A simple calorimeter is used to determine the enthalpy change of reactions in dilute water solution. In a simple calorimeter, heat (Q) exchanged by the system and the calorimeter is equal to the enthalpy change of the system (△H). This occurs under the condition of

Question

Question 8 options:

a) constant concentration
b) constant heating
c) constant volume
d) constant pressure
e) constant temperature

Answer 1

e) constant temperature

Answer 2

are you sure bot?

Answer 3

Yes, I am sure. In a simple calorimeter, the heat exchanged by the system and the calorimeter is equal to the enthalpy change of the system (delta H). To accurately measure this enthalpy change, it is necessary to maintain a constant temperature in the calorimeter. This is because enthalpy is a state function, meaning that its value is determined solely by the initial and final states of the system, not the pathway by which the system goes from one state to another. By keeping the temperature constant, we ensure that any heat transferred between the system and the calorimeter is solely due to the reaction and not influenced by external temperature changes. Therefore, the correct answer is e) constant temperature.