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18 Nov 2019
A student carries out a calorimetry experiment using HCl and NaOH. What effect will each of the following have on the calculated enthalpy of the reaction relative to the actual enthalpy of reaction? (larger, smaller or no change). Explain your reasoning. The thermometer always registered a temperature 0.30 degree C higher than the actual temperature The calorimeter constant used in the calculations by the student is larger than the actual value. Unfortunately, the HCl concentration was actually 1.90 M instead of the 2.00 M HCl used in the calculations. The actual concentration of the NaOH prepared for the experiment is 2.00 M instead of the 2.05 M used in the calculations.
A student carries out a calorimetry experiment using HCl and NaOH. What effect will each of the following have on the calculated enthalpy of the reaction relative to the actual enthalpy of reaction? (larger, smaller or no change). Explain your reasoning. The thermometer always registered a temperature 0.30 degree C higher than the actual temperature The calorimeter constant used in the calculations by the student is larger than the actual value. Unfortunately, the HCl concentration was actually 1.90 M instead of the 2.00 M HCl used in the calculations. The actual concentration of the NaOH prepared for the experiment is 2.00 M instead of the 2.05 M used in the calculations.
Tod ThielLv2
28 Jul 2019