JEE MAIN - Chemistry (2021 - 17th March Evening Shift - No. 17)
Consider the reaction
$$N_{2}O_{4}\left( g\right) \rightleftharpoons 2NO_{2}\left( g\right) $$
The temperature at which KC = 20.4 and KP = 600.1, is ____________ K. (Round off to the Nearest Integer). [Assume all gases are ideal and R = 0.0831 L bar K$$-$$1 mol$$-$$1]
$$N_{2}O_{4}\left( g\right) \rightleftharpoons 2NO_{2}\left( g\right) $$
The temperature at which KC = 20.4 and KP = 600.1, is ____________ K. (Round off to the Nearest Integer). [Assume all gases are ideal and R = 0.0831 L bar K$$-$$1 mol$$-$$1]
Answer
354
Explanation
N2O4(g) $$\rightleftharpoons$$ 2NO2(g)
$$\Delta$$ng = 2 $$-$$ 1 = 1
KP = KC(RT)$$\Delta$$ng
600.1 = 20.4 (0.0831 $$\times$$ T)1
$$ \Rightarrow $$ T = $${{600.1} \over {20.4 \times 0.0831}}$$ = 354 K
$$\Delta$$ng = 2 $$-$$ 1 = 1
KP = KC(RT)$$\Delta$$ng
600.1 = 20.4 (0.0831 $$\times$$ T)1
$$ \Rightarrow $$ T = $${{600.1} \over {20.4 \times 0.0831}}$$ = 354 K
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