting today's needs.......
Explanation:
Which of the choices below has more heat being transferred as thermal energy from one place to another?
A. A bowl of ice water
B. A pot of boiling water
Answer:
B
Explanation:
So, a pot of boliling is hot right? of course, since it is hot thermal energy will be transferred from one place to another. I don't know if this is correct but I just wanted to give it a try.
You deserve 0.72G of potassium chloride (KCI) in 600 ml of water. What is the molarity of the solution ?
Answer:
0.016 M
Explanation:
Molarity refers to the molar concentration of a solution and it can be calculated using the formula below:
Molarity (M) = number of moles (n) ÷ volume (V)
According to this question, the mass of KCl was given to be 0.72 grams and the volume of water as 600 mL.
Using mole = mass/molar mass to convert mass of KCl to moles
Molar mass of KCl = 39 + 35.5 = 74.5g/mol
mole = 0.72g ÷ 74.5g/mol
mole = 0.00966mol
Volume of water = 600mL = 600/1000 = 0.600L
Molarity, M = 0.00966 ÷ 0.600
Molarity of KCl solution = 0.016 M
In what form is energy that is NOT used for life processes released from living things?
1. Thermal energy
2. Chemical energy
3. Light energy
4. Sound energy
Answer:
Correct answer would be Option 2, Chemical Energy
Hope this helps!
To run a spectrophotometry experiment, begin by _______ the spectrophotometer and preparing the samples. Be sure to select the correct ________, then run a measurement on the _______ solution. Follow up by running measurements on _______ solutions. Once data is collected, turn off the instrument, clean the area, and discard the samples.
1.
a) cleaning
b) warming up
c) unplugging
2.
a) wavelength
b) transmittance
c) absorbance
3.
a) blank
b) aqueous
c) sample
4.
a) blank
b) aqueous
c) sample
Answer:
b) warming up a) wavelength a) blank c) sample
Explanation:
To run a spectrophotometry experiment, begin by warming up the spectrophotometer and preparing the samples. It is important that the equipment is warmed up for at least 30 minutes before starting the measurements.
Be sure to select the correct wavelength, then run a measurement on the blank solution. The selected wavelength depends on the analyte of interest. The black solution contains the same matrix but it doesn´t contain the analyte.
Follow up by running measurements on sample solutions. Once data is collected, turn off the instrument, clean the area, and discard the samples. The samples are those of unknown concentration that we want to determine.
To run a spectrophotometry experiment, begin by cleaning the spectrophotometer and preparing the samples. Be sure to select the correct wavelength, then run a measurement on the sample solution. Follow up by running measurements on aqueous solutions. Once data is collected, turn off the instrument, clean the area, and discard the samples.
Spectrophotometry is a technique used to measure the interaction of light with matter, specifically the absorption, transmission, or reflection of light by a sample. It involves the use of a spectrophotometer, an instrument that measures the intensity of light as a function of its wavelength or frequency.
In spectrophotometry, a sample is exposed to light of a specific wavelength or a range of wavelengths. The sample may absorb certain wavelengths of light, which can be detected and measured by the spectrophotometer. The amount of light absorbed is related to the concentration of the analyte in the sample, allowing for quantitative analysis.
Learn more about Spectrophotometry, here:
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Which of the following is a testable hypothesis
Answer:
C
Explanation:
Answer:
C.
Explanation:
Brainiest?
What is the molarity if 6664 grams of boron iodide is dissolved in 5.25 liters of water?
Answer:
3.24 mol/L
Explanation:
Given that:
mass of Boron triiodide = 6664 grams
molar mass of BI_3 = 391.52 g/mol
Recall that:
number of moles = mass/molar mass
∴
number of moles = 6664 g /391.52 g/mol
number of moles = 17.02 mol
Also;
Molarity = moles for solute/liter for solution
= 17.02 mol/5.25 L
= 3.24 mol/L
True or false? An organism may play more than one role in a food web
Answer:
True
Explanation:
Your welcome! :) Good luck!
