Question

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?

Answer 1

Answer:

              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

Answer 2

The temperature of the hydrogen is 35°C, and the pressure in the balloon is 1.05 atmospheres, the volume of the balloon will be 5.77 L

What is volume?

Volume is the space occupied by an object.

Given the Moles  =  n  =  0.24 mol

Temperature  =  T  =  35 °C + 273  =  308 K

Pressure  =  P  =  1.05 atm                

Volume  =  V  is to find

By ideal gas law

PV = nRT

Where R = universal gas constant 0.082057 atm      

         

$V = \dfrac{n R T }{P}$

Putting values in the equation

$V = \dfrac{0.24 \times 0.082057 \times 308 K }{1.05} = 5.77 L$

           

Thus, the volume of the balloon will be 5.77 L.

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