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CBSE - Class 11 > Chemistry > Thermodynamics Worksheets

Free CBSE - Class 11 Chemistry - Thermodynamics worksheets

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1.
The equilibrium constant for a reaction is 10. What will be the value of $ΔG^o$ ? $R = 8.314 \text{ JK}^{-1} \text{ mol}^{-1}$, $T = 300 K$.
2.
Comment on the thermodynamic stability of $NO(g)$, given
$\frac{1}{2} N_2(g) + \frac{1}{2}O_2(g) \rightarrow NO(g)$; $Δ_rH^o = 90 \text{ kJ mol}^{-1}$
$NO(g) + \frac{1}{2}O_2(g) \rightarrow NO_2(g)$: $Δ_rH^o= -74 \text{ kJ mol}^{-1}$
3.
Calculate the entropy change in surroundings when 1.00 mol of $H_2O(l)$ is formed under standard conditions. $Δ_fH^o = -286 \text{ kJ mol}^{-1}$.
4.
For an isolated system, $ΔU = 0$, what will be $ΔS$ ?
5.
For the reaction at 298 K,
$2A + B \rightarrow C$
$ΔH = 400 \text{ kJ mol}^{-1}$ and $ΔS = 0.2 \text{ kJ K}^{-1} \text{ mol}^{-1}$
At what temperature will the reaction become spontaneous considering $ΔH$ and $ΔS$ to be constant over the temperature range.
6.
For the reaction,
$2 Cl(g) \rightarrow Cl_2(g)$, what are the signs of $ΔH$ and $ΔS$ ?
7.
For the reaction
$2 A(g) + B(g) \rightarrow 2D(g)$
$ΔU^o = -10.5 \text{ kJ}$ and $ΔS^o = -44.1 \text{ JK}^{-1}$.
Calculate $ΔG^o$ for the reaction, and predict whether the reaction may occur spontaneously.
8.
Enthalpies of formation of $CO(g)$, $CO_2(g)$, $N_2O(g)$ and $N_2O_4(g)$ are $-110$, $-393$, 81 and $9.7 \text{ kJ mol}^{-1}$ respectively. Find the value of $Δ_rH$ for the reaction:
$N_2O_4(g) + 3CO(g) \rightarrow N_2O(g) + 3CO_2(g)$
9.
Calculate the standard enthalpy of formation of $CH_3OH(l)$ from the following data:
$CH_3OH (l) + \frac{3}{2} O_2(g) \rightarrow CO_2(g) + 2H_2O(l)$ ; $Δ_rH^o = -726 \text{ kJ mol}^{-1}$
$C(graphite) + O_2(g) \rightarrow CO_2(g)$ ; $Δ_cH^o = -393 \text{ kJ mol}^{-1}$
$H_2(g) + \frac{1}{2} O_2(g) \rightarrow H_2O(l)$; $Δ_fH^o = -286 \text{ kJ mol}^{-1}$.
10.
Calculate the enthalpy change for the process
$CCl_4(g) \rightarrow C(g) + 4 Cl(g)$
and calculate bond enthalpy of C – Cl in $CCl_4(g)$.
$Δ_{vap}H^o(CCl_4) = 30.5 \text{ kJ mol}^{-1}$.
$Δ_fH^o (CCl_4) = -135.5 \text{ kJ mol}^{-1}$.
$Δ_aH^o (C) = 715.0 \text{ kJ mol}^{-1}$, where $Δ_aH^o$ is enthalpy of atomisation
$Δ_aH^o (Cl_2) = 242 \text{ kJ mol}^{-1}$
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