Question

A gas evolved during the fermentation of alcohol had a volume of 19.4 L at 17 °C and 746 mmHg. How many moles of gas were collected?

Answer 1

Answer:- 0.800 moles of the gas were collected.

Solution:- Volume, temperature and pressure is given for the gas and asks to calculate the moles of the gas.

It is an ideal gas law based problem. Ideal gas law equation is used to solve this. The equation is:

PV=nRT

Since it asks to calculate the moles that is n, so let's rearrange this for n:

`n=(PV)/(RT)`

V = 19.4 L

T = 17 + 273 = 290 K

P = 746 mmHg

we need to convert the pressure from mmHg to atm and for this we divide by 760 since, 1 atm = 760 mmHg

`P=746mmHg((1atm)/(760mmHg))`

P = 0.982 atm

R =
`0.0821(atm.L)/(mol.K)`

Let's plug in the values in the equation to get the moles.

`n=(0.982atm*19.4L)/(0.0821(atm.L)/(mol.K)*290K)`

n = 0.800 moles

So, 0.800 moles of the gas were collected.