I want to know which ones are molecular equation, complete ionic equation and net ionic equation
Answer:
The molecular equations are:
1. CuSO₄ (aq) + 2 KOH (aq) ----> Cu(OH)₂ (s) + K₂SO₄ (aq)
2. Ba(NO₃)₂ (aq) + K₂SO₄ (aq) + BaSO₄ (s) + 2 KNO₃ (aq)
The complete ionic equations are:
1. Ag + (aq) + NO₃- (aq) + I- (aq) + Na (aq) ---> AgI (s) + No₃- (aq) + Na+ (aq)
2. Cu²+ + SO₄²- (aq) + 2 K+ (aq) + 2 OH- (aq) ---> Cu(OH)₂ (s) + 2K+ (aq) + SO₄²- (aq)
The net ionic equations are:
1. Ca²+ (aq) + SO₄²- (aq) ---> CaSO₄ (s)
2. Ba²+ (aq) +SO₄²- (aq) ---> BaSO₄ (s)
Explanation:
A molecular equation is a balanced chemical equation which shows the reacting species as molecules rather than as componenet ions in their compounds with subscripts written beside the molecules to indicate the state in which they occur in the chemical reaction.
An ionic equation expresses the reacting species as components ions in a chemical reation. All the ions and molecules reacting are shown.
In a net ionic equation, the ions which remain in the ionic state also known as spectator ions are not written as part of the equation.
From the given attachment;
The molecular equations are:
1. CuSO₄ (aq) + 2 KOH (aq) ----> Cu(OH)₂ (s) + K₂SO₄ (aq)
2. Ba(NO₃)₂ (aq) + K₂SO₄ (aq) + BaSO₄ (s) + 2 KNO₃ (aq)
The complete ionic equations are:
1. Ag + (aq) + NO₃- (aq) + I- (aq) + Na (aq) ---> AgI (s) + No₃- (aq) + Na+ (aq)
2. Cu²+ + SO₄²- (aq) + 2 K+ (aq) + 2 OH- (aq) ---> Cu(OH)₂ (s) + 2K+ (aq) + SO₄²- (aq)
The net ionic equations are:
1. Ca²+ (aq) + SO₄²- (aq) ---> CaSO₄ (s)
2. Ba²+ (aq) +SO₄²- (aq) ---> BaSO₄ (s)
14. Which block in the periodic table contains the metalloids?
O A. p block
OB. s block
O C. d block
D. f block
Answer
the answer is p block
so de fanga gu se si gage humang we sapa shata phoni we heo sang pai
Answer:
Which language is this???
Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3 (aq) Na2SO4 (aq) --> Ag2SO4 (s) 2 NaNO3 (aq) If 3.80 moles of AgNO3 and 3.05 moles of Na2SO4 are present initially, how many moles of excess reactant will remain after precipitation is complete
Answer:
1.15 moles of excess reactant will remain after precipitation is complete.
Explanation:
The balanced reaction is:
2 AgNO₃ (aq) + Na₂SO₄ (aq) → Ag₂SO₄ (s) + 2 NaNO₃ (aq)
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:
AgNO₃: 2 molesNa₂SO₄: 1 moleAg₂SO₄: 1 moleNaNO₃: 2 molesThen you can apply the following rule of three:: if by stoichiometry 2 moles of AgNO₃ reacts with 1 mole of Na₂SO₄, 3.80 moles of AgNO₃ reacts with how much moles of Na₂SO₄?
[tex]amount of moles of Na_{2}SO_{4} =\frac{1mole of Na_{2}SO_{4} * 3.80 moles of AgNO_{3} }{2 mols of AgNO_{3} }[/tex]
amount of moles of Na₂SO₄= 1.9 moles
But 3.05 moles of Na₂SO₄ are available. Since you have more moles than you need to react with 3.80 moles of AgNO₃, Na₂SO₄ will be the excess reagent.
To calculate the amount of excess reagent that will remain, you must make the difference between the amount you initially have and the amount that reacts:
3.05 moles - 1.9 moles= 1.15 moles
1.15 moles of excess reactant will remain after precipitation is complete.
How many moles of electrons must be transferred to plate out 110 g of manganese (MW ~ 55g/mol) from a solution of permanganate (MnO4-)
Answer:
14 mol e⁻
Explanation:
Step 1: Write the balanced half-reaction for the reduction of permanganate to manganese
8 H⁺(aq) + 7 e⁻ + MnO₄⁻(aq) ⇒ Mn(s) + 4 H₂O(l)
Step 2: Calculate the moles corresponding to 110 g of manganese
The molar mass of Mn is 55 g/mol.
110 g × 1 mol/55 g = 2 mol
Step 3: Calculate the number of moles of electrons needed to produce 2 moles of Mn
According to the half-reaction, 7 moles of electrons are required to produce 1 mole of Mn.
