A rigid vessel contains a non-reacting mixture of , , and . Their respective partial pressures are , — States of Matter and Gaseous State Chemistry Question
Question
A rigid vessel contains a non-reacting mixture of $N_2$, $O_2$, and $CO_2$. Their respective partial pressures are $38\text{ cm of Hg}$, $190\text{ torr}$, and $0.5\text{ atm}$. Calculate the total pressure of the gaseous mixture in $\text{atm}$ at the same temperature, and then multiply your final answer by $100$ to report an integer.
Answer: 125
💡 Solution & Explanation
First, convert all partial pressures to standard atm. $P_{N_2} = 38\text{ cm Hg} = 380\text{ mm Hg} = 380/760\text{ atm} = 0.5\text{ atm}$. $P_{O_2} = 190\text{ torr} = 190\text{ mm Hg} = 190/760\text{ atm} = 0.25\text{ atm}$. $P_{CO_2} = 0.5\text{ atm}$. By Dalton's Law, $P_{total} = 0.5 + 0.25 + 0.5 = 1.25\text{ atm}$. Multiplying by 100 gives $125$.
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