List of top Chemistry Questions on Thermodynamics asked in TS EAMCET

$\Delta H$ and $\Delta S$ for the reaction, $2A+B \rightarrow C$ at 298 K are $400~kJ~mol^{-1}$ and $2~kJ~K^{-1}mol^{-1}$ respectively. At or above $T(K)$, the reaction becomes spontaneous. What is $T(K)$?

In which of the following reactions \(\Delta S\) (entropy change) is positive?

Identify sets with only extensive or only intensive properties.

What is the enthalpy change (in $kJ~mol^{-1}$) for the following reaction? \[ CCl_4(g)\rightarrow C(g)+4Cl(g) \]

The $\Delta_f\text{H}^\ominus$ of $\text{BaCO}_3\text{(s)}$, BaO(s) and $\text{CO}_2\text{(g)}$ is respectively $-1216.3$, $-553.5$ and $-393.5\text{ kJ mol}^{-1}$. What is the value of $x$ (in $\text{kJ mol}^{-1}$) in the following reaction? \[ \text{BaCO}_3\text{(s)} \xrightarrow{\Delta} \text{BaO(s)}+\text{CO}_2\text{(g)}-x \]

The $\Delta_f\text{H}^\ominus$ of $\text{BaCO}_3\text{(s)}$, BaO(s) and $\text{CO}_2\text{(g)}$ is respectively $-1216.3$, $-553.5$ and $-393.5\text{ kJ mol}^{-1}$. What is the value of $x$ (in $\text{kJ mol}^{-1}$) in the following reaction? \[ \text{BaCO}_3\text{(s)} \xrightarrow{\Delta} \text{BaO(s)}+\text{CO}_2\text{(g)}-x \]

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.

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

At T(K) 10 L of an ideal gas was expanded to 12 L against a pressure of 2 atm irreversibly. What is the work done by the gas?

Identify the correct statements:
I. Energy of an isolated system is constant
II. In a closed system, exchange of both energy and matter is possible
III. Enthalpy is extensive

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 (\(R = 8.314 \text{ J K}^{-1}\text{mol}^{-1}\))