Question

A gas 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?

Answer 1

Answer: 0.129 moles of gas were added to the bottle

Step-by-step explanation:

According to the ideal gas equation:'

`PV=nRT`

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

`(P_1)/(n_1)=(P_2)/(n _2)`

where,

`P_1` = initial pressure of gas =730 mm Hg =0.960 atm (760 mmHg = 1 atm)

`P_2` = final pressure of gas = 1.15 atm

`n_1` = initial number of moles = 0.650

`n_2` = final number of moles = ?

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

`(0.960)/(0.650)=(1.15)/(n_2)`

`n_2=0.779`

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