A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 334 mmHg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?

1110

Convert 1.02 atm to torr. 760 torr = 1 atm.

334 mm Hg = 334 torr.
Add the two (in torr) to find total pressure.

To solve this problem, we need to convert the partial pressure of oxygen from atm to mmHg and then determine the total pressure by adding the partial pressures of cyclopropane and oxygen.

1. Convert the partial pressure of oxygen from atm to mmHg:
1 atm = 760 mmHg
1.02 atm * 760 mmHg/atm = 775.2 mmHg

2. Determine the total pressure by adding the partial pressures of cyclopropane and oxygen:
Total pressure = partial pressure of cyclopropane + partial pressure of oxygen
Total pressure = 334 mmHg + 775.2 mmHg
Total pressure = 1109.2 mmHg

Therefore, the total pressure of the cyclopropane-oxygen mixture is 1109.2 mmHg.

To find the total pressure of the mixture, we need to convert the partial pressures of cyclopropane and oxygen to the same unit before adding them together.

First, let's convert the partial pressure of oxygen from atm to mmHg. Since 1 atm = 760 mmHg, we can multiply the partial pressure of oxygen by 760:

1.02 atm * 760 mmHg/atm = 775.2 mmHg.

Now, let's add the partial pressures of cyclopropane (334 mmHg) and oxygen (775.2 mmHg):

334 mmHg + 775.2 mmHg = 1109.2 mmHg.

Therefore, the total pressure of the mixture is 1109.2 mmHg.