Consider these reactions, where M represents a generic metal.I.2 M(s) + 6 HCI(aq) 2 MCI, (aq) + 3 H, (g)Al = -819.0 kJ2.HCI(g) HCI(aq)Al2 = -74,8 kJH,(g) + Cl, (g) 2 HCI(g)All: = -1845.0 kJ3.4.MCI,(8) → MCI, (aq)AH = -128.0 kJUse the given information to determine the enthalpy of the reaction2 M(s) + 3 Cl, (g) 2 MCI;(s)kJAH =-5849.8Incorrect

In the above reactions we only need 2 reactions to calculate the enthalpy of the following reaction;…

Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI;(aq) + 3H,(g) All = -819.0 kJ %3! 2. HCI(g) HCI(aq) All2= -74.8 kJ %3D 3. H, (g) + Cl,(g) → 2 HCI(g) All3 = -1845.0 kJ 4. MCI, (s) → MCI, (aq) All = -128.0 kJ %3D Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) 2 MCI,(s)

Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI;(aq) + 3H,(g) All = -819.0 kJ %3! 2. HCI(g) HCI(aq) All2= -74.8 kJ %3D 3. H, (g) + Cl,(g) → 2 HCI(g) All3 = -1845.0 kJ 4. MCI, (s) → MCI, (aq) All = -128.0 kJ %3D Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) 2 MCI,(s)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.53PAE: 9.53 Using these reactions, find the standard enthalpy change for the formation of 1 mol of PhO(s)...

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A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?
In a calorimetric experiment, 6.48 g of lithium hydroxide, LiOH, was dissolved in water. The temperature of the calorimeter rose from 25.00C to 36.66C. What is H for the solution process? LiOH(s)Li(aq)+OH(aq) The heat capacity of the calorimeter and its contents is 547 J/C.
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?
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.
Consider the following reaction in the vessel described in Question 57. A(g)+B(g)C(s)For this reaction, E=286 J, the piston moves up and the system absorbs 388 J of heat from its surroundings. (a) Is work done by the system? (b) How much work?
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.
Chemical reactions are run in each of the beakers depicted below (labeled A, B, and C). The magnitude and direction of heat and work for each reaction are represented as arrows, with the length of an arrow depicting the relative magnitude of the heat or work. For the reaction in each beaker, answer the following and explain your reasoning: a Is the reaction endothermic or exothermic? b What is the sign (+ or ) of the work? c What is the sign (+ or ) of the enthalpy of each reaction? d Is there an increase or decrease in internal energy? e What is the temperature of the reaction mixture immediately after the reaction when compared to room temperature?
The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?
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.
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 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl 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 19.6C 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, the specific heat of all solutions is the same as that of water, and volumes are additive.
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