Hi I need help with these following questions. I have all of the data needed.
Calculate the enthalpy change of the reaction for each trial (in kJ)
3. Calculate the heat released by the reaction for each trial (in J):
2. Calculate the heat absorbed by the calorimeter for each trial (in J):
Calculate the heat absorbed by the solution for each trial (in J):
-Mass of the empty calorimeter (g): 18.600g
-Initial temperature in the calorimeter (oC): 21.5 C
-Maximum temperature in the calorimeter from the reaction (oC): 30.7 C
-ΔT (oC) 9.2 C
-Mass of the calorimeter and its contents after the reaction (g):69.0g
-Mass of the solution, e - a (g)50.4g
-Moles of Mg reacted: 0.0062 moles
Thank you for your help!
Could you please show work, too? I'm really trying to understand it.
To calculate the enthalpy change of the reaction (ΔH), you can use the equation:
ΔH = q / moles of reactant
Here, "q" represents the heat released or absorbed by the reaction. Since it is not mentioned whether the reaction is exothermic or endothermic, we will need to consider the sign of q.
To calculate the heat released by the reaction (q), you can use the equation:
q = m * ΔT * Cp
Here, "m" represents the mass of the solution, "ΔT" represents the change in temperature, and "Cp" represents the specific heat capacity of the solution.
To calculate the heat absorbed by the calorimeter (q_calorimeter), you can use the equation:
q_calorimeter = m_calorimeter * ΔT * Cp_calorimeter
Here, "m_calorimeter" represents the mass of the calorimeter, and "Cp_calorimeter" represents the specific heat capacity of the calorimeter. Note that the calorimeter absorbs heat from the reaction, so q_calorimeter will have a negative sign.
To calculate the heat absorbed by the solution (q_solution), you can use the equation:
q_solution = q - q_calorimeter
Now let's calculate the values:
1. Calculate the heat released by the reaction (q):
q = m * ΔT * Cp
= 50.4g * 9.2°C * (specific heat capacity of the solution)
2. Calculate the heat absorbed by the calorimeter (q_calorimeter):
q_calorimeter = m_calorimeter * ΔT * Cp_calorimeter
= (69.0g - 18.600g) * 9.2°C * (specific heat capacity of the calorimeter)
3. Calculate the heat absorbed by the solution (q_solution):
q_solution = q - q_calorimeter
4. Calculate the enthalpy change of the reaction (ΔH):
ΔH = q_solution / moles of Mg reacted
= q_solution / 0.0062 moles
Ensure to substitute the appropriate values for the specific heat capacity of the solution and the calorimeter in the calculations. After calculating these values, you will have the enthalpy change of the reaction for each trial.