Enthalpy is the energy absorbed or released when a chemical change occurs. Assume you have the following thermochemical reaction:2H2Sig) + 3021g) -> 2SOzig) + 2H2Oig AH = -1036 KJHow much energy is absorbed or released when 19.6 g of hydrogen sulfide (H,S) is burned? Is this an exothermic or endothermic reaction?Show all work for full credit.

Answered: Image /qna-images/answer/b729424a-fbca-4103-b812-96632acfef22.jpg

Enthalpy is the energy absorbed or released when a chemical change occurs. Assume you have the following thermochemical reaction: 2H3Sg + 30zg - 2502g 2H2Ogi AH = -1036 KJ How much energy is absorbed or released when 19.6 g of hydrogen sulfide (H,S) is burned? Is this an exothermic or endothermic reaction? Show all work for full credit.

Enthalpy is the energy absorbed or released when a chemical change occurs. Assume you have the following thermochemical reaction: 2H3Sg + 30zg - 2502g 2H2Ogi AH = -1036 KJ How much energy is absorbed or released when 19.6 g of hydrogen sulfide (H,S) is burned? Is this an exothermic or endothermic reaction? Show all work for full credit.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 15Q: The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as...

See similar textbooks

Similar questions

Consider the following reaction in a vessel with a movable piston. R(g)+T(g)X(g)As the reaction takes place, the piston loses 1072 J of heat. The piston moves down and the surroundings do 549 J of work on the system. What is E?
Combustion of table sugar produces CO2(g) and H2O( l). When 1.46 g table sugar is combusted in a constant-volume (bomb) calorimeter, 24.00 kJ of heat is liberated. a. Assuming that table sugar is pure sucrose, C12H22O11 (s), write the balanced equation for the combustion reaction. b. Calculate E in kJ/mol C12H22O11 for the combustion reaction of sucrose.
9.31 A metal radiator is made from 26.0 kg of iron. The specific heat of iron is 0.449Jg1C1 . How much heat must be supplied to the radiator to raise its temperature from 25.0 to 5 5.0°C?
A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 21.8C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, and volumes are additive.
Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU. (a) How many joules are in one therm? (1J=9.48104BTU) (b) When propane gas, C3H8, is burned in oxygen, CO2 and steam are produced. How many therms of energy are given off by 1.00 mol of propane gas?
How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?
9.89 A sample of gas is 80.0% CH4 and 20.0% C2H6 by mass. What is the heat from the combustion of 1.00 g of this mixture? Assume the products are CO2 (g) and H2O (l).
When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?
The overall reaction in a commercial heat pack can be represented as 4Fe(s)+3O2(g)2Fe2O3(s)H=1652KJ a. How much heat is released when 4.00 moles of iron are reacted with excess O2? b. How much heat is released when 1.00 mole of Fe2O3 is produced? c. How much heat is released when 1.00 g iron is reacted with excess O2? d. How much heat is released when 10.0 g Fe and 2.00 g O2 are reacted?
How much heat is produced when loo mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M NaOH (density, 1.00 g/mL) are mixed? HCl(aq)+NaO(aq)NaCl(aq)+H2O(l)H298=58kJ If both solutions are at the same temperature and the heat capacity of the products is 4.19 J/g C, how much will the temperature increase? What assumption did you make in your calculation?
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 one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid water are formed. The reaction absorbs 90.1 kJ of heat. (a) Write a balanced thermochemical equation for the reaction. (b) Using Table 8.3, calculate Hf for calcium cyanamide.