Multiple Choice
A 4.30 L gas has a pressure of 7.0 atm when the temperature is 60.0 ºC. What will be the temperature of the gas mixture if the volume and pressure are decreased to 2.45 L and 403.0 kPa respectively?
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11 Gases
Chemistry Gas Laws: Combined Gas Law
Multiple Choice
A sealed container with a movable piston contains a gas with a pressure of 1380 torr, a volume of 820 mL and a temperature of 31°C. What would the volume be if the new pressure is now 2.83 atm, while the temperature decreased to 25°C?
A
0.0253 L
B
0.167 L
C
0.326 L
D
0.516 L
E
1.46 L
Verified step by step guidance1
First, convert all units to the appropriate SI units. Convert the initial pressure from torr to atm using the conversion factor: 1 atm = 760 torr. Use the formula: \( P_{\text{atm}} = \frac{P_{\text{torr}}}{760} \).
Convert the initial volume from mL to L using the conversion factor: 1 L = 1000 mL. Use the formula: \( V_{\text{L}} = \frac{V_{\text{mL}}}{1000} \).
Convert the temperatures from Celsius to Kelvin using the formula: \( T_{\text{K}} = T_{\text{°C}} + 273.15 \). Apply this to both the initial and final temperatures.
Use the combined gas law to find the new volume. The combined gas law is \( \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \). Rearrange the formula to solve for \( V_2 \): \( V_2 = \frac{P_1 V_1 T_2}{P_2 T_1} \).
Substitute the converted values into the rearranged formula to calculate the new volume \( V_2 \).
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