An empty water bottle is full of air at 15°c and standard pressure. the volume of the bottle is 0.500 liter. how many moles of air are in the bottle?

- 0.0211 moles of air.

Solution:- This problem is based on an ideal gas law equation.

temperature, pressure and volume are given and asked to calculate the moles of the air. Standard pressure is 1.00 atm.

T = 15 + 273 = 288 K

P = 1.00 atm

V = 0.500 L

The ideal gas law equation is, PV = nRT

where R is the universal gas law constant and its value is 0.0821 atm.L per mol per K.

n is the number of moles and its what we are asked to calculate.

For n, the equation is rearranged as:

Let's plug in the values and do the calculations:

n = 0.0211 moles

So, there are 0.0211 moles of the air in the bottle.

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .