285271
Lattice enthalpy for NaCl is\(+788 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and \(\Delta_{\mathrm{Hyd}}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1}\). Enthalpy of solution of NaCl is
285272
The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of 1 L to 10 L at\(300 \mathrm{~K}^{-18}\left(R=0.0083 \mathrm{~kJ} \mathrm{~K} \mathrm{~mol}^{-1}\right)\)
1 0.115 kJ
2 58.5 kJ
3 11.5 kJ
4 5.8 kJ
Explanation:
(c) For an isothermal reversible expansion of an ideal gas work done is calculated as:
\(\begin{aligned}
& w=-2.303 n R T \log \left(\frac{V_2}{V_1}\right) \\
& =-2.303 \times 2 \times 0.0083 \mathrm{~kJ} \times 300 \times \log \left(\frac{10}{1}\right) \\
& =-11.5 \mathrm{~kJ}
\end{aligned}\)
Karnataka CET 2022
CHEMISTRY(KCET)
285273
Bond enthalpies of\(A_2, B_2\) and \(A B\) are in the ratio 2 : \(1: 2\). If bond enthalpy of formation of \(A B\) is -100 kJ \(\mathrm{mol}^{-1}\). The bond enthalpy of \(B_2\) is
285271
Lattice enthalpy for NaCl is\(+788 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and \(\Delta_{\mathrm{Hyd}}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1}\). Enthalpy of solution of NaCl is
285272
The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of 1 L to 10 L at\(300 \mathrm{~K}^{-18}\left(R=0.0083 \mathrm{~kJ} \mathrm{~K} \mathrm{~mol}^{-1}\right)\)
1 0.115 kJ
2 58.5 kJ
3 11.5 kJ
4 5.8 kJ
Explanation:
(c) For an isothermal reversible expansion of an ideal gas work done is calculated as:
\(\begin{aligned}
& w=-2.303 n R T \log \left(\frac{V_2}{V_1}\right) \\
& =-2.303 \times 2 \times 0.0083 \mathrm{~kJ} \times 300 \times \log \left(\frac{10}{1}\right) \\
& =-11.5 \mathrm{~kJ}
\end{aligned}\)
Karnataka CET 2022
CHEMISTRY(KCET)
285273
Bond enthalpies of\(A_2, B_2\) and \(A B\) are in the ratio 2 : \(1: 2\). If bond enthalpy of formation of \(A B\) is -100 kJ \(\mathrm{mol}^{-1}\). The bond enthalpy of \(B_2\) is
285271
Lattice enthalpy for NaCl is\(+788 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and \(\Delta_{\mathrm{Hyd}}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1}\). Enthalpy of solution of NaCl is
285272
The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of 1 L to 10 L at\(300 \mathrm{~K}^{-18}\left(R=0.0083 \mathrm{~kJ} \mathrm{~K} \mathrm{~mol}^{-1}\right)\)
1 0.115 kJ
2 58.5 kJ
3 11.5 kJ
4 5.8 kJ
Explanation:
(c) For an isothermal reversible expansion of an ideal gas work done is calculated as:
\(\begin{aligned}
& w=-2.303 n R T \log \left(\frac{V_2}{V_1}\right) \\
& =-2.303 \times 2 \times 0.0083 \mathrm{~kJ} \times 300 \times \log \left(\frac{10}{1}\right) \\
& =-11.5 \mathrm{~kJ}
\end{aligned}\)
Karnataka CET 2022
CHEMISTRY(KCET)
285273
Bond enthalpies of\(A_2, B_2\) and \(A B\) are in the ratio 2 : \(1: 2\). If bond enthalpy of formation of \(A B\) is -100 kJ \(\mathrm{mol}^{-1}\). The bond enthalpy of \(B_2\) is
285271
Lattice enthalpy for NaCl is\(+788 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and \(\Delta_{\mathrm{Hyd}}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1}\). Enthalpy of solution of NaCl is
285272
The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of 1 L to 10 L at\(300 \mathrm{~K}^{-18}\left(R=0.0083 \mathrm{~kJ} \mathrm{~K} \mathrm{~mol}^{-1}\right)\)
1 0.115 kJ
2 58.5 kJ
3 11.5 kJ
4 5.8 kJ
Explanation:
(c) For an isothermal reversible expansion of an ideal gas work done is calculated as:
\(\begin{aligned}
& w=-2.303 n R T \log \left(\frac{V_2}{V_1}\right) \\
& =-2.303 \times 2 \times 0.0083 \mathrm{~kJ} \times 300 \times \log \left(\frac{10}{1}\right) \\
& =-11.5 \mathrm{~kJ}
\end{aligned}\)
Karnataka CET 2022
CHEMISTRY(KCET)
285273
Bond enthalpies of\(A_2, B_2\) and \(A B\) are in the ratio 2 : \(1: 2\). If bond enthalpy of formation of \(A B\) is -100 kJ \(\mathrm{mol}^{-1}\). The bond enthalpy of \(B_2\) is
