Question

Lab: Calorimetry of a salt solution Procedure: measure NaOH on the electronic balcance and put it in the calorimetry cup and stir with therometer when salt dissolved ,then read the therometer. next, measure KCl on the electonic balance and put it in the new calorimetry cup and stir with the same therometer you used it before without cleaning it, then read the temperature. There are 3 assumptions here: 1. No heat is transferred between the calrorimeter and the outside environment.2. All heat changes within the calrorimeter are the result of the reaction taking place, and this reaction yeilds 100% product.3. Dilute solution are given the density and specific heat capacity of pure water. Sample | Mass of Water(g) | Initial temp of water(C) | Final temp of water(C) | Change in temp of water(C) | Energy change use mct(kJ) | Mass of salt used(g) | Enthalpy of solution kJ/g NaOH | 75 | 21.4 | 40.4 | 19.0 | 5.96 | 6.28 | -0.95 KCl | 75 | 21.3 | 16.3 | -5.0 | -1.6 | 5.90 | 0.26 Q)3.If some heat were transferred to the air or Styrofoam cup calorimeter., would your calculated enthalpy of solution of the salt be too high or too low? Explain your answer. Q)4.. If some salt were accidentally spilled as it was transferred from the balance to the cup, would your calculated enthalpy of solution of the salt be too high or too low? Explain your answer.

          Lab: Calorimetry of a salt solution
Procedure: measure NaOH on the electronic balcance and put it in the calorimetry cup and stir with therometer when salt dissolved ,then read the therometer. next, measure KCl on the electonic balance and put it in the new calorimetry cup and stir with the same therometer you used it before without cleaning it, then read the temperature.
There are 3 assumptions here: 1. No heat is transferred between the calrorimeter and the outside environment.2. All heat changes within the calrorimeter are the result of the reaction taking place, and this reaction yeilds 100% product.3. Dilute solution are given the density and specific heat capacity of pure water.
Sample | Mass of Water(g) | Initial temp of water(C) | Final temp of water(C) | Change in temp of water(C) | Energy change use mct(kJ) | Mass of salt used(g) | Enthalpy of solution kJ/g
NaOH | 75 | 21.4 | 40.4 | 19.0 | 5.96 | 6.28 | -0.95
KCl | 75 | 21.3 | 16.3 | -5.0 | -1.6 | 5.90 | 0.26
Q)3.If some heat were transferred to the air or Styrofoam cup calorimeter., would your calculated enthalpy of solution of the salt be too high or too low? Explain your answer.
Q)4.. If some salt were accidentally spilled as it was transferred from the balance to the cup, would your calculated enthalpy of solution of the salt be too high or too low? Explain your answer.

Lab: Calorimetry of a salt solution
Procedure: measure NaOH on the electronic balcance and put it in the calorimetry cup and stir with therometer when salt dissolved ,then read the therometer. next, measure KCl on the electonic balance and put it in the new calorimetry cup and stir with the same therometer you used it before without cleaning it, then read the temperature.
There are 3 assumptions here: 1. No heat is transferred between the calrorimeter and the outside environment.2. All heat changes within the calrorimeter are the result of the reaction taking place, and this reaction yeilds 100% product.3. Dilute solution are given the density and specific heat capacity of pure water.
Sample | Mass of Water(g) | Initial temp of water(C) | Final temp of water(C) | Change in temp of water(C) | Energy change use mct(kJ) | Mass of salt used(g) | Enthalpy of solution kJ/g
NaOH | 75 | 21.4 | 40.4 | 19.0 | 5.96 | 6.28 | -0.95
KCl | 75 | 21.3 | 16.3 | -5.0 | -1.6 | 5.90 | 0.26
Q)3.If some heat were transferred to the air or Styrofoam cup calorimeter., would your calculated enthalpy of solution of the salt be too high or too low? Explain your answer.
Q)4.. If some salt were accidentally spilled as it was transferred from the balance to the cup, would your calculated enthalpy of solution of the salt be too high or too low? Explain your answer.

Added by Mark R.

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