List of top Chemistry Questions on Thermodynamics asked in TS EAMCET

Observe the following equation
$H_2O_2(g) \rightarrow 2H(g) + 2O(g)$; $\Delta_a H^\ominus = 1066 \, kJ mol^{-1}$.
If $\Delta_{O-H} H^\ominus$ is $464 \, kJ mol^{-1}$, then $\Delta_{O-O} H^\ominus$ (in $kJ mol^{-1}$) value will be

The $C_p$ of an ideal gas is $10.314 \text{ J} \text{mol}^{-1} \text{K}^{-1}$. One mole of this gas is expanded against a constant pressure of $p \text{ atm}$. The change in temperature during expansion is $1.0 \text{ K}$. The values of $q$ (in J) and $\Delta H$ (in $\text{J} \text{mol}^{-1}$) are respectively

The entropy and enthalpy changes for the reaction \( \text{CO(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \) at 300 K and 1 atm are respectively \(-42.4 \text{ JK}^{-1}\) and \(-41.2 \text{ kJ}\). The temperature at which the reaction will go in the reverse direction is

Which of the following processes are reversible? I. Vaporization of a liquid at its boiling point. II. Expansion of gas into vacuum. III. Transformation of a solid substance into liquid at its melting point. IV. Neutralization of an acid by a base.

At 298 K, the enthalpy change (in kJ) for the reaction given below is: \( \text{CH}_4(g) + \text{O}_2(g) \to \text{C}(s) + 2\text{H}_2\text{O}(l) \) (Given: \( \text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \to \text{H}_2\text{O}(l); \Delta H^\ominus = -286 \text{ kJ} \) \( \text{C}(s) + \text{O}_2(g) \to \text{CO}_2(g); \Delta H^\ominus = -394 \text{ kJ} \) \( \text{CH}_4(g) + 2\text{O}_2(g) \to \text{CO}_2(g) + 2\text{H}_2\text{O}(l); \Delta H^\ominus = -890 \text{ kJ} \))

At 298K, if the standard Gibbs energy change \(\Delta_r G^\circ\) of a reaction is - 115 kJ, the value of \(\log_{10} K_p\) will be (\(R = 8.314 \text{ J K}^{-1}\text{mol}^{-1}\))