# If the partial pressure of the diatomic gas is 0.540 atm, what is the total pressure?

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If the partial pressure of the diatomic gas is 0.540 atm, what is the total pressure?

Consider this molecular-level representation of a gas.

If the partial pressure of the diatomic gas is 0.540 atm, what is the total pressure?

6 blue dots

5 yellow dots

3 pair green dots (sticked together)

One way to solve this problem is to find the mole fraction of the diatomic gas. There is a total of 14 independently moving gas particles in this sample. Of those 14 particles, 3 are diatomic. Thus, the mole fraction of the diatomic gas is X = 3/14 = 0.2143. Use the following equation to solve for the total pressure. If you aren\'t familiar with mole fraction or the formula above, that\'s ok. Instead, consider that the diatomic gas makes up of 3/14 = 21.43% of the particles. Thus, 0.540 atm is 21.43% of the total pressure.

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Ignoring everything except the last line in "details", you have the equation:

0.2143P = 0.540 atm

which means that P = 2.52 atm.

Is that answer being marked wrong?

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Pgas=XgasxPtotal

0.540=3/14xPtotal

Ptotal =2.52

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Given: P(total) = 0.54, X(A) = 0.2143

P(total) = P(A) x X(A)

so P(A) = P(total) / X(A) = 0.54/0.2143

= 2.5

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