Question

calculate the entropy change when 0.02 mol of an ideal gas (Cv= 12.6 j/mol.k) is heated from 25⁰C to 100⁰C so that its volume is al

Answer 1

To calculate the entropy change for heating 0.02 mol of an ideal gas from 25℃ to 100℃, only the temperature change is considered due to lack of volume change information. The entropy change is determined using the formula ΔS = nCvln(T2/T1), with T in Kelvin.

Step-by-step explanation:

To calculate the entropy change when 0.02 mol of an ideal gas (Cv= 12.6 J/mol·K) is heated from 25℃ to 100℃ so that its volume is also changing, we use the formula for entropy change (ΔS) for an ideal gas given by:

ΔS = nCvln(T2/T1) + nRln(V2/V1)

However, since the problem does not provide information about the change in volume, the second term involving volume change cannot be calculated.

We will only focus on the temperature change part of the entropy change. Convert the temperatures from Celsius to Kelvin by adding 273.15, so T1 becomes 298.15 K and T2 becomes 373.15 K. Using the formula for entropy change with only temperature:

ΔS = nCvln(T2/T1)

Now plug in the values:

ΔS = 0.02 mol × 12.6 J/mol·K × ln(373.15 K / 298.15 K)

After calculating this, you will get the entropy change due to temperature increase for the ideal gas.