A sample of hydrogen has a volume of 1107 mL when the temperature is 101.9 degC and the pressure is 0.867 atm. What will be the volume of the gas at STP?

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A sample of hydrogen has a volume of 1107 mL when the temperature is 101.9 degC and the pressure is 0.867 atm. What will be the volume of the gas at STP?

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Answer 1 · 2016-06-20T16:55:31

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

Explanation:

So what is $STP$ $"STP"$ ? Standards differ across curricula. I use the IUPAC standard of $273.15 \cdot K$ $273.15*K$ , and $0.98692 \cdot a t m$ $0.98692*atm$ . (The pressure is this absurd value because this represents $100 \cdot k P a$ $100*kPa$ . Chemists usually prefer to work in $atmospheres$ $"atmospheres"$ , as this may be directly measured in a laboratory with a mercury column.)

For the calculation, $V_{2}$ $V_2$ $=$ $=$ $\frac{P_{1} \cdot V_{1} \cdot T_{2}}{T_{1} \cdot P_{2}}$ $(P_1*V_1*T_2)/(T_1*P_2)$

$=$ $=$ $\frac{0.867 \cdot a t m \times 1107 \cdot m L \times 273.15 \cdot K}{375.1 \cdot K \times 0.987 \cdot a t m}$ $(0.867*atmxx1107*mLxx273.15*K)/(375.1*Kxx0.987*atm)$

$=$ $=$ $? ? m L$ $??mL$

Clearly, the expression gives an answer in $m L$ $mL$ , as is required for a volume.

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A sample of hydrogen has a volume of 1107 mL when the temperature is 101.9 degC and the pressure is 0.867 atm. What will be the volume of the gas at STP?

1 Answer

Explanation:

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