We are asked to find the **pressure in the canister containing argon gas **at the given conditions. Since mass, volume and temperature are given, we will use the **ideal gas equation** to calculate for pressure.

$\overline{){\mathbf{PV}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{nRT}}}$

P = pressure, atm

V = volume, L

n = moles, mol

R = gas constant = 0.08206 (L·atm)/(mol·K)

T = temperature, K

We will do the following steps to solve the problem:

Step 1: Calculate the moles of argon gas in the canister

Step 2: Calculate the pressure in the canister

**Step 1****: Calculate the moles of argon gas in the canister**

In the ideal gas equation, moles are needed but the mass of argon is given instead. We’ll** **calculate the moles of argon using the mass and its molar mass.

A wine-dispensing system uses argon canisters to pressurize and preserve wine in the bottle. An argon canister for the system has a volume of 59.6 mL and contains 30.1 g of argon.

Assuming ideal gas behavior, what is the pressure in the canister at 297 K ?

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