Calculate Delta_{r} G^{ominus} for the conver | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The relationship between standard Gibbs free energy change and the equilibrium constant is given by the formula: $\Delta_{r} G^{\ominus} = -RT \ln

Vedclass · Accepted Answer

$163 \, kJ \, mol^{-1}$

Vedclass · Answer

(A) The relationship between standard Gibbs free energy change and the equilibrium constant is given by the formula: $\Delta_{r} G^{\ominus} = -RT \ln K_{p} = -2.303 \, RT \log K_{p}$.Given values are $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,$T = 298 \, K$,and $K_{p} = 2.47 	imes 10^{-29}$.Substituting these values into the equation:$\Delta_{r} G^{\ominus} = -2.303 	imes (8.314 \, J \, K^{-1} \, mol^{-1}) 	imes (298 \, K) 	imes \log(2.47 	imes 10^{-29})$.$\Delta_{r} G^{\ominus} = -2.303 	imes 8.314 	imes 298 	imes (\log 2.47 + \log 10^{-29})$.$\Delta_{r} G^{\ominus} = -5705.85 	imes (0.3927 - 29)$.$\Delta_{r} G^{\ominus} = -5705.85 	imes (-28.6073) \approx 163229 \, J \, mol^{-1}$.Converting to $kJ \, mol^{-1}$,we get $\Delta_{r} G^{\ominus} \approx 163 \, kJ \, mol^{-1}$.

Calculate $\Delta_{r} G^{\ominus}$ for the conversion of oxygen to ozone,$\frac{3}{2} O_{2(g)} \rightarrow O_{3(g)}$ at $298 \, K$,if $K_{p}$ for this conversion is $2.47 \times 10^{-29}$.

Similar Questions

At $227^{\circ} C$,dinitrogen tetraoxide is $60 \%$ dissociated. What is the standard free energy change at this temperature and at $1 \ atm$ pressure?

Assertion: For every chemical reaction at equilibrium,the standard Gibbs energy change is zero.
Reason: At constant temperature and pressure,a chemical reaction is spontaneous in the direction of decreasing Gibbs energy.

For the reaction $A \rightleftharpoons B$,find the value of $log_{10}K$. Given: $\Delta_rH^o_{298\,K} = -54.07\, kJ\, mol^{-1}$,$\Delta_rS^o_{298\,K} = 10\, J\, K^{-1}\, mol^{-1}$,$R = 8.314\, J\, K^{-1}\, mol^{-1}$,$2.303 \times 8.314 \times 298 = 5705$.

For the reversible reaction,$A_{(s)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$,$\Delta G^{\circ} = -350 \ kJ$,which one of the following statements is true?

If the equilibrium constant of a process is $3.8 \times 10^{-3}$ at $25^{\circ} C$, what is the standard free energy change of the process? $(R = 8.314 \ J \ mol^{-1} \ K^{-1}, \log 0.0038 = -2.42)$

Vedclass Test Series

Exam Paper Generator

Online Exam Module