$2.4 \ g$ coal is burnt in a bomb calorimeter in excess of oxygen at $298 \ K$ and $1 \ atm$ pressure. The temperature of the calorimeter rises from $298 \ K$ to $300 \ K$. The enthalpy change during the combustion of coal is $-x \ kJ \ mol^{-1}$. The value of $x$ is. (Nearest Integer) (Given: Heat capacity of bomb calorimeter $20.0 \ kJ \ K^{-1}$. Assume coal to be pure carbon)
- A$201$
- B$202$
- C$203$
- D$200$
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Similar Questions
The molar heats of fusion and vaporisation of benzene are $10.9$ and $31.0 \ kJ \ mol^{-1}$ respectively. The changes in entropy for the solid $\rightarrow$ liquid and liquid $\rightarrow$ vapour transitions for benzene are $x$ and $y \ JK^{-1} \ mol^{-1}$,respectively. The value of $(y-x)$ (in $JK^{-1} \ mol^{-1}$) is (At $1 \ atm$,benzene melts at $5.5^{\circ} C$ and boils at $80^{\circ} C$).
The heat of neutralization of a strong acid and a strong alkali is $-57.0 \ kJ \ mol^{-1}$. The heat released when $0.5 \ mole$ of $HNO_3$ solution is mixed with $0.2 \ mole$ of $KOH$ is ....$kJ$
Medium
View Solution$11.0 \ L$ of an ideal gas at a constant external pressure of $5 \ atm$ is compressed isothermally to a final volume of $1 \ L$. The heat absorbed and work done,respectively,during this compression (in $L \ atm$) are:
Match the transformations in Column-$I$ with the appropriate options in Column-$II$.
Column-$I$ Column-$II$ $(A) \; CO_{2(s)} \to CO_{2(g)}$ $(p) \; \text{Transition state}$ $(B) \; CaCO_{3(s)} \to CaO_{(s)} + CO_{2(g)}$ $(q) \; \text{Allotropic change}$ $(C) \; 2H^{\cdot} \to H_{2(g)}$ $(r) \; \Delta H > 0$ $(D) \; P_{\text{(white solid)}} \to P_{\text{(red solid)}}$ $(s) \; \Delta S > 0$ $(t) \; \Delta S < 0$
| Column-$I$ | Column-$II$ |
|---|---|
| $(A) \; CO_{2(s)} \to CO_{2(g)}$ | $(p) \; \text{Transition state}$ |
| $(B) \; CaCO_{3(s)} \to CaO_{(s)} + CO_{2(g)}$ | $(q) \; \text{Allotropic change}$ |
| $(C) \; 2H^{\cdot} \to H_{2(g)}$ | $(r) \; \Delta H > 0$ |
| $(D) \; P_{\text{(white solid)}} \to P_{\text{(red solid)}}$ | $(s) \; \Delta S > 0$ |
| $(t) \; \Delta S < 0$ |
Difficult
View Solution$A$ gas expands from $3 \ dm^{3}$ to $5 \ dm^{3}$ against a constant pressure of $3 \ atm$. The work done during this expansion is used to heat $10 \ mol$ of water at $290 \ K$. What will be the final temperature of the water in $K$? (Specific heat of water = $4.184 \ J \ g^{-1} \ K^{-1}$)
Medium
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