What would be the volume of a balloon at the summit of Mt. Everest (P = 0.33 atm

Question

What would be the volume of a balloon at the summit of Mt. Everest (P = 0.33 atm) if it had begun as a 4.50 l balloon at sea level (1.00 atm)? (Assuming T is constant ellipsis) If a 2.50 l balloon at 0 degree C were heated to 85.0 degree C, what would its new volume be? A gas has a volume of 4.00 lat 20.0 degree C and a pressure of 1.50 atm. What is its pressure if the volume is decreased to 1.25 l and its temperature is increased to 60.0 degree C? How many moles of N_2 (g) are in a 100.0 ml container at a pressure of 74.5 atmospheres and a temperature of 32.0 degree C? H_2 is collected over water in a closed container at an atmospheric pressure (P_r)of 748 mm Hg at 21.0 degree C. If the vapor pressure (P_) at this temperature is 18.65 mm Hg, what is the pressure of the dry H_2 gas PH_2)? According to the equation, KCIO_3 (s) rightarrow KCl(s) +O_2(g) how many milliliters of O_2 could be formed from the decomposition of 5.00 g of KCIO_3 at a temperature of 22.0 degree C and a pressure of 1.00 atm?

Explanation / Answer

1.   Since temperature is constant assuming gas to be ideal we can apply boyles law

I.e. p1V1 = p2v2

1*4.5 = 0.33*v2   

Hence v2=13.636L

2. Assuming pressure to be constant and gas to be ideal

Using charles law

V1/v2. =T1/T2 (temp must be in Kelvin)

2.5/v2. =. 273/358. (Since Tk. =Tc +273)

V2=. 3.278L

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