| Partial Pressure |
| A container has 3.40 g of N2 gas and an unknown mass of CO2 gas. If the partial pressure of the CO2 is twice that of the N2, then what is the mass of the CO2 gas in the container? |
| Find the molecular weights of N2 and CO2.
N2= 14.2 * 2= 28 g/mol CO2= 44 g/mol |
| We know from the problem that the container has 3.40 g of N2
gas. Convert that to moles using its molecular weight.
3.40 g N2 * mol/ 28 g N2= .12 mol N2 Here's what it looks like if you write it on paper. |
| We know from the problem that the partial pressure of CO2
is twice that of N2.
Multiply the last answer by 2. .12 * 2= .24 mol CO2 |
| Convert the above answer to grams of CO2. To do that, use
the molecular weight of CO2 we found earlier.
.24 mol CO2 * 44 g CO2/ mol= 10.56 g CO2 Here's what it looks like if you write it on paper. |
| Something to remember from this problem: volume and pressure are inversely proportional. |
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