Q. 8.63 - An Introduction to General, Organic, and Biological Chemistry

Question

Two flasks of equal volume and at the same temperature contain different gases. One flask contains $10.0g$ of $He$. Is each of the following statements true or false? Explain.$(8.1)$

a. The flask that contains $He$ has a higher pressure than the flask that contains $Ne$.

b. The densities of the gases are the same.

Step-by-Step Solution

Answer

a. The statement the flask that contains $He$ has a higher pressure than the flask that contains $Ne$ is  false.

b. The statement the densities of the gases are the same is true.

Part (a) step 1: Given Information

We need to find the given statement the flask that contains $He$has a higher pressure than the flask that contains $Ne$ is true or false.

Part (a) step 2: Simplify

Here,

From $PV=nRT$

So, $V$ and $T$ is the same for both the gases.

$n=\raisebox{1ex}{$mass$}\!\left/ \!\raisebox{-1ex}{$molar mass$}\right.$

mass is also the same therefore, the pressure depends on the inverse of molar mass. And the molar mass of $Ne$ is more than $He$ therefore, it has less pressure in the flask.

So, the statement is false.

Part (b) step 1: Given Information

We need to find the given statement the densities of the gases are the same is true or false.

Part (b) step 2: Simplify

Each gas has the same mass in the same volume therefore, it has the same mass density too.

So, the statement is true.