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C) Pressure is not affectea. ime of a quarter mol of ideal gas at standard conditions...
At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 65 ∘C? Express your answer numerically in liters.
Assuming that the behavior of the gas is ideal. How much pressure would exercise 0.0468g of NH3 (molecular mass = 17 g / mol) on the walls of a container from 4.00L to 35.0oC? a) 0.0174 atm b) 0.296 atm c) 0.00198 atm d) 0.278 atm A sample of an unknown gas was added to a flask. It was heated in a water bath up to 100oC. When weighing the flask, the difference in weight was 0.504g and the volume...
At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 75 ∘C ?
At 273 K, 1.00 mol of an ideal gas confined to a 2.00-L container exerts a pressure of 11.2 atm. Under the same conditions, what pressure is exerted by CO2, for which a = 3.59 L2 atm mol-2 and b = 0.0427 L mol-1 0 -0.90 10.5 09.1 O 7.2 11.4
1. what is the volume of a gas in linters under the following conditions, 4.59 mol of gas, with a pressure of 1.09 atm at a temperature of 35 degrees C. 2. what is the pressure of a gas in atm under the follwing conditions? 32.6 g of chlorine gas, at a temperature of 398 K, whose volume equals 1.62 Liters.
Find the volume of 4.50 mol of an ideal gas at 25.0°C and a pressure of 419 kPa. Use the ideal gas law and R = 0.0821 atm • L/mol • K.
1. What volume is occupied by 1 mol of an ideal gas at a temperature of O°C and a pressure of 1 atm? Ans: 22.4 L
1) If 97.5 mol of an ideal gas occupies 28.5 L at 17.00 ∘C, what is the pressure of the gas? 2) If 3.04 mol of an ideal gas has a pressure of 2.72 atm and a volume of 63.53 L, what is the temperature of the sample in degrees Celsius? 3) What volume is occupied by 0.716 mol of CO2 at 200.8 K and 869 mmHg?
1.Ideal Gas Law PV = nRT with atm: R = 0.0821 L*atm/(K*mol) If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 2. If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 3. If I have 7.7 moles of gas at a pressure of 0.09...
Find the volume of 2.50 mol of an ideal gas at 26.0 °C and a pressure of 413 kPa Use the ideal gas law and R = 0.0821 atm l/mol k.