The volume of a sample of a gas at 273°C is 200.0 L. If the volume is decreased to 100.0 L at constant pressure, what will be the new temperature of the gas?

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The volume of a sample of a gas at 273°C is 200.0 L. If the volume is decreased to 100.0 L at constant pressure, what will be the new temperature of the gas?

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Answer 1 · 2015-11-03T21:41:37

$T_{2} = 273 K$ $T_2="273 K"$

Explanation:

Charles' Law states that when pressure is held constant, the temperature and volume of a gas are directly proportional, so that if one goes up, so does the other. Note: The temperature needs to be in Kelvins.

The equation for Charles' Law is $\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}$ $V_1/T_1=V_2/T_2$

$V_{1} = 200.0 L$ $V_1="200.0 L"$
$T_{1} = 273^{o} C+273=546 K$ $T_1="273"^"o""C+273=546 K"$
$V_{2} = 100.0 L$ $V_2="100.0 L"$
$T_{2} = ?$ $T_2="?"$

Solution
Rearrange the equation to isolate $T_{2}$ $T_2$ and solve.

$T_{2} = \frac{V_{2} T_{1}}{V_{1}}$ $T_2=(V_2T_1)/V_1$

$T_2=(100.0cancel"L"xx546"K")/(200cancel"L")=$

$T_2="273 K"$

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The volume of a sample of a gas at 273°C is 200.0 L. If the volume is decreased to 100.0 L at constant pressure, what will be the new temperature of the gas?

1 Answer

Explanation:

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