Agas bottle contains 0.650 mol of gas at 730 mm hg pressure. if the final pressure is 1.15 atm, how many moles of gas were added to the bottle?

0.779 mol

Explanation:

Since the gas is in a bottle, the volume of the gas is constant. Assuming the temperature remains constant as well, then the gas pressure is proportional to the number of moles:

so we can write

where

p1 = 730 mm Hg = 0.96 atm is the initial pressure

n1 = 0.650 mol is the initial number of moles

p2 = 1.15 atm is the final pressure

n2 is the final number of moles

Solving for n2,

0.129 moles of gas were added to the bottle

Explanation:

According to the ideal gas equation:'

P = Pressure of the gas

V= Volume of the gas

T= Temperature of the gas

R= Gas constant

n=  moles of gas

As Volume , gas constant and temperature are constant

where,

= initial pressure of gas =730 mm Hg =0.960 atm (760 mmHg = 1 atm)

= final pressure of gas = 1.15 atm

= initial number of moles = 0.650

= final number of moles =  ?

Now put all the given values in the above equation, we get the final moles of gas.

Therefore, the number of moles of gas will be 0.779

Thus moles of gas were added to the bottle are (0.779-0.650) = 0.129

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