Calculate the change in entropy of the system when 10g of ice at -10c is converted into water vapor at 115c and at a constant pressure of 1bar. the constant pressure molar heat capacity of h2o(s) and h2o(l) is 75.291j/kmol and that of h2o(g) is 33.58j/kmo

Total change in entropy of the system is 85.84 J/K

Explanation:

Δ = Δ+Δ+Δ+Δ

Δ = total entropy of the system in J/K

Δ = entropy due to warming ice from - 10°C (263 K) to 0°C (273 K) in J/K

Δ = entropy due to melting of ice at 0°C (273 K) in J/K

Δ = entropy due to warming liquid from 0°C (273 K) to 115°C (388 K) in J/K

Δ = entropy due to vaporizing liquid at 115°C (388 K) in J/K

Therefore,

Δ = m**

m = mass = 10 g;   = specific heat of ice = 2.106 J/(g*K)

Δ = 10*2.106* = 0.79 J/K

Δ = m*/273

m = 10 g; = 334 J/g

Δ = 10*334/273 = 12.23 J/K

Δ = m**

m = mass = 10 g;   = specific heat of water = 4.218 J/(g*K)

Δ = 10*4.218* = 14.83 J/K

Δ = m*/388

m = 10 g; = 2250 J/g

Δ = 10*2250/388 = 57.99 J/K

Therefore,

Δ = Δ+Δ+Δ+Δ = 0.79+12.23+14.83+57.99 = 85.84 J/K

Thus, the change in entropy of the system is 85.84 J/K

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.

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