Question

At a constant pressure, 200g H2O is heated from 283 to 293K. The Cp of water is 75.3 J/mol*K. What is the entropy change?

a) 0.251 J/K
b) 0.502 J/K
c) 1.005 J/K
d) 2.010 J/K

Answer 1

The entropy change is 0.251 J/K.

Step-by-step explanation:

To determine the entropy change, we can use the formula ΔS = nCpΔT, where ΔS is the entropy change, n is the number of moles of the substance, Cp is the molar heat capacity, and ΔT is the temperature change. In this case, we are given that the mass of water is 200g, so we need to convert it to moles:

Number of moles of water = mass / molar mass = 200g / 18g/mol = 11.11 mol

Using the formula, ΔS = nCpΔT = 11.11 mol × 75.3 J/mol*K × (293K - 283K) = 0.251 J/K

Therefore, the entropy change is 0.251 J/K.