A scientist collects 0.24 mole of hydrogen gas in a balloon. The temperature of the hydrogen is 35°C, and the pressure in the balloon is 1.05 atmospheres. What is the volume of the balloon?

5.77 L

Solution:

Data Given:

Moles = n = 0.24 mol

Temperature = T = 35 °C + 273 = 308 K

Pressure = P = 1.05 atm

Volume = V = ?

Formula Used:

Let's assume that the hydrogen gas in balloon is acting as an Ideal gas, the according to Ideal Gas Equation,

P V = n R T

where; R = Universal Gas Constant = 0.082057 atm. L. mol⁻¹. K⁻¹

Solving Equation for V,

V = n R T / P

Putting Values,

V = (0.24 mol * 0.082057 atm. L. mol⁻¹. K⁻¹ * 308 K) : 1.05 atm

V = 5.77 L

5.78

Explanation:

Volume of the balloon is 5.78 L.

Solution: - There are 0.24 moles of hydrogen gas in a balloon at 35 degree C and 1.05 atm pressure. It asks to calculate the volume of the balloon.

This problem is based on ideal gas law equation:

P = 1.05 atm, n = 0.24 mole, T = 35 + 273 = 308 K

R =

V = ?

The equation could be rearranged for the volume as:

Let's plug in the values and do the calculations to get the volume of the balloon:

V = 5.78 L

So, the volume of the gas balloon is 5.78 L.