## Related questions with answers

If $25.50$ mol of helium gas is at $10\degree\mathrm{C}$ and a gauge pressure of $0.350$ atm, calculate (a) the volume of the helium gas under these conditions, and (b) the temperature if the gas is compressed to precisely half the volume at a gauge pressure of $1.00$ atm.

Solutions

Verified**Given/Constants**

$\begin{aligned} n&=25.50\text{ mol} \\ P&=0.350\text{ atm} \\ R&=8.315\text{ J/mol-K} \\ T&=10^\circ\text{C}=283.15\text{ K} \end{aligned}$

For this problem, we are to solve for **a.)** the volume $V_1$ of the helium gas and **b.)** the temperature $T_2$ if the gas was compressed half the original volume $V_2 = \frac{1}{2} V_1$ and with $P_2 = 1.00 \,\mathrm{atm}$ given that there is a $n = 25 \,\mathrm{mol}$ of helium gas at $T_1 = 10^\circ\mathrm{C}$ and $P_2 = 0.350 \,\mathrm{atm}$ .

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