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I am having a heck of a time understanding these. If you could explain the steps...

I am having a heck of a time understanding these. If you could explain the steps that would be wonderful!

a. If the reaction above (c) were conducted at 273K with [NH4+] = 0.34M and [NO3-] = 0.12M, what would be the value of ΔG? Would the reaction be spontaneous in the forward or reverse direction?

b. Should CrCl3 be more soluble in a solution buffered at pH = 5.5 or pH = 9.5, given that it forms the complex ion Cr(OH)4-? (explain please).

c. Given the information below, determine values for ΔH°, ΔS°, and ΔG°. Is this reaction spontaneous in the forward direction (from standard state)? Which piece of information tells you this? NH4NO3(s) → NH4+(aq) + NO3-(aq)

ΔHf° (kJ/mol)

ΔS° (J/molK)

NH4NO3(s)

-365.56

151.08

NH4+(aq)

-132.51

113.4

NO3-(aq)

-205.0

146.4
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Answer #1

I have done part c first as i have to find the standard enthalpy and entropy first and from this I determined stnd Gibbs free energy and then from this I solved part (a)

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