Multiple Choice
A sample of nitrogen gas has a pressure of 986 torr at 186°C. Assuming the volume and amount of gas remain constant, at what temperature in °C will the sample of gas have a pressure of 685 torr?
7. Gases
Chemistry Gas Laws
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
In an underground gas reserve, a bubble of methane gas (CH₄) has a volume of 45.0 mL at 1.60 atm pressure. What volume, in milliliters, will the gas bubble occupy when it reaches the surface where the atmospheric pressure is 744 mmHg, if there is no change in temperature?
A
36.0 mL
B
54.0 mL
C
60.0 mL
D
45.0 mL
Verified step by step guidance1
Identify the given values: initial volume \( V_1 = 45.0 \text{ mL} \), initial pressure \( P_1 = 1.60 \text{ atm} \), and final pressure \( P_2 = 744 \text{ mmHg} \).
Convert the final pressure from mmHg to atm for consistency in units. Use the conversion factor: \( 1 \text{ atm} = 760 \text{ mmHg} \). Calculate \( P_2 \) in atm.
Apply Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure and volume are inversely proportional: \( P_1 \times V_1 = P_2 \times V_2 \).
Rearrange the equation to solve for the final volume \( V_2 \): \( V_2 = \frac{P_1 \times V_1}{P_2} \).
Substitute the known values into the equation and solve for \( V_2 \) to find the volume of the gas bubble at the surface.
Related Videos
Related Practice
Chemistry Gas Laws practice set
Problem sets built by lead tutorsExpert video explanations