A reaction of 1.00 gram of NaOH with 100 mL of 1.0 M HCl in a styrofoam calorimeter causes a 10.5°C increase in the temperature of the reaction solution. Assuming the specific heat of the solution is 4.184 J/g°C, density is 1.00 g/mL, and the heat capacity of the styrofoam cup calorimeter is 10.0 JPC, calculate the heat of this reaction per mole of NaOH. ΔΗΞ kJ/mol

A reaction of 1.00 gram of NaOH with 100 mL of 1.0 M HCl in a styrofoam calorimeter causes a 10.5°C increase in the temperature of the reaction solution. Assuming the specific heat of the solution is 4.184 J/g°C, density is 1.00 g/mL, and the heat capacity of the styrofoam cup calorimeter is 10.0 JPC, calculate the heat of this reaction per mole of NaOH. ΔΗΞ kJ/mol

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

33.79 g of a solid is heated to 100.°C and added to 50.0 g of water in a coffee cup calorimeter and the contents are allowed to sit until they finally have the same temperature. The water temperature changes from 29.76 °C to 38.3 °C and the specific heat capacity of water is 4.184J/g °C. What is the specific heat capacity (in J/g°C) of the solid? O 1.73 O 1.17 O 0.857 O 0.579
A 1.595 g samples of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.67 degrees Celsius to 29.44 degrees Celsius. The heat capacity (calorimeter constant) of the calorimeter is 30.29 kJ/degrees Celsius, what is the heat of combustion per gram of the material?
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.
A piece of molybdenum metal whose mass is 6.87 g is heated to 100.0 °C and then dropped into an ice calorimeter. As the molybdenum cools to 0.0°C, 0.513 g of ice melts (it takes 6.01 kJ of heat to melt exactly 1 mol of ice). What is the molar heat capacity (in J/mol·K) of molybdenum? i J/mol*K
a chemist wastes a delicious brownie by burning it in a bomb calorimeter. before burning, the brownie weighed 16.13 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.40 degrees celsius. The known heat capacity of the calorimeter that was used was 26.53 kJ/Celsius. What is the energy content, in kJ/g, of this brownie?
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?
A 32.1 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 25.8°C. Calculate the mass of water in the calorimeter.
75.0 mL of 1.80 M CuSO 4 solution is mixed with 150 mL of 1.80 M NAOH solution in a coffee cup calorimeter of negligible heat capacity. If the initial temperature of the two solutions are both 21.0 degrees C, and the final temperature of the mixed solution is 27.1, how much heat was released by the reaction? Assume density of solution d is 1.00 g/mL and that the solution has the same specific heat as water. The thermochemical equation is: CuSO4 (ag) + 2NAOH (ag) --> Cu(OH)2 (s) + Na SO4 (ag) AH xn = - 42.3 kJ/mol rxn Hint: no limiting reagent, substances are presented in correct molar ratios. O 6180 J O 9270 J O 3120 J O 5740 J O 9300 J O 1250 J O 6230 J O 3380 J
In a coffee-cup calorimeter, 120.0 mL of 1.4 M NaOH and 120.0 mL of 1.4 M HCL are mixed. Both solutions were originally at 20.6°C. After the reaction, the final temperature is 30.0°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCL by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH = kJ/mol
When 1.366 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.
In a coffee-cup calorimeter, 110.0 mL of 1.3 M and 110.0 mL of 1.3 M are mixed. Both solutions were originally at 22.2°C. After the reaction, the final temperature is 30.9°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH in (kJ/mol). Assume that no heat is lost to the surroundings or to the calorimeter.