A common laboratory reaction is the neutralization of an acid with a base. When 17.5 mL of 0.500 M HCl at 25.0°C is added to 46.6 mL of 0.500M NAOH at 25.0°C in a coffee cup calorimeter, the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of acid (in J/mol)? Assume the mixture has a specific heat capacity of 4.18 J/(g-K) and that the densities of the reactant solutions are both 1.07 g/mL. Enter a number in J/mol to 0 decimal places.

A common laboratory reaction is the neutralization of an acid with a base. When 17.5 mL of 0.500 M HCl at 25.0°C is added to 46.6 mL of 0.500M NAOH at 25.0°C in a coffee cup calorimeter, the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of acid (in J/mol)? Assume the mixture has a specific heat capacity of 4.18 J/(g-K) and that the densities of the reactant solutions are both 1.07 g/mL. Enter a number in J/mol to 0 decimal places.

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 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
In a coffee-cup calorimeter, 59.0 mL of 0.100 M AgNO3 and 59.0 mL of 0.100 M HCI are mixed to yield the following reaction. Ag (aq) + Cl(aq) → AgCl(s) The two solutions were initially at 19.10°C, and the final temperature is 19.90°C. Calculate the heat that accompanies this reaction in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 118.0 g and has a specific heat capacity of 4.18 1/°C 9- 407 kJ/mol
During an experiment, a student adds 0.339 g of calcium metal to 100.0 mL of 2.05 M HCI. The student observes a temperature increase of 11.0 °C for the solution. Assuming the solution's final volume is 100.0 mL, the density is 1.00 g/mL, and the specific heat is 4.184 J/(g-°C), calculate the heat of the reaction, AH. Ca(s) + 2H* (aq) → Ca²* (aq) + H, (g) AHran 543.1 kJ/mol Incorrect
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
You have 8.99 g sample of an unknown salt (MM = 116.82 g/mol). It is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What is the Mass inside calorimeter (g)? Change in Temp inside calorimeter (C)? How much Heat gained (J)? Total Heat? How many mols of the unknown salt? What is the change in empalthy?
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.
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic? how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius
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.
when 50.0 mL of 0.200 M NaOH is mixed with 50 mL of 0.200 M HCl in a coffee cup calorimeter, the temperature increases from 23.5 degrees C to 26.5 degrees C. Assuming that the density of the resulting solution is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g degrees C, what is qrxn?
A 42.0 g sample of water at 100.00°C was placed in an insulated cup. Then 15.4 g of zinc metal at 23.60°C was added to the water. The temperature of the water dropped to 97.52°C. What is the specific heat of zinc? Assume the specific heat is that of pure water, 4.18 J/(g⋅°C).
Isooctane is a primary component of gasoline and gives gasoline its octane rating. Burning 1isooctane releases 47.965 kJ/gmol of heat. When 10.0 mL of isooctane (d=0.688 g/mL) is burned in a bomb calorimeter, the temperature in the bomb increases from 23.2°C to 66.5°C. What is the heat capacity of the bomb calorimeter?
A block of iron weighing 3.50 kg at a temperature of 107.0 °C was inserted into a container containing 1.00 liter of water at a temperature of 30.0 °C isolated from the environment. What is the final temperature (in °C) of the water and the iron at the end of the process? (The specific heat of solid iron is 0.450 J /g and the specific heat of water is 4.184 J/ g°C ) Density of water = 1.0 g/mL.