Question

Hikers climbing mount everest discovered it took much longer to cook a boiled egg than it does at sea level, because the boiling water is not as hot. The ∆h(vap) of water is 40. 7 kj/mol. Atmospheric pressure at sea level is 760 torr. R = 8. 314 ×10⁻³ kj/mol･k. Calculate the temperature of boiling water (in °c) at an atmospheric pressure of 375 torr.

Answer 1

The temperature of Boiling Water in °c is;

T₁ = 121.22 °c

Use of Clausius Clapeyron Equation

We are given;

Initial atmospheric Pressure; P₁ = 375 torr

∆h(vap) of water= 40. 7 kj/mol = 40700 J/mol

Final atmospheric pressure; P₂ = 760 torr

R = 8.314 10⁻³ kj/mol.k = 8.314 j/mol.k

Using Clausius Clapeyron Equation, we have;

In(P₂/P₁) = (-∆h/R) * (1/T₂ - 1/T₁)

where T₂ = 373.15 K (boiling point)

Thus;

In(760/375) = -(40700/8.314) * (1/373.15 - 1/T₁)

0.70639 = -4895.357 * (0.00268 - 1/T₁)

(0.00268 - 1/T₁) = -0.70639/4895.357

0.0268 - 1/T₁ = -0.0001443

1/T₁ = 0.00268 - 0.0001443

T₁ = 1/0.0025357

T₁ = 394.37 K

in °c gives; T₁ = 121.22 °c

Read more about the use of Clausius-Clapeyron Equation at; https://brainly.com/question/21504082