alka8q7

2021-11-17

The air in a bicycle tire is bubbled through water and collected at ${25}^{\circ}C$. If the total volume of gas collected is 5.45 L at a temperature of ${25}^{\circ}C$ and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

Froldigh

Beginner2021-11-18Added 17 answers

Step 1

$T=(25+273.15)K=298.15K$

${P}_{\to t}=745\to rr=745mmHg$

${P}_{{H}_{2}O}=23.78mmHg$

$V=5.45L$

${n}_{gas}=?$

Write down the known and unknown values.

Step 2

$P}_{\to t}={P}_{{H}_{2}O}+{P}_{gas$

$P}_{gas}={P}_{\to t}-{P}_{{H}_{2}O$

$=745mmHg--23.7mmHg$

$=721.3mmHg$

To determine the evolved gas's partial pressure, use the gas-evolution equation based on Dalton's Law of

Step 3

${P}_{gas}=\begin{array}{cc}721.3\mathrm{m\u0338}\mathrm{m\u0338}\mathrm{H\u0338}g& 1atm\\ & 760\mathrm{m\u0338}\mathrm{m\u0338}\mathrm{H\u0338}g\end{array}=0.94908atm$

Convert the evolved gas's partial pressure into atmospheres.

Step 4

${P}_{gas}V={n}_{gas}RT\phantom{\rule{0ex}{0ex}}{n}_{gas}=\frac{{P}_{gas}V}{RT}\phantom{\rule{0ex}{0ex}}=\begin{array}{ccc}0.94908\mathrm{a\u0338}\mathrm{t\u0338}\mathrm{m\u0338}& mol\cdot \mathrm{K\u0338}& 5.45\mathrm{L\u0338}\\ & 0.08206\mathrm{L\u0338}\cdot \mathrm{a\u0338}\mathrm{t\u0338}\mathrm{m\u0338}& 298.15\mathrm{K\u0338}\end{array}=0.211mol$

To determine how many moles of the evolved gas there are, use the Ideal Gas Law.

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