When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution(dissolving) can be determined using a coffee cup calorimeter.In the laboratory a general chemistry student finds that when 5.77 g of NaClO4(s) aredissolved in 112.90 g of water, the temperature of the solution drops from 23.94 to 22.44 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) wasdetermined in a separate experiment to be 1.62 J/°C.Based on the student's observation, calculate the enthalpy of dissolution of NaClO4(s) inkJ/mol.Assume the specific heat of the solution is equal to the specific heat of water.AH dissolutionkJ/molSubmit AnswerRetry Entire Group3 more group attempts remainingThermometerCardboard orStyrofoam lidNestedStyrofoam cupsReactionoccurs insolution.

Given NaClO4 is dissolved in water. The mass of NaClO4 dissolved in water =5.77 gThe mass of water…

Answered: When a solid dissolves in water, heat…

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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A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
When a 7.00 g sample of KCl is dissolved in water in a calorimeter that has a total heat capacity of 3.76 kJ⋅K−1, the temperature decreases by 0.430 K. Calculate the molar heat of the solution of KCl.
A 77.5g piece of brass is heated so that its temperature is 98.7◦C. Next,it is quickly placed in a calorimeter containing 102.76 g of water at 18.5◦C.Knowing that the final temperature is 23.5◦C, what is the specific heat of this alloy?Note: Brass is an alloy of copper and zinc. From 98.7 to 23.5◦C, this alloy does not changeno phase, it remains in solid form.
A 29.00 g sample of metal alloy is heated to 92.6 °C; then placed in 55.23 g of water in an insulated calorimeter at 21.3 °C. If the final temperature of the system is 43.9 °C, what is the specific heat of the metal alloy? Assume that the calorimeter absorbs a negligible amount of heat.
When 1.836 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?
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
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?
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 a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.79 g of KOH(s) are dissolved in 104.10 g of water, the temperature of the solution increases from 24.69 to 26.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. kJ/mol AH dissolution = BrookaCom Cengage Leaming Thermometer Cardboard or Styrofoam lid Nested Styrofoam cups Reaction occurs in solution.
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.34 kg sample of C,H¸0 from -1.5 °C to 18.1 °C. The experiment shows that 1.09 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,O? Round your answer to 2 significant digits. J• mol -1 1 ·K x10
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.

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