How is 4.3 x 10^-3 the answer to this question? A sample of air from a home is found to contain 6.2 ppm of carbon monoxide. This means that if the total pressure is 695 torr, then the partial pressure of CO is..................4.3 x 10^-3.

Answers

Answer 1

Answer: The partial pressure of CO2 is equal to the total pressure * molar fraction of CO2.

To give 4.3 * 10^-3, they are using molar fraction = 6.2 * 10^ - 6

Because, 695 * 6.2-10^-6 = 0.004309 = 4.309 * 10^-3 = 4.3 * 10^-3.

Then the new question is why the molar fraction is consideres to be the same ppm concentration. This is because ppm means parts per million, and in this case, they are considering that the parts are moles (usually it is grams, but it is not the case, given the result).

6.2 ppm = 6.2 / 1,000,000 = 6.2*10^-6, which is the number used above to multiply the total pressure and get the partial pressure of CO2.

If you had not told me that the result was 4.3 * 10^-3, I had assumedthat 6.2 was referred to grams and not moles and I had made a conversionusing the molar masses of the air and the CO2 but, again, this is not the case.

Answer 2

Answer:

Final answer:

The partial pressure of CO in a home with air containing 6.2 ppm CO, when the total air pressure is 695 torr, can be calculated by (6.2 ÷ 1,000,000) x 695, which equals 4.3 x 10^-3 torr.

Explanation:

The partial pressure of a gas is the individual pressure contribution a single type of gas makes to the overall pressure of a gas mixture. In this case, a sample of air from a home was found to contain 6.2 parts per million (ppm) of carbon monoxide (CO). To calculate the actual pressure of CO in the room, we can use the fact that 1 ppm = 1 part of the substance per 1,000,000 parts of air.

To do so, we need to multiply thetotal pressure of the air, which is 695 torr, by the ratio of the CO to the total volume of the air. That would be: (6.2 ÷ 1,000,000) x 695 = 4.3 x 10-3 torr. Hence, that is how 4.3 x 10-3 is derived as the partial pressure of CO in this context.

Learn more about Partial Pressure here:

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Answers

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Answers

Answer:

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Answers

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Answers

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