1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg²+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.

1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg²+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.

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...

See similar textbooks

Similar questions

When a 3.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity of 0.903 kJ⋅K−1, the temperature decreases by 0.440 K. Calculate the molar heat of solution of RbBr.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
To measure the enthalpy of an acid-base reaction, a student places the thermometer in the hydrochloric acid solution, and then, without rinsing with DI water, places it in the sodium hydroxide solution prior to adding the hydrochloric acid solution to the calorimeter. How would this affect the calculated enthalpy of the reaction, be too high, too low, or unaffected? Why?
A quantity of 85.0 mL of 0.600 M HCl is mixed with 85.0 mL of 0.600 M KOH in a constant-pressure calorimeter. The initial temperature of both solutions is the same at 17.35°C, and the final temperature of the mixed solution is 19.02°C. What is the heat capacity of the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is −56.2 kJ/mol.
22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.
A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?
When a 6.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 3.74 kJ · K¯¹, the temperature decreases by 0.400 K. Calculate the molar heat of solution of KSCN. ΔΗsoln = kJ/mol
A quantity of 100.0 mL of 1.0 M HCl and 100.0 mL of 1.0 M NaOH are mixed in a calorimeter. The initial temperatures of the HCl and NaOH solutions are the same at 20.0°C and the final temperature of the mixture is 27.0oC. Calculate the heat of neutralization for the reaction in kJ/mole of NaOH. Assume the density and specific heat of the solutions are the same as pure water and that no heat was lost to the surroundings.