An air sample contains 0.038% CO2. If the total pressure is 764 mm Hg , what is the partial pressure of CO2?

dont you just multiply .038 times the total pressure?

i tried that but it says its wrong

oh i think you have to convert the mm Hg to atm first

To find the partial pressure of CO2 in the air sample, we need to use Dalton's law of partial pressures. According to this law, the total pressure of a gas mixture is equal to the sum of the partial pressures of each gas component.

In this case, the air sample contains CO2, which is one of the gas components. The partial pressure of CO2 can be calculated by multiplying the total pressure by the fraction of CO2 in the air sample.

Step 1: Convert the fraction of CO2 to a decimal.
0.038% is equivalent to 0.038/100 = 0.00038.

Step 2: Calculate the partial pressure of CO2.
Partial pressure of CO2 = Total pressure × Fraction of CO2
Partial pressure of CO2 = 764 mm Hg × 0.00038

Using a calculator, multiply 764 by 0.00038 to get the answer.

The partial pressure of CO2 in the air sample is approximately 0.2903 mm Hg.