In a constant pressure process for $5 \text{ mole}$ of an ideal monoatomic gas,the temperature of the gas increased from $300 \ K$ to $500 \ K$. Which of the following is incorrect regarding the process?
- A$\Delta H_{sys} = 2500 \ R$
- B$\Delta U_{sys} = 1500 \ R$
- C$q = 3500 \ R$
- D$w = -1000 \ R$
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$A$ pure substance (solid,liquid,or gas) of constant composition is taken in a closed container. Select the correct plot if pressure is applied at constant temperature in the absence of non-expansion work.
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View SolutionMatch the thermodynamic processes given under Column $I$ with the expression given under Column $II$:
Column $I$
Column $II$
$A$. Freezing of water at $273 \ K$ and $1 \ atm$
$P$. $q=0$
$B$. Expansion of $1 \ mol$ of an ideal gas into a vacuum under isolated conditions
$Q$. $w=0$
$C$. Mixing of equal volumes of two ideal gases at constant temperature and pressure in an isolated container
$R$. $\Delta S_{sys} < 0$
$D$. Reversible heating of $H_{2(g)}$ at $1 \ atm$ from $300 \ K$ to $600 \ K$,followed by reversible cooling to $300 \ K$ at $1 \ atm$
$S$. $\Delta U=0$
$T$. $\Delta G=0$
| Column $I$ | Column $II$ |
| $A$. Freezing of water at $273 \ K$ and $1 \ atm$ | $P$. $q=0$ |
| $B$. Expansion of $1 \ mol$ of an ideal gas into a vacuum under isolated conditions | $Q$. $w=0$ |
| $C$. Mixing of equal volumes of two ideal gases at constant temperature and pressure in an isolated container | $R$. $\Delta S_{sys} < 0$ |
| $D$. Reversible heating of $H_{2(g)}$ at $1 \ atm$ from $300 \ K$ to $600 \ K$,followed by reversible cooling to $300 \ K$ at $1 \ atm$ | $S$. $\Delta U=0$ |
| $T$. $\Delta G=0$ |
Calculate the difference between heat of combustion of carbon monoxide gas at constant pressure and at constant volume at $27^{\circ} C$ (in $cal$)? $(R = 2 \ cal \ K^{-1} \ mol^{-1})$
DifficultMHT CET 2019
View SolutionCalculate the enthalpy change on freezing of $1.0 \ mol$ of water at $10.0^{\circ} C$ to ice at $-10.0^{\circ} C$. Given: $\Delta_{fus} H = 6.03 \ kJ \ mol^{-1}$ at $0^{\circ} C$,$C_p [H_2 O_{(l)}] = 75.3 \ J \ mol^{-1} \ K^{-1}$,$C_p [H_2 O_{(s)}] = 36.8 \ J \ mol^{-1} \ K^{-1}$.
Medium
View SolutionThe heat associated with the combustion of liquid benzene at constant volume is $-3268 \ kJ \ mol^{-1}$. Calculate the change in enthalpy when this reaction occurs at $300 \ K$ $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$.
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