Question

fill in the missing words
the gas pressure of a mixture of oxygen, nitrogen and carbon dioxide is 0.950 atm. the partial pressure of oxygen is 123 mm hg, the partial pressure of nitrogen is 541 mm hg. the partial pressure of carbon dioxide is
mm hg. the percentages of the gases in the mixture are
% (nitrogen),
% (oxygen),
% (carbon dioxide).

Explanation:

Step1: Convert total pressure to mmHg

1 atm = 760 mmHg, so 0.950 atm = 0.950×760 mmHg = 722 mmHg.

Step2: Calculate partial pressure of CO₂

According to Dalton's law of partial pressures $P_{total}=P_{O_2}+P_{N_2}+P_{CO_2}$. So $P_{CO_2}=P_{total}-P_{O_2}-P_{N_2}=722 - 123-541=58$ mmHg.

Step3: Calculate percentage of nitrogen

Percentage of nitrogen $=\frac{P_{N_2}}{P_{total}}\times100=\frac{541}{722}\times100\approx74.93\%$.

Step4: Calculate percentage of oxygen

Percentage of oxygen $=\frac{P_{O_2}}{P_{total}}\times100=\frac{123}{722}\times100\approx17.04\%$.

Step5: Calculate percentage of carbon - dioxide

Percentage of carbon - dioxide $=\frac{P_{CO_2}}{P_{total}}\times100=\frac{58}{722}\times100\approx8.03\%$.

Answer:

58; 74.93; 17.04; 8.03