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10 Nov 2019

The value of ΔGo for the precipitation reaction,

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

is -48.1 kJ at 298 K.

Calculate the value of ΔG in kJ at 298 K if the concentrations of Ca2+(aq) and
CO32-(aq) are 2.97 and 1.09, M respectively---> please show steps and how you get any ratios (the ans should be -51.01)

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Nelly Stracke
Nelly StrackeLv2
28 Oct 2019

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Related questions

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.

Thevalue ofDGo for the precipitation reaction,

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

is -48.1 kJ at 298 K.

Calculate the value of DG in kJ at 298 K if the concentrationsofCa2+(aq) and
CO32-(aq) are 0.478 and 0.388, Mrespectively.

CORRECT ANSWER: -43.9

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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