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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The temperature of the system decreases in an ______. |
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Which of the following is an intensive property? |
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The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm3 to a volume of 100 dm3 at 27°C is |
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The Gibbs energy for the decomposition of Al2O3 at 500°C is as follows: $\dfrac{2}{3}$Al2O3 → $\dfrac{4}{3}$Al + O2, ΔrG = +966 kJ mol–1 The potential difference needed for electrolytic reduction of Al2O3 at 500°C is at least |
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For the reversible reaction, A(s) + B(g) ⇌ C(g) + D(g), ΔG° = –350kJ which one of the following statements is true? |
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