1) for Gas A:
Given:
V = 5.06 L
n = 1.92 mol
T = 35.0 oC
= (35.0+273) K
= 308 K
use:
P * V = n*R*T
P * 5.06 L = 1.92 mol* 0.08206 atm.L/mol.K * 308 K
P = 9.5903 atm
= 9.5903*101.33 kPa
= 972 kPa
Answer: 972 kPa
2) for Gas B:
Given:
V = 5.06 L
n = 3.25 mol
T = 35.0 oC
= (35.0+273) K
= 308 K
use:
P * V = n*R*T
P * 5.06 L = 3.25 mol* 0.08206 atm.L/mol.K * 308 K
P = 16.2336 atm
= 16.2336*101.33 kPa
= 1645 kPa
Answer: 1645 kPa
A 5.06 L cylinder contains 1.92 mol of gas A and 3.25 mol of gas B,...
A 7.86-L cylinder contains 1.70 mol of gas A and 3.63 mol of gas B, at a temperature of 33.8 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior. PA= PB= What is the total pressure? Ptotal= Answers in kPa.
A 6.40 L cylinder contains 2.62 mol of gas A and 3.07 mol of gas B, at a temperature of 33.3 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior.
(III) If 3.25 L of gas at 16.0 °C and 1.00 atm is compressed at a pressure of 125 atm at 20.0 °C, calculate the new volume of the gas. (IV) Calculate its volume (in liters) of 88.4 g of CO2 at STP. (V) H20 and CH4 are gases at 150 °C. Which exhibits more ideal behavior? Why? (VI) Assume that you have a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if...
Question 6 of 17 > A gas cylinder contains 1.50 mol He, 1.00 mol Ne, and 1.65 mol Ar. If the total pressure in the cylinder is 2430 mmHg, what is the partial pressure of each of the components? Assume constant temperature. mmHg mmHg mmHg
11. A gas cylinder contains 35.0 L of nitrogen gas at a temperature of 24.6°C and a pressure of 1.95 atm. How many moles of nitrogen gas are in the cylinder? 12. How much faster does He gas diffuse than N2 gas? Assume their temperature is constant.
A cylinder contains 12.8 L of air at a total pressure of 43.0 psi and a temperature of 35 ∘C. How many moles of gas does the cylinder contain? (Hint: You must convert each quantity into the correct units (L, atm, mol, and K) before substituting into the ideal gas law.)
A cylinder contains 12.4 L of air at a total pressure of 41.4 psi and a temperature of 35 ∘C. How many moles of gas does the cylinder contain? (Hint: You must convert each quantity into the correct units (L, atm, mol, and K) before substituting into the ideal gas law.)
A cylinder contains 0.250 mol of carbon dioxide (CO2) gas at a temperature of 27.0∘C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm on the gas. The gas is heated until its temperature increases to 127.0∘C. Assume that the CO2 may be treated as an ideal gas. How much work W is done by the gas in this process? What is the change in internal energy ΔU of the gas? How much...
A cylinder contains 0.300 mol of carbon dioxide (CO2)gas at a temperature of 23.0 ∘C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm on the gas. The cylinder is placed on a hot plate and a 920 J of heat flows into the gas, thereby raising its temperature to 130 ∘C. Assume that the CO2 may be treated as an ideal gas. 1. What is the change in internal energy of the...
A cylinder witha movable piston contains an ideal gas. Both the amount of gas and the volume of the container can be adjusted, but the temperature remains constant at 300.0 K. Use the ideal gas law and the individual gas law relationships to answer the questi ons below. L x atm nRT where R = 0.08206 PV mol xK 1st attempt See Periodic Table See Hint Part 1 (1 point) Calculate the number of moles of the gas in the...