2 mol Mn × 7 mol e⁻/1 mol Mn = 14 mol e⁻
Helpppp
What is the volume of 2.99 moles of C3H8 at STP?
0.0680L
5.87 L
ОООО
1.52 L
67.0L
Answer:
67.0 L
Explanation:
Step 1: Given data
Moles of C₃H₈: 2.99 molPressure: 1 atm (standard pressure)Temperature: 273.15 K (standard temperature)Step 2: Calculate the volume occupied by 2.99 moles of C₃H₈ at STP
C₃H₈ is a gas. If we assume ideal behavior, 1 mole of C₃H₈ at STP occupies 22.4 L.
2.99 mol × 22.4 L/1 mol = 67.0 L
Calculate the number of milliliters of 0.587 M NaOH required to precipitate all of the Fe3 ions in 197 mL of 0.654 M FeCl3 solution as Fe(OH)3. The equation for the reaction is: FeCl3(aq) 3NaOH(aq) Fe(OH)3(s) 3NaCl(aq)
Answer: The number of milliliters of 654 mL for 0.587 M NaOH required to precipitate all of the [tex]Fe^{3+}[/tex] ions in 197 mL of 0.654 M [tex]FeCl_{3}[/tex] solution as [tex]Fe(OH)_{3}[/tex].
Explanation:
The reaction equation is as follows.
[tex]FeCl_{3}(aq) + 3NaOH(aq) \rightarrow Fe(OH)_{3}(s) + 3NaCl(aq)[/tex]
Therefore, moles of [tex]Fe(OH)_{3}[/tex] are calculated as follows.
Moles = Molarity of [tex]Fe(OH)_{3}[/tex] [tex]\times[/tex] Volume (in L)
= 0.654 M [tex]\times[/tex] 0.197 L
= 0.128 mol
Now, according to the given balanced equation 1 mole of [tex]FeCl_{3}(aq)[/tex] reacts with 3 moles of NaOH(aq). Hence, moles of [tex]Fe(OH)_{3}[/tex] reacted are calculated as follows.
3 [tex]\times[/tex] 0.128 mol = 0.384 moles of NaOH
As moles of NaOH present are as follows.
Moles of NaOH = Molarity of NaOH [tex]\times[/tex] Volume (in L)
0.384 mol = 0.587 M [tex]\times[/tex] Volume (in L)
Volume (in L) = 0.654 L (1 L = 1000 mL) = 654 mL
Thus, we can conclude that the number of milliliters of 654 mL for 0.587 M NaOH required to precipitate all of the [tex]Fe^{3+}[/tex] ions in 197 mL of 0.654 M [tex]FeCl_{3}[/tex] solution as [tex]Fe(OH)_{3}[/tex].
163 mL of 2.75 mol/L aluminum sulfate is to have all aluminum ions removed by adding a 3.65 mol/L sodium sulfide solution.
Al2(SO4)3(aq) + 3 Na2S(aq) → Al2S3(s) + 3 Na2SO4(aq)
What is the minimum volume of sodium sulfide that must be added to completely remove all the aluminum ions? What mass of aluminum sulfide will form?
Answer:
[tex]V_{Na_2S}=368mL[/tex]
[tex]m_{Al_2S_3}=67.3gAl_2S_3[/tex]
Explanation:
Hello there!
In this case, according to the given information, it is possible to realize that the only way for us to calculate the required volume of sodium sulfide, is by calculating the moles of this substance consumed 163 mL of 2.75 mol/L aluminum sulfate by using the definition of molar concentration and the 1:3 mole ratio between these two:
[tex]n_{Na_2S}=0.163L*2.75\frac{molAl_2(SO_4)_3}{L}*\frac{3molNa_2S}{1molAl_2(SO_4)_3} =1.34molNa_2S[/tex]
Now, we divide these moles by the molar concentration of sodium sulfide to obtain the required volume:
[tex]V_{Na_2S}=\frac{1.34molNa_2S}{3.65mol/L} =0.368L=368mL[/tex]
For the last part, we now use the 1:1 mole ratio of aluminum sulfate to aluminum sulfide and the molar mass of the latter (150.158 g/mol) in order to calculate the required mass:
[tex]m_{Al_2S_3}=0.163L*2.75\frac{molAl_2(SO_4)_3}{L}*\frac{1molAl_2S_3}{1molAl_2(SO_4)_3} *\frac{150.158gAl_2S_3}{1molAl_2S_3} \\\\m_{Al_2S_3}=67.3gAl_2S_3[/tex]
Regards!
