Problem: Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.40°C. A 300. mL sealed flask contains 0.620g of butane at -21.0°C. How much liquid butane is present?A. 0.375g B. 0.475g C. 0.245g D. 0.620g E. no liquid left

FREE Expert Solution

We are asked how much liquid butane is present in a 300. mL sealed flask contains 0.620g of butane at -21.0°C


We go through the following steps to solve the problem: 

Step 1. Calculate the vapor pressure at -21.0 °C

Step 2. Calculate the mass in the gas phase

Step 3. Calculate the mass in the liquid phase



Step 1. Calculate the vapor pressure at -21.0 °C

For this part, we can use the Clausius-Clapeyron Equation:


lnP2P1 = -HvapR[1T2-1T1]


where:

P1 = vapor pressure at T1

P2 = vapor pressure at T2

ΔHvap = heat of vaporization (in J/mol)

R = gas constant (8.314 J/mol•K)

T1 and T2 = temperature (in K).


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Problem Details

Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.40°C. A 300. mL sealed flask contains 0.620g of butane at -21.0°C. How much liquid butane is present?

A. 0.375g 

B. 0.475g 

C. 0.245g 

D. 0.620g 

E. no liquid left

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