1
MHT CET 2024 9th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

For the reaction,

$$\mathrm{C}_3 \mathrm{H}_{8(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 3 \mathrm{CO}_{2(\mathrm{~g})}+4 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$$

at constant temperature, $\Delta \mathrm{H}-\Delta \mathrm{U}$ is

A
$-$2RT
B
RT
C
$-$3RT
D
3RT
2
MHT CET 2024 9th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

What is change in internal energy of the system when work done by the system is 150 J and system release 300 J of heat?

A
$+450$ J
B
$-450$ J
C
$+300$ J
D
$-150$ J
3
MHT CET 2024 9th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

Two moles of an ideal gas is expanded isothermally from a volume of $300 \mathrm{~cm}^3$ to 2.5 $\mathrm{dm}^3$ at 298 K against a constant pressure at 1.9 bar. Calculate the work done in joules.

A
$-$418 J
B
$-$565 J
C
$-$918 J
D
$-$950 J
4
MHT CET 2024 4th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

Calculate heat required to convert 9 g of liquid water to water vapours from following equations.

$$\begin{aligned} & \mathrm{H}_{2(\mathrm{~g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \Delta \mathrm{H}=-57 \mathrm{kCal} \\ & \mathrm{H}_{2(\mathrm{~g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \Delta \mathrm{H}=-68.3 \mathrm{kCal} \end{aligned}$$

A
5.65 k Cal
B
6.28 k Cal
C
7.05 k Cal
D
9.72 k Cal
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