If the volume of an ideal gas at $"350 torr"$ of pressure and $25^@ "C"$ is $"450 L"$ , at what temperature is its volume $"420 L"$ and pressure $"830 torr"$ in a sealed balloon?

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Answer 1 · 2016-12-08T13:53:44

386.6 degrees C

$(V_1 xx P_1)/T_1 = (V_2 xx P_2)/T_2$

$V_1 = 450$
$P_1 = 350$
$T_1 = 273 + 25 = 298$ temperature must be calculated in degrees K or absolute zero.

$V_2 = 420$
$P_2 = 830$
$T_2 = unknown ?$

putting these values into the equation gives

$(450 xx 350)/298 = (420 xx 830)/T_2$ Solving for $T_2$ gives

$T_2 = (420 xx 830 xx 298)/ (450 xx 350)$ solving gives

#T_2 = 659.57333333 subtract 273 to bring back to degrees C and round off to four significant figures. gives

$T_2 = 386.6$

If the volume of an ideal gas at "350 torr""350 torr" of pressure and 25^@ "C"25^@ "C" is "450 L""450 L", at what temperature is its volume "420 L""420 L" and pressure "830 torr""830 torr" in a sealed balloon?