1) A gas has a volume of 4.00 L at 0°C. What final temperature in degrees Celsiu

Question

1) A gas has a volume of 4.00 L at 0°C. What final temperature in degrees Celsius is needed to change the volume of the gas to 1.50 L if P and N do not change.
2) Calculate the final temperature of the gas in degrees Celsius when initial pressure is changed with V and n constant. A tank of helium gas with a pressure of 250 torr at 0°C is heated to give a pressure of 1500 torr.
3)The molar volume of a gas at STP(0°C,1atm) is 22.4 L. Calculate the volume in liters occupied by 2.50 moles of N2 gas at STP. Molar mass of N2=28.02g
4) A 0.226-g sample of carbon dioxide CO2 has a volume of 525 mL and a pressure of 455mmHg. What is the temperature in kelvin's and degrees Celsius of the gas? Molar mass of CO2=44.01 g 1) A gas has a volume of 4.00 L at 0°C. What final temperature in degrees Celsius is needed to change the volume of the gas to 1.50 L if P and N do not change.
2) Calculate the final temperature of the gas in degrees Celsius when initial pressure is changed with V and n constant. A tank of helium gas with a pressure of 250 torr at 0°C is heated to give a pressure of 1500 torr.
3)The molar volume of a gas at STP(0°C,1atm) is 22.4 L. Calculate the volume in liters occupied by 2.50 moles of N2 gas at STP. Molar mass of N2=28.02g
4) A 0.226-g sample of carbon dioxide CO2 has a volume of 525 mL and a pressure of 455mmHg. What is the temperature in kelvin's and degrees Celsius of the gas? Molar mass of CO2=44.01 g 1) A gas has a volume of 4.00 L at 0°C. What final temperature in degrees Celsius is needed to change the volume of the gas to 1.50 L if P and N do not change.
2) Calculate the final temperature of the gas in degrees Celsius when initial pressure is changed with V and n constant. A tank of helium gas with a pressure of 250 torr at 0°C is heated to give a pressure of 1500 torr.
3)The molar volume of a gas at STP(0°C,1atm) is 22.4 L. Calculate the volume in liters occupied by 2.50 moles of N2 gas at STP. Molar mass of N2=28.02g
4) A 0.226-g sample of carbon dioxide CO2 has a volume of 525 mL and a pressure of 455mmHg. What is the temperature in kelvin's and degrees Celsius of the gas? Molar mass of CO2=44.01 g
2) Calculate the final temperature of the gas in degrees Celsius when initial pressure is changed with V and n constant. A tank of helium gas with a pressure of 250 torr at 0°C is heated to give a pressure of 1500 torr.
3)The molar volume of a gas at STP(0°C,1atm) is 22.4 L. Calculate the volume in liters occupied by 2.50 moles of N2 gas at STP. Molar mass of N2=28.02g
4) A 0.226-g sample of carbon dioxide CO2 has a volume of 525 mL and a pressure of 455mmHg. What is the temperature in kelvin's and degrees Celsius of the gas? Molar mass of CO2=44.01 g

Explanation / Answer

Hello, hope this helps you

1) Combined equation for gases: (P1xV1)/(n1xT1) =(P2xV2)/(n2xT2) , you use the elements you need each time, the constants obviously are not included when not needed, this will help you with many gas problems.

For this problem:
V1/T1 = V2/T2 ...............................always remember to convert temperature to Kelvin to work with this equation, I used K = °C + 273 (obviously you cannot divide by zero, this problem teachs you to remember this convertion)

4L/273K = 1.5L/T2
Doing the math it gives you 443.625 K ---> 170.625 °C

2) P1/T1 = P2/T2 ....Note: you could convert torr to atm BUT in this case is not necessary because torr gets eliminated with torr at the other side of the equation, it is necessary however when you use R (the universal gas constant because this constant has the atm unit, and it is easier to convert your pressure units than to convert the constant to torr)

250torr/273K = 1500torr/T2

T2= 1638 K ----> 1365 °C

3) This is quite simple, you could use the universal gas formula (PV=nRT) but it is not necessary because the gas is at STP conditions.

Like this: 1 mole of gas at STP-----22.4 L

2.5 moles of gas at STP--X

X = (22.4 L x 2.5 moles)/1mol = 56 L .....you can double check the result using the universal equation

4) PV = nRT ............R = 0.082 atm.L / K.mol
   T = (PV)/(nR)

T= 0.6 atm x 0.525 L / 5.13x10-3moles x 0.082 atm.L/K.mol
   T = 748 K -----> 475 °C

Hope this can help you, regards.

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