Questions: Determine the density of NH3 gas at 435 K and 1.00 atm. A) 0.851 g / L B) 0.321 g / L C) 0.477 g / L D) 2.10 g / L E) 2.24 g / L A sample of nitrogen gas had a volume of 500 mL, a pressure in its container of 740 Torr, and a temperature of 25°C. What was the new volume of the gas when the temperature was changed to 50°C and the new pressure was 760 Tom? A) 528 mL B) 408 mL C) 244 mL D) 452 mL E) 976 mL

\(\boxed{0.477 \, \text{g/L}}\)

To find the new volume of the nitrogen gas when the temperature and pressure change, we use the combined gas law:

\[ \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \]

where:

• \(P_1 = 740 \, \text{Torr}\),
• \(V_1 = 500 \, \text{mL}\),
• \(T_1 = 25^\circ \text{C} = 298 \, \text{K}\),
• \(P_2 = 760 \, \text{Torr}\),
• \(T_2 = 50^\circ \text{C} = 323 \, \text{K}\),
• \(V_2\) is the new volume.

Rearrange the equation to solve for \(V_2\):

\[ V_2 = V_1 \times \frac{P_1}{P_2} \times \frac{T_2}{T_1} \]

Substitute the given values into the equation:

\[ V_2 = 500 \, \text{mL} \times \frac{740 \, \text{Torr}}{760 \, \text{Torr}} \times \frac{323 \, \text{K}}{298 \, \text{K}} \]

Perform the calculation:

\[ V_2 = 500 \times 0.9737 \times 1.0839 \approx 528.1 \, \text{mL} \]

\(\boxed{528 \, \text{mL}}\)