Question #52ade

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Question #52ade

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Answer 1 · 2015-11-26T00:46:36

The final volume of nitrogen gas will be $528 mL$ $"528 mL"$ .

Explanation:

Use the combined gas law with the equation $\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ $(P_1V_1)/(T_1)=(P_2V_2)/(T_2)$ .

Given/Known
$P_{1} = 740 torr$ $P_1="740 torr"$
$V_{1} = 500. mL$ $V_1="500. mL"$
$T_{1} = 25^{o} C + 273.15 = 298 K$ $T_1="25"^"o""C"+273.15="298 K"$
$P_{2} = 760 torr$ $P_2="760 torr"$
$T_{2} = 50^{o} C + 273.15 = 323 K$ $T_2="50"^"o""C"+273.15="323 K"$

Unknown
$V_{2}$ $V_2$

Equation
$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ $(P_1V_1)/(T_1)=(P_2V_2)/(T_2)$

Solution
Rearrange the equation to isolate $V_{2}$ $V_2$ and solve.

$V_{2} = \frac{P_{1} V_{1} T_{2}}{T_{1} P_{2}}$ $V_2=(P_1V_1T_2)/(T_1P_2)$

$V_2=(740cancel"torr"xx500. "mL"xx323cancel"K")/(298cancel"K"xx760cancel"torr")="528 mL N"_2"$

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Question #52ade

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