an air sample contains 0.046% CO2 if the total pressure is 760mmHg what is the partial pressure of CO2
To find the partial pressure of CO2 in the air sample, you can 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 individual gas component.
In this case, the total pressure is given as 760 mmHg. The partial pressure of CO2 can be calculated as follows:
1. Convert the percentage of CO2 to decimal form: 0.046% = 0.046/100 = 0.00046.
2. Multiply the decimal form by the total pressure to find the partial pressure of CO2: 0.00046 × 760 mmHg = 0.3496 mmHg.
Therefore, the partial pressure of CO2 in the air sample is approximately 0.35 mmHg.