Question

if we add 800 j of heat to 9 moles of an ideal monatomic gas at constant volume, what will be the change in temperature of the gas? (r

Answer 1

To find the change in temperature of the gas, we can use the equation:

ΔQ = nCvΔT

Where:

ΔQ is the change in heat energy (in joules)

n is the number of moles of the gas

Cv is the molar specific heat capacity at constant volume (for a monatomic gas, Cv = (3/2)R)

ΔT is the change in temperature

Given:

ΔQ = 800 J

n = 9 moles

Cv = (3/2)R (since it's a monatomic gas)

R is the ideal gas constant (approximately 8.314 J/(mol·K))

Substituting the given values into the equation, we have:

800 J = 9 * (3/2)R * ΔT

Simplifying, we get:

800 J = (27/2)R * ΔT

Now we can solve for ΔT:

ΔT = (800 J) / ((27/2)R)

ΔT = (800 J) / ((27/2) * 8.314 J/(mol·K))

ΔT ≈ 11.3 K

Therefore, the change in temperature of the gas is approximately 11.3 Kelvin.