The overall reaction in a commercial heat pack can be represented as shown below.4 Fe(s)30,(g)2 Fe,0,(s) AH- -1652 kJ(a) How much heat is released when 4.60 mol iron are reacted with excess 0,?k)(b) How much heat is released when 1.72 mol Fe,0, is produced?k)(C) How much heat is released when 1.90 g iron are reacted with excess 0,?(d) How much heat is released when 10.0 g Fe and 2.19 g 0, are reacted?k)

Answered: Image /qna-images/answer/27af195a-712f-45cb-b5aa-645d6f881a41.jpg

Answered: The overall reaction in a commercial…

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Energy

Section: Chapter Questions

Problem 61A

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Given 2Al2O3(s)4Al(s)+3O2(g)H=3351.4kJ (a) What is the heat of formation of aluminum oxide? (b) What is H for the formation of 12.50 g of aluminum oxide?
Given 2Cr2O3(s)4Cr(s)+3O2(g)H=+2269.4kJ (a) What is the heat of formation of chromium(III) oxide? (b) What is H for the formation of 13.65 g of chromium (III) oxide?
9.50 When a 13.0-g sample of NaOH(s) dissolves in 400.0 mL of water in a coffee cup calorimeter, the temperature of the water changes from 22.6°C to 30.7C Assuming that the specific heat capacity of the solution is the same as for water, calculate (a) the heat transfer from system to surroundings and (b) H for the reaction NaOH(s)Na+(aq)+OH(aq)
When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?
Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00 mol of powdered aluminum and 3.00 mol of ammonium nitrate crystals reacts exothermically yielding nitrogen gas, water vapor, and aluminum oxide. How many grams of the mixture are required to provide 245 kJ of heat? See Appendix C for data.
9.32 The material typically used to heat metal radiators is water. If a boiler generates water at 79.5°C, what mass of water was needed to provide the heat required in the previous problem? Water has a specific heat of 4.184Jg1 C1 .
A small car is traveling at twice the speed of a larger car, which has twice the mass of the smaller car. Which car has the greater kinetic energy? (Or do they both have the same kinetic energy?)
You wish to heat water to make coffee. How much heat (in joules) must be used to raise the temperature of 0.180 kg of tap water (enough for one cup of coffee) from 30C to 96C (near the ideal brewing temperature)? Assume the specific heat is that of pure water, 4.18 J/(gC).
Hydrogen cyanide is a highly poisonous, volatile liquid. It can be prepared by the reaction CH4(g)+NH3(g)HCN(g)+3H2(g) What is the heat of reaction at constant pressure? Use the following thermochemical equations: N2(g)+3H2(g)2NH3(g);H=91.8kJC(graphite)+2H2(g)CH4(g);H=74.9kJ12H2(g)+C(graphite)+12N2(g)HCN(g);H=135.1kJ
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.

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