Question

Question 4 of 21 

A sample of an ideal gas at 1.00 atm and a volume of 1.76 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 75.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

Questions of 21 

A hot air balloon is filled with 1.31 x 10 L of an ideal gas on a cool morning (11 'C). The air is heated to 115 'C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. volume:

Answer 1

Answer: 0 we used the Boyle's Laco. PU, = P₂ U2 - Constant P- Pressure vo Volume (P. Viinitial = (P242) Final 1.0 atum X 1.762 = 75.0 atm X U2 U2 = 1.0 atom x1.764 7500 atym V2 = 1.76 L = 0.023L 75.0 V2 = 0.023L We weed Charle's Law 7 2 = constant | V = v=volume T = Temperature (unk) (initial = ( 12 ) Final Ta = 11°C TIF 11+273.15 = 284.15k T2 = 115°C T2 = 113+2 73.15= 388.15K - 1.31x106L 284.15K V2 388.15K V2 1-31X106LX388.15k 284.Isk Uz 508.476X106 L 284. 15 1.789 x 106 L Uz = - 1.79 xlobl. Please rate it".