4. A 2.00 L balloon of gas at s0.0°C is cooled to 0,0°C. What is the new volume

Question

4. A 2.00 L balloon of gas at s0.0°C is cooled to 0,0°C. What is the new volume (liters) of the balloon? Ans: 1.69 Assume P & n are constant. 3 K 5. If the volume of a gas at 200°C changes from 1.75 L to 755 mL, what will be the final temperature in °C? Ans Assume P&n; are constant. 6. A balloon originally had a volume of 0.500 L at 80°C and a pressure of 729 torr. To what temperature Kelvin must the balloon cooled to reduce its volume to 250 mL, if the pressure remained constant? Assume P & n are constant Ans: 177K What happens to the volume of a gas when you quadruple the number of moles of gas while keeping the temperature and pressure constant? Show mathematically Ans: Quadruples dded to a balloon that started with 1.9 moles of gas and a volume of 1.0 L given that the final Ans: 5.7 mol 8. How many moles of gas were balloon that volume was 4.0 L? Hint: remember to subtract the starting moles of gas) Assume P &T; are constant. 9. If each of the following 10 gram gas sample are at STP, which sample has the greatest volume? Ans: Helium Neon, Helium, Argon 10. A gas cylinder contains only the gases radon, nitrogen, and oxygen. The radon has a pressure of 98 torr while the nitrogen has a pressure of 446 torr. If the total pressure inside the cylinder is 755 torr, what is the pressure that is due to the oxygen? Ans: 211 torr

Explanation / Answer

4)

we have:

V1 = 2.00 L

T1 = 50.0 oC

= (50.0+273) K

= 323 K

T2 = 0.0 oC

= (0.0+273) K

= 273 K

we have below equation to be used:

V1/T1 = V2/T2

2.00 L / 323.0 K = V2 / 273.0 K

V2 = 1.69 L

Answer: 1.69 L

5)

we have:

T1 = 200.0 oC

= (200.0+273) K

= 473 K

V1 = 1.75 L

V2 = 755.0 mL

= (755.0/1000) L

= 0.755 L

we have below equation to be used:

V1/T1 = V2/T2

1.75 L / 473.0 K = 0.755 L / T2

T2 = 204.0657 K

T2 = -68.9 oC

Answer: -68.9 oC

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