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 183 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

Enthalpy of reaction - 1.42 kJ/mol

Step-by-step explanation:

given data:

specific heat capacity of water = 4.18 J/g degree celcius

mass of solution = 184 g

temperature difference
`\Delta T` = 24.70 - 21.0 = 3.7 Degree celcius

we know that quantity of heat is given as

`q = mass\ of\ solution * specific\ heat *\Delta T`

q = 184*4.18*3.7

`q =2845.74 J * (1kJ)/(1000j)`

q = 2.84 kJ

Enthalpy of reaction is given as

`= (2845.74)/(2) = 1422.872 J`

= 1.42 kJ

FOR exothermic reaction = - 1.42 kJ/mol