High School

When 4.6 g of ethanol ([tex]C_2H_6O[/tex], MW = 46.07 g/mol) was dissolved in 10.4 g of water, the temperature of the system increased from 20.0 °C to 35.9 °C.

What is the [tex]\Delta H_{\text{dissolution}}[/tex] for ethanol in water?

Is the enthalpy of dissolution for ethanol in water more or less favorable for a spontaneous process than for urea in water? Use your data from the lab to support your explanation.

Answer :

Explanation of enthalpy change for ethanol dissolution and a comparison with urea's dissolution.

The enthalpy change for the dissolution of ethanol in water can be calculated using the formula: q = m x C x ∆T

where q is the heat absorbed by the system, m is the mass of the solution, C is the specific heat capacity of water, and ∆T is the temperature change. The enthalpy of dissolution for ethanol in water is more favorable for a spontaneous process compared to urea in water because ethanol forms stronger hydrogen bonds with water, making it more soluble.

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