List of top Chemistry Questions on Work done in Thermodynamics asked in KEAM

The mathematical statement of the first law of thermodynamics with the usual notation is
1 g of graphite is burnt completely in excess oxygen at 298K and 1 atmospheric pressure in a bomb calorimeter. During the reaction, the temperature raises from 298K to 299K. If the heat capacity of the bomb calorimeter is 20.7 kJ K\(^{-1}\), what is the enthalpy of combustion of C(gr)? (Atomic mass of carbon is 12 g mol\(^{-1}\))
In a free expansion of a gas
The first law of thermodynamics can be stated as
An ideal gas is allowed to expand from 1 L to 10 L against a constant external pressure of 1 bar. The work done is [1 bar = 100 J]}
\( \Delta G \) for \( 3\text{X}_{(g)} + 2\text{Y}_{(g)} \rightarrow 3\text{Z}_{(g)} \) at 293 K is
( \( \Delta H^\circ = -13\,\text{kJ mol}^{-1} \), \( \Delta S^\circ = -45\,\text{J mol}^{-1}\text{K}^{-1} \) )
Given: $\Delta_r H^{+}(\text{Ag}^+)=105.6\ \text{kJ mol}^{-1}$, $\Delta_r H^{+}(\text{Cl}^-)=-167.2\ \text{kJ mol}^{-1}$, and $\Delta_r H^{+}(\text{AgCl})=-127.1\ \text{kJ mol}^{-1}$, find the value of $\Delta_r H$.
Types of system and their definitions are given below. Choose the correct match from the following codes:
System:
(a) Closed system
(b) Open system
(c) Isolated system
(d) Homogeneous system
(e) Heterogeneous system
Definition:
(i) A system which can exchange both energy and matter with surrounding
(ii) A system which cannot exchange matter or energy with surrounding
(iii) A system consisting of single phase
(iv) A system consisting of many phases
(v) A system which can exchange only energy with surrounding
The enthalpy of combustion values of $C_{2}H_{4(g)}$, $C_{(graphite,s)}$ and $H_{2(g)}$ are respectively $-1411\ \text{kJ mol}^{-1}$, $-394\ \text{kJ mol}^{-1}$ and $-286\ \text{kJ mol}^{-1}$. What is the enthalpy of formation of $C_{2}H_{4(g)}$ in $\text{kJ mol}^{-1}$?
In which of the following reactions does entropy decrease? (i) $2Pb(NO_{3})_{2(s)}\rightarrow 2PbO_{(s)}+4NO_{2(g)}+O_{2(g)}$ (ii) $H_{2}O_{(g)}\rightarrow H_{2}O_{(l)}$ (iii) $Br_{2(l)}\rightarrow 2Br_{(g)}$ (iv) $C_{6}H_{6(l)}\rightarrow C_{6}H_{6(s)}$
In the reaction \( \frac{3}{2}O_2(g) \rightarrow O_3(g) \), the value of \( \Delta_r G^\circ \) at \( 298\,K \) is approximately ( \( K_p = 10^{-30},\ 2.303RT = 5.7\,\text{kJ mol}^{-1} \) )
Consider the following thermodynamic properties of a system: (i) Volume (ii) Pressure (iii) Density (iv) Heat capacity. The extensive property/properties of the system is/are
\( \mathrm{Fe_2O_{3(s)} + 3H_{2(g)} \rightarrow 2Fe_{(s)} + 3H_2O_{(l)}} \) \(\text{(Given: } \Delta H^\circ(\mathrm{H_2O_{(l)}}) = -285.83\,\text{kJ mol}^{-1},\ \Delta H^\circ(\mathrm{Fe_2O_{3(s)}}) = -824.2\,\text{kJ mol}^{-1}\text{)}\)
Enthalpy change is always negative for which one of the following processes?
What are the thermodynamic conditions for a reaction to be spontaneous at low temperature and non-spontaneous at high temperature?
In which one of the following reactions, entropy decreases?
The standard enthalpies of formation of \(H_2O(l)\) and \(CO_2(g)\) are respectively \(-286\ \text{kJ mol}^{-1}\) and \(-394\ \text{kJ mol}^{-1}\). If the standard heat of combustion of \(CH_4(g)\) is \(-891\ \text{kJ mol}^{-1}\), then the standard enthalpy of formation of \(CH_4(g)\) is
The standard heat of formation of CH\(_4\), CO\(_2\) and H\(_2\)O (l) are \( -76.2 \), \( -394.8 \) and \( -285.82 \) kJ mol\(^{-1} \), respectively. Heat of vaporization of water is 44 kJ mol\(^{-1} \). Calculate the amount of heat evolved when 22.4 L of CH\(_4\), kept under normal conditions, is oxidized into its gaseous products
One mole of ethanol is produced reacting graphite, $H_2$ and $O_2$ together. The standard enthalpy of formation is $-277.7\,\text{kJ mol}^{-1}$. Calculate the standard enthalpy of the reaction when 4 moles of graphite is involved
For the process $A(l,\,0.05\,\text{atm},\,32^\circ C) \rightarrow A(g,\,0.05\,\text{atm},\,32^\circ C)$, the correct set of thermodynamic parameters is
The standard enthalpy of formation of H₂O(l) and Fe₂O₃(s) are respectively −286 kJ mol⁻¹ and −824 kJ mol⁻¹. What is the standard enthalpy change for the following reaction?
\[ \text{Fe}_2\text{O}_3(s) + 3\text{H}_2(g) \rightarrow 3\text{H}_2\text{O}(l) + 2\text{Fe}(s) \]
The enthalpy of combustion of glucose (molecular weight = 180 g mol$^{-1}$) is $-2840$ kJ mol$^{-1}$. Then the amount of heat evolved when $0.9$ g of glucose is burnt, will be}
The enthalpy change for a reaction at equilibrium is $-20.5$ kJ mol$^{-1}$. Then the entropy change for this equilibrium at 410 K is}
The entropy of vaporization of a liquid is 58 JK\textsuperscript{--1mol\textsuperscript{--1}. If 100 g of its vapour condenses at its boiling point of 123$^\circ$C, the value of entropy change for the process is (Molar mass of the liquid = 58 g mol\textsuperscript{--1})}
The entropy of vaporization of a liquid is 58 JK\textsuperscript{--1mol\textsuperscript{--1}. If 100 g of its vapour condenses at its boiling point of 123$^\circ$C, the value of entropy change for the process is (Molar mass of the liquid = 58 g mol\textsuperscript{--1})}