A student performs a calorimetry experiment. The student combines 100. g of 0.40 M HC1(aq) with 100. g of 0.40 M NAOH(ag). Data are given in the table. Temperature of HCI(ag) before mixing 25.0°C Temperature of NaOH(ag) before mixing 25.0°C Temperature of solution after mixing 27.8°C Drag the claim and evidence statements that are correct for the experiment. Claim Evidence Evidence: The temperature increases when the solutions are combined Evidence: The temperature decreases when the : Claim: The reaction is endothermic. : Claim: The reaction is exothermic. solutions are combined.

A student performs a calorimetry experiment. The student combines 100. g of 0.40 M HC1(aq) with 100. g of 0.40 M NAOH(ag). Data are given in the table. Temperature of HCI(ag) before mixing 25.0°C Temperature of NaOH(ag) before mixing 25.0°C Temperature of solution after mixing 27.8°C Drag the claim and evidence statements that are correct for the experiment. Claim Evidence Evidence: The temperature increases when the solutions are combined Evidence: The temperature decreases when the : Claim: The reaction is endothermic. : Claim: The reaction is exothermic. solutions are combined.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Н.С. C H2 || OH + HC | | | HC. H H -OH CH H+/heat
When 50 mL of 0.400 M aqueous hydrochloric acid (HCI; Molar mass: 36.5 g'mol) is mixed with 50 mL of 0.400 M aqueous sodium hydroxide (NaOH; Molar mass: 40 g/mol) in a calorimeter the temperature increases by 3.4°C. If the heat capacity of calorimeter (excluding water) is 320 Ji°C, calculate AH of neutralization reaction in kJ/mol. (Specific heat capacity of water is 4.184 J°C- gl. Density of water is 1 g'mL Assume that the heat capacity and the density of the solution is same with water) 2511 kJ/mol O A. 1.09 kJ/mol O B. 1088 kJ/mol OC. 125.5 kJ/mol OD. 2.5 kJ/mol O E.
When 3.02 g of NHẠCI is dissolved in enough water to make 20.05 mL of solution, the temperature dropped from 19.8°C to 9.1°C. Calculate the enthalpy change (in kJ) when 1 mole of NH4CI is dissolved in water. The density and specific heat of water are 1.00 g/mL and 4.18 J/g°C respectively. Type your numeric answer and submit
Which reaction would it be possible to calculate (Triangle H)?
#3
1) A 0.416 g sample of KCl is added to 56.5 g of water in a calorimeter. If the temperature decreases by 1.24°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? _____ J 2) Is the reaction exothermic or endothermic?
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