A gas bottle contains 0.450 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?

Question

Quizplus · Accepted Answer

Using the ideal gas law in the form $P_1V_1 = n_1RT$ and $P_2V_2 = n_2RT$ for the same volume and temperature, we can set $P_1/n_1 = P_2/n_2$. Given $P_1 = 730 \, \text{mm Hg}$ (which is equivalent to $730/760 = 0.961 \, \text{atm}$) and $P_2 = 1.15 \, \text{atm}$, with $n_1 = 0.450 \, \text{mol}$, we solve for $n_2$. Rearranging gives $n_2 = n_1 \times (P_2/P_1)$. Plugging in the numbers: $n_2 = 0.450 \times (1.15/0.961) = 0.5387 \, \text{mol}$. The moles of gas added is $n_2 - n_1 = 0.5387 - 0.450 = 0.0887 \, \text{mol}$, which rounds to $0.0888 \, \text{mol}$.

A Gas Bottle Contains 0