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2. A certain amount of gas at 35 C and at a pressure of 0.900 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 1.50 atm. How high can you raise the temperature of the gas without bursting the vessel? 3. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.

2. A certain amount of gas at 35 C and at a pressure of 0.900 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 1.50 atm. How high can you raise the temperature of the gas without bursting the vessel? 3. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter8: Gases
Section: Chapter Questions
Problem 31Q
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l activities s ely understand, address and resolve iss forces and energy by means of explaii communities. (LPO 2, EPO 2. Take the risk of e test pot- 2. A certain amount of gas at 35 C and at a pressure of 0.900 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 1.50 atm. How high can you raise the temperature of the gas without bursting the vessel? 3. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases. ROCESSING QUESTIONS: How is ideal gas law different from the previous laws?
Transcribed Image Text:l activities s ely understand, address and resolve iss forces and energy by means of explaii communities. (LPO 2, EPO 2. Take the risk of e test pot- 2. A certain amount of gas at 35 C and at a pressure of 0.900 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 1.50 atm. How high can you raise the temperature of the gas without bursting the vessel? 3. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases. ROCESSING QUESTIONS: How is ideal gas law different from the previous laws?
WEEK 2 ACTIVITY 3 IDEAL AND PARTIAL In the previous activity, we deal with individual gas laws. In this activity, we will combine those laws and simplify it to become ideal gas law. Dalton's Law is a different statement since it talks about the partial pressures of a gas in a container. Ideal gas law combines the relationship of the previous laws discussed in the previous activity. It is simplified as PV = nRT Where P, V, n, and T are pressure, volume, amount of substance, and temperature, respectively. R is the L·atm proportionality constant whose value is 0.0821 mol·K On the other hand, Dalton's Law of Partial Pressures the total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone. Generally, it is given by Pr = P + P, + P3 + .…. Let us answer the activity that follows. DIRECTIONS: Answer the given word problems. SHOW YOUR SOLUTION. 1. A sample of nitrogen gas is kept in a container of volume 4.5 L and at a temperature of 35 C exerts a pressure of 3.2 atm. Calculate the number of moles of gas present. 008
Transcribed Image Text:WEEK 2 ACTIVITY 3 IDEAL AND PARTIAL In the previous activity, we deal with individual gas laws. In this activity, we will combine those laws and simplify it to become ideal gas law. Dalton's Law is a different statement since it talks about the partial pressures of a gas in a container. Ideal gas law combines the relationship of the previous laws discussed in the previous activity. It is simplified as PV = nRT Where P, V, n, and T are pressure, volume, amount of substance, and temperature, respectively. R is the L·atm proportionality constant whose value is 0.0821 mol·K On the other hand, Dalton's Law of Partial Pressures the total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone. Generally, it is given by Pr = P + P, + P3 + .…. Let us answer the activity that follows. DIRECTIONS: Answer the given word problems. SHOW YOUR SOLUTION. 1. A sample of nitrogen gas is kept in a container of volume 4.5 L and at a temperature of 35 C exerts a pressure of 3.2 atm. Calculate the number of moles of gas present. 008
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