MCQ
$4$ moles of an ideal gas is at $0°C.$ At constant pressure it is heated to double its volume, then its final temperature will be ...... $^oC$
- A$0$
- ✓$273$
- C$546$
- D$136.5$
✓
Answer
Correct option: B.
$273$
b
$\frac{{{V_1}}}{{{V_2}}} = \frac{{{T_1}}}{{{T_2}}}$
$\frac{{{V_1}}}{{{V_2}}} = \frac{{{T_1}}}{{{T_2}}}$
$\Rightarrow {T_2} = 2 \times {T_1}$ $ = 2 \times (273 + 0) = 546K$
$\Rightarrow$ ${T_2} = 273 \times 2 = 546K$
$\Rightarrow 273^\circ C$ $\Rightarrow 273$ $^\circ$$ C$
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