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  • The following reaction is performed at 298 K .         2NO(g) + O2 (g) <img alt="\rightleftharpoons" src="https://entrancecorner.oncodec

The following reaction is performed at 298 K .

        2NO(g) + O2 (g) \rightleftharpoons 2NO2 (g)  

The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. 

What is the standard free energy of formation of NO2(g) at 298 K ?    \left ( K_{p}= 1.6\times 10^{12} \right )

 

Option: 1

R(298)\: ln(1.6\times 10^{12})-86600


Option: 2

86600+R(298)\: ln (1.6\times 10^{12})


Option: 3

86600-\frac{ln (1.6\times 10^{12})}{R(298)}


Option: 4

0.5\left [ 2\times 86,600-R(298)ln(1.6\times 10^{12}) \right ]


Answers (1)

best_answer

As we learnt in 

2NO(g)+O_{_{2}}\left ( g \right )\leftrightharpoons 2NO_{2}(g)

Given that \Delta G_{f^{0}} (NO)= 86.6 kj mol ^{-1}

and we know that \Delta G_{f^{\circ}} (O_{2})= 0

K=1.6 \times 10^{12}

\Delta -RT ln k=2\Delta G_{f^{\circ}} (NO_{2})-\left [ 2 \times 86600+0 \right ]

\Delta G_{f^{\circ}} (NO_{2})=0.5 \left [ 2 \times 86600-R (298) ln (1.6X10^{12})\right ]

 

Posted by

mansi

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