Hydrogen chloride gas is shipped in a container under 5,100 mmHg of pressure that occupies 20.1 liters at 29°C. How many liters of gas would be produced at STP? A. 1.7 x 10-5 L B.8.3 x 10-3 L C. 120 L D. 150 L

To calculate the volume of hydrogen chloride gas at standard temperature and pressure (STP), we need to use the ideal gas law and the combined gas law. The combined gas law is given by:

\[ P_1 \cdot V_1 / T_1 = P_2 \cdot V_2 / T_2 \]

Where: - \( P_1 \) and \( V_1 \) are the initial pressure and volume - \( T_1 \) is the initial temperature in Kelvin - \( P_2 \), \( V_2 \), and \( T_2 \) are the pressure, volume, and temperature at STP, respectively.

STP is defined as 0°C (273 K) and 1 atmosphere of pressure. 1 atmosphere is equivalent to 760 mmHg.

Given: - \( P_1 = 5100 \) mmHg - \( V_1 = 20.1 \) L - \( T_1 = 29 \)°C (which is 29 + 273 = 302 K) - \( P_2 = 760 \) mmHg (pressure at STP) - \( T_2 = 273 \) K (temperature at STP)

We can substitute these values into the combined gas law to find \( V_2 \):

\[ V_2 = (P_1 \cdot V_1 \cdot T_2) / (P_2 \cdot T_1) \]

\[ V_2 = (5100 \text{ mmHg} \cdot 20.1 \text{ L} \cdot 273 \text{ K}) / (760 \text{ mmHg} \cdot 302 \text{ K}) \]

\[ V_2 = (27675300 \text{ mmHg} \cdot L \cdot K) / (229520 \text{ mmHg} \cdot K) \]

\[ V_2 \approx 120.5 \text{ L} \]

So the volume of hydrogen chloride gas at STP would be approximately 120.5 liters.

Therefore, the correct answer is C. 120 L.