A hot-air balloon is aloft with a volume of 2,000 L when it is on the ground, at 25°C and 1.0 atm. The rope is let go, and the balloon rises rapidly, then it levels off. It is found that the temperature at this height is 35°C, and the volume has swollen to 2,500 L. What is the air pressure at this height? Remember that PV = nRT, and perform the calculation using temperature in K. Use the correct significant figures and units.
Chemistry Question! What Is The Air Pressure?
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2000L * 1.0atm = nR * 298K
nR = 2000/298
= 6.7114
2500x = 6.7114 * 308K
x = 0.82684 atm correctly rounded to 0.82 atm is the air pressure at this height.
At ground level, you have two variables you don’t know the n and the R. When the balloon rises, you don’t know the n, the R and the P, but since R and n don’t change you can calculate their values on the ground and apply them to when the balloon rises. So know all you don’t know is the pressure which you can easily calculate using the values you have.
Do your own damn homework from now on.