1
MHT CET 2022 11th August Evening Shift
+1
-0

What is the heat of formation of $$\mathrm{HCl}_{(\mathrm{g})}$$ from following equation?

$$\mathrm{H}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{g})} \rightarrow 2 \mathrm{HCl}_{(\mathrm{g})} \Delta_{\mathrm{f}} \mathrm{H}=-194 \mathrm{~kJ}$$

A
$$-388 \mathrm{~kJ}$$
B
$$-194 \mathrm{~kJ}$$
C
$$-97 \mathrm{~kJ}$$
D
$$194 \mathrm{~kJ}$$
2
MHT CET 2022 11th August Evening Shift
+1
-0

If $$\mathrm{Q}$$ is the heat liberated from the system and $$\mathrm{W}$$ is the work done on the system then first law of thermodynamics can be written as,

A
$$\mathrm{Q}=\mathrm{W}-\Delta \mathrm{U}$$
B
$$\mathrm{Q}=\Delta \mathrm{U}-\mathrm{W}$$
C
$$\mathrm{Q}=\Delta \mathrm{U}+\mathrm{W}$$
D
$$\mathrm{Q}=-\mathrm{W}$$
3
MHT CET 2021 24th September Evening Shift
+1
-0

For isochoric process, the first law of thermodynamics can be expressed as

A
$$\Delta \mathrm{U}=\mathrm{Q}_{\mathrm{V}}$$
B
$$\mathrm{-\Delta U=Q-P \Delta V}$$
C
$$\mathrm{-\Delta U=-W}$$
D
$$\mathrm{W}=-\mathrm{Q}$$
4
MHT CET 2021 24th September Evening Shift
+1
-0

When certain volume of gas expands against a constant external pressure of $$2.40 \times 10^5 \mathrm{~Pa}$$ at 300 $$\mathrm{K}$$ to $$2.2 \times 10^{-3} \mathrm{~m}^3$$. If the work obtained is $$-0.048 \mathrm{~kJ}$$. What is the initial volume of the gas?

A
$$2 \times 10^{-3} \mathrm{~m}^3$$
B
$$4.5 \times 10^{-2} \mathrm{~m}^3$$
C
$$1.5 \times 10^{-3} \mathrm{~m}^3$$
D
$$2.8 \times 10^{-2} \mathrm{~m}^3$$
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