Question

A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 114 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 ∘C. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures.

Answer 1

Answer:

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Explanation:

Answer 2

The enthalpy of this reaction is 0.882 kJ/mol.

Given the following data:

• Initial temperature = 21.0°C

• Final temperature = 24.70°C

• Mass of solution = 114 grams.

• Number of moles = 2.00 mol

We know that the specific heat capacity of water is 4.184 J/g°C.

To find the enthalpy of this reaction:

First of all, we would determine the quantity of heat energy that was used during this chemical reaction by using the formula;

$Q = mc\theta$

Where:

• Q represents the quantity of heat.

• m represents the mass of an object.

• c represents the specific heat capacity.

• ∅ represents the change in temperature.

$\theta = T_2 - T_1\\\\\theta = 24.70 - 21.00\\\\\theta = 3.70$

Substituting the values into the formula, we have:

$Q = 114$ × $4.184$ × $3.70$

Quantity of heat, Q = 1764.81 Joules

Now, we can find the enthalpy of this reaction by using the formula;

$Enthalpy = \frac{Energy}{Number\; of\; moles}$

Substituting the parameters into the formula, we have:

$Enthalpy = \frac{1764.81}{2.00}$

Enthalpy = 882.405 J/mol.

In Kilojoules per mole of compound to three significant figures:

Note: 1 Kilojoules = 1000 Joules

$Enthalpy = \frac{882.405}{1000}$

Enthalpy = 0.882 kJ/mol.

Therefore, the enthalpy of this reaction is 0.882 kJ/mol.

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