Solving Gas Law Problems: Partial Pressure & Relative Diffusion Rates

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To solve the gas law problem regarding partial pressures, one must convert the weights of carbon dioxide and ammonia into moles, as partial pressures are proportional to their molar fractions. For the second question about relative diffusion rates, Graham's law can be applied, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molecular weight. Given that the relative rate of diffusion is 1.89 and the molecular weight of methane is 16, the molecular weight of the other gas can be calculated using the formula derived from Graham's law. Understanding these concepts is essential for solving gas law problems effectively. Mastery of these principles will enhance comprehension of gas behavior in mixtures.
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heres a partial pressure one:
1. A mixture of gases containing equal weights of carbon dioxide, CO, and ammonia exerts an overall pressure of 450 torr. What pressure is exerted by each gas individually?

my last question is:
2. The relative rate of diffusion between two gases is 1.89. If the lighter gas is methane (mw=16), what is the molecular weight of the other gases?

for the first one, I could probably guess and check to get my answer, but i wouldn't understand it overall. For the second one, my teacher didn't even go over rates and that stuff. Mind explaining to me how to get the answer? thank you.
 
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1. Convert weights to moles. Partiall pressures are proportional to molar fractions.

2. Graham's law

Please note, that you should use homework template, when asking homework questions.
 

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