A mixture of `N_2` and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 10 atm?

Explanation

To find the density of the gas mixture of \(N_2\) and Ne at 500 K and 10 atm, we can follow these steps:

### Step 1: Determine the Molar Mass of Each Gas
- The molar mass of nitrogen (\(N_2\)) is approximately 28 g/mol.
- The molar mass of neon (Ne) is approximately 20 g/mol.

### Step 2: Calculate the Molar Mass of the Mixture
Since the mixture contains equal moles of \(N_2\) and Ne, we can calculate the average molar mass of the mixture using the formula:
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