Question

Can someone help me answer these chemistry problems?

1. How many moles of helium are required to fill a 5.10 L balloon to a pressure of 1.1 atm at 22 degrees C? Show your work to receive full credit.

2. If there are 4.00 moles of a gas at a pressure of 5.60 atm and a volume of 12.0 liters, what is the temperature? Show your work to receive full credit.

3. 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? Show your work to receive full credit.

4. You are given a 3.00 mol sample of krypton with a volume of 7.00 L. The temperature is held at 300. K. What is the pressure of the krypton sample? Show your work to receive full credit.

5. The air at the top of Mount Everest has pressures of 201.0 torr N2, 50.0 torr O2, 2.0 torr Ar, and 0.5 torr CO2. What is the total air pressure at the top of the highest peak in the world? Show all work to receive full credit.

6. A mixture of 1.20 mols He, 2.40 mols Ne, 4.80 mols Kr, and 0.60 mols Ar has a total pressure of 600.0 mm Hg. What is the partial pressure of the Kr? Show all work to receive full credit.

Answer 1

Q.1

To calculate moles of helium (n)=?

given

p=1.1 Atm

V=5.10 L

T =22°C

R =8.314 (universal gas constant)

Now use,

PV = nRT

1.1×5.10 =n×8.314×22

n= 5.61÷182.9

n= 0.030 moles

Use the same method to solve further questions!