Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g) ? 2NO2(g) ?rHº= 57.24 kJ/mol At 298K, a reaction vessel initially contains 0.100 bar of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 388K? Assume that the initial pressure of N2O4 is the same (0.100 bar).
Please explain how you would go about solving this problem. Thanks you.