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What are the characteristics of ionic compounds?
Answer:
the characteristics of ionic compounds are :
1.They form crystals.
2.They are hard and brittle.
Answer:
they form crystals.
they have high melting and boiling points.
they are hard and brittle.
they are good insulators.
when dissolve in water...they dissociate Into ions.
classify the following compounds as chiral, achiral (but not meso), or meso. 1st structure: _________ 2nd structure: _________ 3rd structure: _________
Answer:
1st structure - Meso
2nd structure - Chiral
3rd structure - achiral
Explanation:
In the 1st structure there is nitrogen atom bonded with 4 different groups. It is Meso compound. In the second structure a carbon atom is attached with hydroxide molecule OH and has four different environment. It is Chiral compound. In the third structure no atom have different atom or group surrounding it. Therefore it is Achiral compound.
What is the limiting reagent when 22 g of sodium is added to 28 g water?
Answer:
Limiting reagent is Na
Explanation:
Reaction of Na with water is:
Na + H₂O → NaOH + H₂
It is a very exothermic reaction.
The correctly balanced equation is:
2Na + 2H₂O → 2NaOH + H₂
Ratio is 2:2, between reactants, according to stoichiometry.
We convert mass to moles:
22 g . 1 mol / 23 g = 0.956 moles of Na
28 g . 1mol / 18 g = 1.56 moles of water.
Certainly the limiting reagent is sodium. For 1.56 moles, we need the same amount of sodium and we only have 0.956 moles.
We do not have enough sodium to complete the reaction.
Of the below gases, which would deviate most from ideal gas behavior? CO O2 NH3 SF4
Answer:
For gases such as hydrogen, oxygen, nitrogen, helium, or neon, deviations from the ideal gas law are less than 0.1 percent at room temperature and atmospheric pressure. Other gases, such as carbon dioxide or ammonia, have stronger intermolecular forces and consequently greater deviation from ideality.
Explanation:
2. Energy cycles through ecosystems because it returns to the sun.
True or false
Please help I will give 50 points
Answer:
false
Explanation:
energy does not return to the sun, it returns to the plants or producers. if energy were to return to the sun, it would have to travel though space.
A 1.0 g sample of propane, C3H8, was burned in calorimeter. The temperature rose from 28.5 0C to 32.0 0C and heat of combustion 10.5 kJ/g. Calculate the heat capacity of the calorimeter apparatus in kJ/0C
Answer:
A 1.0 g sample of propane, C3H8, was burned in the calorimeter.
The temperature rose from 28.5 0C to 32.0 0C and the heat of combustion 10.5 kJ/g.
Calculate the heat capacity of the calorimeter apparatus in kJ/0C
Explanation:
[tex]Heat of combustion = heat capacity of calorimeter * deltaT\\[/tex]
Given,
The heat of combustion = 10.5kJ/g.
[tex]deltaT = (32.0-28.5)^oC\\deltaT = 3.5^oC[/tex]
Substitute these values in the above formula to get the value of heat capacity of the calorimeter.
[tex]deltaT =heat capacity of calorimeter * (change in temperature)\\10.5kJ/g = heat capacity of calorimeter * (3.5^oC)\\\\=>heat capacity of calorimeter = \frac{10.5kJ/g}{3.5^oC} \\=>heat capacity of calorimeter = 3.0 kJ/g.^oC[/tex]
Answer:
The heat capacity of the calorimeter is [tex]3.0kJ/g.^oC.[/tex]
The temperature of a sample of silver increased by 23.8 °C
when 261 J of heat was applied.
What is the mass of the sample?
Answer:
46.67 g
Explanation:
From the question given above, the following data were obtained:
Change in temperature (ΔT) = 23.8 °C
Heat (Q) = 261 J
Specific heat capacity (C) of silver = 0.235 J/gºC
Mass of silver (M) =?
The mass of the sample of silver can be obtained as follow:
Q = MCΔT
261 = M × 0.235 × 23.8
261 = M × 5.593
Divide both side by 5.593
M = 261 / 5.593
M = 46.67 g
Thus, the mass of the sample of silver is 46.67 g
Which substance has Delta.Hf defined as 0 kJ/mol? H2O (s) Ne (l) F2 (g) CO2 (g)
Answer:
F2 (g)
Explanation:
Edg 2021
Answer:
F2 g
Explanation: