The diagram that best shows the major type of attractive force that exists between the particles in the solution is diagram B which shows hydrogen bonding.
The coreect ansdwer is B.
What is hydrogen bonding?Hydrogen bonding is a type of intermolecular bonding that occurs between hydrogen atoms that are bonded to strongly electronegative elements like oxygen, chlorine, fluorine, and nitrogen.
Due to the stronger attraction of the electronegative elements to the shared electron pair, the electronegative element acquires a partial negative charge while the hydrogen atom acquires a partial negative charge. This uneven charge distribution results in the atoms of hydrogen being attracted to the atoms of the electronegative elements of neighboring molecules, thus producing hydrogen bonding.
Hydrogen bonding exists in water as well as in methanol. The dissolution of methanol in water is due to the hydrogen bonds formed between the molecules
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Using the following standard reduction potentials,
Fe3+(aq) + e- →Fe2+(aq) E° = +0.77 V
Ni2+(aq) + 2 e- →Ni(s) E° = -0.23 V
calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions.
Ni2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Ni(s)
a) E° = -1.00 V, spontaneous
b) E° = +1.00 V, nonspontaneous
c) E° = +1.00 V, spontaneous
d) E° = -1.00 V, nonspontaneous
d) E° = -1.00 V, nonspontaneous is the correct answer.
Regarding the specified chemical reaction:
[tex]Ni^{2+}(aq.) + 2Fe^{2+}(aq.)[/tex] → [tex]2Fe^{3+} (aq.) + Ni(s)[/tex]
In this case, iron is being oxidized because it is losing electrons, whereas nickel is being reduced because it is receiving electrons.
We know that:
[tex]E^{0}_{(Fe^{3+}/Fe^{2+})} = 0.77V[/tex]
[tex]E^{0}_{(Ni^{2+}/Ni)} = -0.23V[/tex]
The substance that is being oxidized acts as the cathode and the substance that is being reduced acts as the anode.
We use the equation to determine the reaction [tex]E^{0}_{cell}[/tex].
[tex]E^{0}_{cell} = E^{0}_{cathode} - E^{0}_{anode}[/tex]
[tex]E^{0}_{cell} = -0.23-0.77= -1.0 V[/tex]
The following shows how standard electrode potential and standard Gibbs free energy relate:
Δ[tex]G^{0} = -nFE^{0}_{cell}[/tex]
The standard electrode potential of the cell for the mentioned cell is negative. As a result, the reaction's standard Gibbs free energy change will become positive, making it non-spontaneous.
So, the mentioned response is non-spontaneous.
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A compound is found to contain 26.73 % phosphorus, 12.09 % nitrogen, and 61.18 % chlorine by mass. What is the molecular
formula for this compound
The Molecular formula for this compound would be [tex]N{6} Cl{12} P{6}[/tex]
What is Molecular formula?The molecular formula is described as an expression that defines the number of atoms of each element in one molecule of a compound
The first step is to find out how many grams of each element are in one mole of the compound.
We do this because we have the molar mass of the compound, as well as the percent mass of each element.
695g * 26.73% = 186g of Phosphorous/mol of compound.
695g * 12.09% = 84g of Nitrogen/mol of compound.
695g * 61.18% = 425g of Chlorine/mol of Compound.
Because we know how many grams of each element are present per mole of compound, we can use the molar masses of each element to find out how many moles of each element are present per mole of the compound.
186g P * (1mole P/30.1g) = 6 moles of Phosphorous.
84g N * (1mole N/14g) = 6 moles of Nitrogen.
425g Cl * (1mole/35g) = 12 moles of Chlorine.
Therefore, the molecular formula for this compound would be [tex]N{6} Cl{12} P{6}[/tex]
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