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.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

a