Identify the correct statement from the following in a chemical reaction.
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The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is |
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The species which by definition has ZERO standard molar enthalpy of formation at 298 K is |
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One mole of which of the following has the highest entropy? |
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Consider the reaction : 4NO2(g) + O2(g) ⟶ 2N2O5(g), ΔrH = –111 kJ. If N2O5(s) is formed instead of N2O5(g) in the above reaction, the ΔrH value will be: |
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For a particular reversible reaction at temperature T, ΔH and ΔS were found to be both +ve. If Te is the temperature at equilibrium, the reaction would be spontaneous when |
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In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298.0 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is 2.5 kJ K–1, the numerical value for the enthalpy of combustion of the gas in kJ mol–1 is |
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In which of the following process, a maximum increase in entropy is observed? |
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The enthalpy of vaporization of benzene is +35.3 kJ/mol at its boiling point of 80°C. The entropy change in the transition of vapour to liquid at its boiling point is ______. (in J mol–1 K–1) |
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ΔHvap = 30 KJ/mole and ΔSvap = 75 Jmol–1K–1. Find temperature of vapour, at one atmosphere |
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Standard entropy of X2, Y2 and XY3 are 60, 40 and 50 JK–1mol–1, respectively. For the reaction, $\dfrac{1}{2}$X2 + $\dfrac{3}{2}$Y2 → XY3, ΔH = –30 kJ, to be at equilibrium, the temperature will be |
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