What is the molar mass of a gas that has a density of 1.18g/L at 25°C and 1 atm?

Answer 1

You can get this from the Ideal Gas Law.

We are going to solve this by first figuring out what the volume of one mole of a gas is at #25^o#C and 1 atm. Once we know how many liters of gas we need for one mole, we will be able to figure out how many grams of gas are in one mole, given the gas density.

First, let's review the Ideal Gas Law: PV=nRT.

For 1 mole of a gas, n=1. You are at (#25^o#C) and 1 atm. R = 0.082057 liter-atm/mol-K.

In order to solve PV=nRT for V, we get V=nRT/P = 24.453 liters.

Thus, we now know that one mole will require 24.453 liters of gas, which will weigh:

11.8 g/liter times 24.453 liters is 28.854 grams per mole.

3 significant figures adjusted: 28.9 grams per mole.

The Ideal Gas Law helped us determine how many liters of gas were required to produce one mole, which was the crucial step.

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Answer 2

Naomi Aronson

The molar mass of the gas is approximately 29.1 g/mol.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.