The standard enthalpy of formation (ΔfH°) at 298 K for methane, CH4(g), is –74.8 kJ mol–1. The additional information required to determine the average energy for C–H bond formation would be
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Based on the first law of thermodynamics, which one of the following is correct? |
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Entropy of the universe is |
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The amount of heat evolved when 500 cm3 of 0.1 M HCl is mixed with 200 cm3 of 0.2 M NaOH is ______. |
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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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