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11 Dec 2019

The value of ?Go for the precipitation reaction,

Ca2+(aq) + CO32-(aq) <=>CaCO3(s)

is -48.1 kJ at 298 K.

Calculate the value of ?G in kJ at 298 K if the concentrationsof Ca2+(aq) and
CO32-(aq) are 0.815 and 0.406, Mrespectively.

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Deanna Hettinger
Deanna HettingerLv2
13 Dec 2019

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Related questions

The correct complete ionic equation for the reaction that occurs when aqueous solutions
of Ca(NO3)2 and Na2CO3 are mixed is

a) Ca(NO3)2(aq) + Na2CO3(aq) Ã CaCO3(s) + 2 NaNO3(aq)

b) Ca2+ (aq) + 2 NO3- (aq) + 2Na+ (aq) + CO32- (aq) Ã CaCO3(s) + 2 Na+ (aq) + 2 NO3- (aq)

c) Ca2+ (aq) + 2 NO3- (aq) + 2Na+ (aq) + CO32- (aq) Ã Ca2+(aq) + CO32- (aq) + 2 NaNO3(s)

d) Ca2+ (aq) + CO32- (aq) Ã CaCO3(s)

e) Na+ (aq) + NO3- (aq) Ã NaNO3(s)

Calculate K at 298 K for each reaction:

a. MgCo3 (s) <-----> Mg2+ (aq) + Co32- (aq)

b. 2HCl (g) + Br2 (l) <----> 2HBr (g) + Cl2 (g)

c. H2 (g) + O2 (g) <---> H2O2 (l)

Limestone stalactites and stalagmites are formed in caves by the following reaction: Ca2+(aq)+2HCO−3(aq)→CaCO3(s)+CO2(g)+H2O(l) If 1 mol of CaCO3 forms at 298 K under 1 atm pressure, the reaction performs 2.49 kJ of P−V work, pushing back the atmosphere as the gaseous CO2 forms. At the same time, 38.95 kJ of heat is absorbed from the environment.

1. What is the value of ΔH for this reaction? Express your answer using four significant figures.

2. What is the value of ΔE for this reaction? Express your answer using four significant figures.

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