Question

How many moles of an ideal gas is present in a 0.45 L sample of gas at 273 K and 0.50 atm pressure?(1 point)
Responses

50.37 mol
50.37 mol

99.6 mol
99.6 mol

0.01 mol
0.01 mol

0.00027 mol

Answer 1

To find the number of moles of an ideal gas, we can use the Ideal Gas Law, which is given by the equation:

\[
PV = nRT
\]

Where:
- \( P \) = pressure in atm (0.50 atm)
- \( V \) = volume in liters (0.45 L)
- \( n \) = number of moles of gas
- \( R \) = ideal gas constant (0.0821 L·atm/(K·mol))
- \( T \) = temperature in Kelvin (273 K)

We need to solve for \( n \):

\[
n = \frac{PV}{RT}
\]

Now substituting the values into the equation:

\[
n = \frac{(0.50 \, \text{atm}) \times (0.45 \, \text{L})}{(0.0821 \, \text{L·atm/(K·mol)}) \times (273 \, \text{K})}
\]

Calculating the denominator:

\[
0.0821 \, \text{L·atm/(K·mol)} \times 273 \, \text{K} \approx 22.4143 \, \text{L·atm/mol}
\]

Now substituting everything in:

\[
n = \frac{0.50 \times 0.45}{22.4143} \approx \frac{0.225}{22.4143} \approx 0.01004 \, \text{mol}
\]

So, the number of moles of gas present is approximately 0.01 mol.

The correct response is:

**0.01 mol**