9. What is the volume occupied by 1.24 mol of a gas at 35°C if the pressure is 96.2 kPa?

The answer to your question is V = 33 L

Explanation:

Data

R = 0.082 atm L / mol°K

Volume = ?

moles = 1.24

Temperature = 35°C = 273 + 35 = 308°K

Pressure = 96.2 kPa

Process

1.- Convert kPa to atm

               1000 Pa 1 kPa

                     x        96.2 kPa

                    x = (96.2 x 1000) / 1

                    x = 96200 Pa

                1 atm 101325 Pa

                x         96200 Pa

                x = (96200 x 1) / 101325

                x = 0.949 atm

2.- Substitute in the Ideal gas law

       PV = nRT

- Solve for V

         V = nRT / P

         V = (1.24)(0.082)( 308) / 0.949

3.- Result

         V = 31.32 / 0.949

         V = 33 L              

33.0 L is occupied

Explanation:

Step 1: Data given

Number of moles of the gas = 1.24 moles

Temperature = 35.0 °C  = 308 K

Pressure = 96.2 kPa = 0.9494202 atm

Step 2: Calculate volume

p*V = n*R*T

⇒ with p= The pressure = 0.9494202 atm

⇒ with V= The volume of the gas = TO BE DETERMINED

⇒with n = The moles of gas = 1.24 moles

⇒with R = the gas constant = 0.08206 L*atm/K*mol

⇒with T = the temperature = 308 K

V = (n*R*T) / p

V = (1.24 * 0.08206 * 308) / 0.9494202

V = 33.0 L

33.0 L is occupied

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radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.