Calculate value of ′ln(Keq)' for the reaction at 250 K. N2O4(g)⇌2NO2(g) Given: H0f((NO2)g)=+40.407kJ/mol H0f((N2O4)g)=+70kJ/mol S0r=10JK−1
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Q2
For a reaction equilibrium, N2O4(g)→2NO2(g), the concentration of N2O4(g) and NO2 at equilibrium are 4.8×10−2 and 1.2×10−2mol/L respectively.
The value of k for the reaction is:
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Q3
For the reaction equilibrium N2O4(g)⇌2NO2(g) the concentrations of N2O4 and NO2 at equilibrium are 4.8×10−2 and 1.2×10−2molL−1 respectively. The value of Kc for the reaction is
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Q4
For the reaction at equilibrium: N2O4(g)⇌2NO2(g), the concentration of N2O4 and NO2 at equilibrium are 4.8×10−2 and 1.2×10−2 mol/L respectively. The value of Kc for the reaction is:
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Q5
For the reaction at 300K, N2O4(g)⇌2NO2(g), the value of ΔG when concentration of each species is 5 mol/litre will be: