List of top Chemistry Questions on Thermodynamics asked in VITEEE

The enthalpy change for the reaction \(2\text{C(graphite) + 3\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\) is called:}

Here Z is

In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true?

For the reaction \[ \text{H}_2 \text{(g)} + \frac{1}{2} \text{O}_2 \text{(g)} \rightarrow \text{H}_2 \text{O}(\ell), \Delta H = -285.8 \, \text{kJ/mol}^{-1} \] \text{The value of free energy change at 27°C for the reaction is:}

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at 25°C is:

The values of \( \Delta H \) and \( \Delta S \) for the reaction, \[ \text{C(graphite)} + \text{CO}_2(g) \rightarrow 2\text{CO}(g), \] are 170 kJ and 170 J/K, respectively. This reaction will be spontaneous at:

For the process \( H_2O(g) \, (1 \, \text{bar}, 373 \, \text{K}) \rightarrow H_2O(g) \, (1 \, \text{bar}, 373 \, \text{K}) \), the correct set of thermodynamic parameters is:

A certain reaction is non spontaneous at 298 K. The entropy change during the reaction is 121 J K\(^{-1}\). Is the reaction endothermic or exothermic? The minimum value of \( \Delta H \) for the reaction is

Consider the reaction: \[ \text{N}_2 (g) + 3 \text{H}_2 (g) \rightarrow 2 \text{NH}_3 (g) \] carried out at constant temperature and pressure. If \( \Delta H \) and \( \Delta U \) are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?

Standard entropies of \( X_2 \), \( Y_2 \), and \( X Y_3 \) are 60, 30, and 30 J mol\(^{-1}\) K\(^{-1}\) respectively. For the reaction \[ \frac{1}{2} X_2 + Y_2 \rightarrow X Y_3, \, \Delta H = -30 \, \text{kJ} \] at equilibrium, the temperature should be

The emf of a particular voltaic cell with the cell reaction $Hg_{2}^{2+}+H_{2} {\rightleftharpoons} 2Hg+2H^{+}$ is 0.65 V. The maximum electrical work of this cell when 0.5 g of $H_{2}$ is consumed.

The enthalpy change for a given reaction at 298 K is \( -x \, \text{J mol}^{-1} \). For the reaction to be spontaneous at 298 K, the entropy change at that temperature

A plot of \( \ln K \) against \( 1/T \) (abscissa) is expected to be a straight line with intercept on ordinate axis equal to

Standard entropy of X2, Y2 and X3Y is 60, 40 and 50 J K\(^{-1}\) mol\(^{-1}\), respectively. For the reaction, \[ 1/2 \, \text{X}_2 + 3/2 \, \text{Y}_2 \rightarrow \text{X}_3\text{Y}, \, \Delta H = -30 \, \text{kJ}, \, T = 1250 \, \text{K} \] the equilibrium temperature will be

One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litres. Then \( \Delta S \) (cal deg\(^{-1}\) mol\(^{-1}\)) for this process is: \( R = 2 \, \text{cal K}^{-1} \text{mol}^{-1} \)

A plot of ln K against $\frac{1}{T}$ (abscissa) is expected to be a straight line with intercept on ordinate axis equal

The standard molar heat of formation of ethane, CO2, and water (\( \Delta H_f \)) are respectively -21.1, -94.1, and -68.3 kcal. The standard molar heat of combustion of ethane will be?

The standard molar heat of formation of ethane, $CO_2$ and water are respectively $-21.1, -94.1$ and $-68.3\, kcal$. The standard molar heat of combustion of ethane will be

The equivalent conductivity of a solution containing $2.54\, g$ of $CuSO _{4}$ per $L$ is $91.0\, W ^{-1} cm ^{2} eq ^{-1}$. Its conductivity would be

The reaction of zinc with \( \text{Cu}^{2+} \) produces the following. Entropy change \( \Delta S \) is given by \( 96.5 J \cdot \text{mol}^{-1} \cdot \text{K}^{-1} \).