1 . A gas is put into a 4.3 L cylinder under 2.07 atm at -55°C. The gas is compr

Question

1. A gas is put into a 4.3 L cylinder under 2.07 atm at -55°C. The gas is compressed to 1.09 L while heated to 388°C. What is the final pressure of the gas?

2. 2.98 L of helium at 18°C has a pressure of 2.01 atm. What will the temperature be if the pressure increases to 2.75 atm while the volume drops to 1.03 L?

3. 8.10 L of nitrogen has at 302 K has a pressure of 1.92 atm. If the pressure changes to 2.53 atm and the temperature cools to 138 K, what will the new volume be?

4. 3.109 L of gas at 22 degrees Celcius is heated to 109 degrees Celcius. While the pressure is held at 1928 mm Hg, what will the new volume of gas be?

Explanation / Answer

Ans 1 :

Using the ideal gas law , pV = nRT , the relation between p , V and T can be determined as :

p1V1T2 = p2V2T1

T1 = -55 degrees C = 218.15 K

T2 = 388 degrees C = 661.15 K

Putting all the values we get :

2.07 x 4.3 x 661.15 = p2 x 1.09 x 218.15

p2 = 24.75 atm

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