To find the pressure of the gas, you can use the Ideal Gas Law, which is given by the equation:
\[ PV = nRT \]
Where:
- \( P \) = pressure (atm)
- \( V \) = volume (L)
- \( n \) = number of moles (mol)
- \( R \) = ideal gas constant (0.0821 L atm / mol K)
- \( T \) = temperature (K)
Given:
- \( n = 6.1 \) moles
- \( V = 24.8 \) L
- \( T = 280 \) K
- \( R = 0.0821 \) L atm / mol K
Now, rearranging the Ideal Gas Law to solve for pressure \( P \):
\[ P = \frac{nRT}{V} \]
Substituting in the values:
\[ P = \frac{(6.1 , \text{mol}) \times (0.0821 , \text{L atm / mol K}) \times (280 , \text{K})}{24.8 , \text{L}} \]
Calculating the numerator:
\[ (6.1) \times (0.0821) \times (280) = 142.2846 \]
Now, divide this by \( 24.8 \):
\[ P = \frac{142.2846}{24.8} \approx 5.73 , \text{atm} \]
Rounding to two decimal places, we find:
\[ P \approx 5.7 , \text{atm} \]
Thus, the correct answer is:
D. 5.7 atm