5. A carries out a experiment using HCI NaoH. What effect will each of the follo

Question

5. A carries out a experiment using HCI NaoH. What effect will each of the following have on the calculated enthalpy of the reaction relative actual enthalpy of to the reaction? (larger, or no change). Explain your reasoning. a. The thermometer a registered a temperature higher than the actua temperature b. The calorimeter constant used in the calculations by the student is larger than the actual value. (Hint: The best way to answer this guestion is to take your calorimeter C add at least 5 or 10 to the value and guickly redo the calculations. After calorimeter calculations, you should be able to complete the following statement: As the Constant increases, the calculated enthalpy of the reaction M HCI used c. Unfortunately, the HCI concentration was actually 1.90 M instead of the 2.00 in the calculations. (Hint: do a similar calculation. This is an estimate of how errors affect the result. lf your data is not matching the expected values, perhaps these questions will help you understand why.) d. The actual concentration of the NaoH prepared for the experiment is 2.00 M instead of the 2.05 M used in the calculations 6. Calculate the moles of water formed when 25.00 mL of 3.00 M HCl is reacted with 25.00 mL of 3.01 M NaOH. Write a balanced equation. me Chem 24B Lab: Enthalpy 153 Revised Sp 17 non of Hmo M 120, M

Explanation / Answer

Look it is very basic concept related to concentration nad enthalpy

In case , (a)-The actual enthalpy is smaller than the calculated enthalpy because

Thermometer show 0.30 c higher than the actual enthalpy

For(b)_The actual enthalpy is larger than the calculated enthalpy because

Colorimetric constants is the ratios between the heat applied to the colorimeter & corresponding change in temperature there fore temperature increasees enthalpy also increasing

(C) The actual enthalpy is larger than calculated enthalpy because,concentration increases due to 2M HCL there fore concentration increases ultimately enthalpy increases

(d) The actual enthalpy is smaller than calculated enthalpy because concentration of NaoH taken smaller than the required

Because ,heat release or enthalpy directly proportional to the reactant.

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