**Question**

The temperature of a sample of an ideal gas confined in a 2.0 L container was raised from 27 °C to 77 °C. If the initial pressure of the gas was 1200 mm Hg, what was the final pressure of the gas?

**Solution**

Step 1

Convert temperatures from Celsius to Kelvin

K = °C + 273

Initial temperature (T_{i}): 27 °C

K = 27 + 273

K = 300 Kelvin

T_{i} = 300 K

Final temperature (T_{f}): 77 °C

K = 77 + 273

K = 350 Kelvin

T_{f} = 350 K

**Step 2**

Using the ideal gas relationship for constant volume, solve for the final pressure (P_{f})

P_{i} / T_{i} = P_{f} / T_{f}

solve for P_{f}:

P_{f} = (P_{i} x T_{f}) / T_{i}

P_{f} = (1200 mm Hg x 350 K) / 300 K

P_{f} = 420000 / 300

P_{f} = 1400 mm Hg

**Answer**

The final pressure of the gas is 1400 mm Hg.