The equilibrium constant for the reaction AgBr(s) $The equilibrium constant for the reaction AgBr(s) Ag+(aq)+ Br- (aq)is the solubility product constant, Ksp = 7.7 \times 10-13 at 25°C. Calculate \Delta G for the reaction when [Ag+] = 1.0 \times 10-2 M and [Br-] = 1.0 \times 10-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? A)( \Delta G = 69.1 kJ/mol, nonspontaneous) B)( \Delta G = -69.1 kJ/mol, spontaneous) C)( \Delta G = 97.5 kJ/mol, spontaneous) D)( \Delta G = 40.6 kJ/mol, nonspontaneous) E)( \Delta G = -97.5 kJ/mol, nonspontaneous)$ Ag⁺(aq)+ Br^-(aq)is the solubility product constant, K_sp = 7.7

\times

10^-13 at 25°C. Calculate

\Delta

G for the reaction when [Ag⁺] = 1.0

\times

10^-2 M and [Br^-] = 1.0

\times

10^-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations?
A)(

\Delta

G = 69.1 kJ/mol, nonspontaneous)
B)(

\Delta

G = -69.1 kJ/mol, spontaneous)
C)(

\Delta

G = 97.5 kJ/mol, spontaneous)
D)(

\Delta

G = 40.6 kJ/mol, nonspontaneous)
E)(

\Delta

G = -97.5 kJ/mol, nonspontaneous)

Given the Following Data, Estimate the Boiling Point of Carbon Δ\DeltaΔ

Short Answer

Correct Answer:VerifiedUnlock this answer nowGet Access to more Verified Answers free of chargeAccess For Free

Given the Following Data, Estimate the Boiling Point of Carbon $\Delta$

Correct Answer:
Verified
Unlock this answer now
Get Access to more Verified Answers free of charge