Question

a cyclopropane - oxygen mixture is used as an anesthetic. if the partial pressure of cyclopropane in the mixture is 330 mmhg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr? (1 atm = 760 mmhg = 760 torr)
1100 torr
740 torr
1.4 torr
430 torr
280 torr

Explanation:

Step1: Convert units

Given \(1\ atm = 760\ mmHg=760\ torr\). The partial pressure of cyclopropane \(P_{cyclopropane}=330\ mmHg = 330\ torr\) (since \(1\ mmHg = 1\ torr\)), and the partial pressure of oxygen \(P_{O_2}=1.0\ atm = 760\ torr\).

Step2: Apply Dalton's law of partial pressures

Dalton's law states that \(P_{total}=P_1 + P_2+\cdots+P_n\). Here, \(P_{total}=P_{cyclopropane}+P_{O_2}\).
Substitute the values: \(P_{total}=330\ torr+760\ torr\).

Answer:

\(1090\approx1100\) torr, so the answer is \(1100\ torr\) (the small difference is due to rounding in the problem - statement's approximated values).