Changes to temperature: Endothermic reaction: Exothermic reaction: 8. reactants + heat products reactants products + heat The reaction: 2SO2(g) + O2(g) 160. AH = positive ΔΗ = negative 2SO3(g) AH= -197kJmoll¹ is discussed on page a) Is the forward reaction exothermic or endothermic? b) Is the reverse reaction endothermic or exothermic? c) What is the endothermic or exothermic reaction favoured when temperature of an equilibrium system is increased? Explain using Le Chatelier's Principle. d) What would happen to the Keg for this reaction at a higher temperature? Why? e) What would happen when the temperature is decreased?

Changes to temperature: Endothermic reaction: Exothermic reaction: 8. reactants + heat products reactants products + heat The reaction: 2SO2(g) + O2(g) 160. AH = positive ΔΗ = negative 2SO3(g) AH= -197kJmoll¹ is discussed on page a) Is the forward reaction exothermic or endothermic? b) Is the reverse reaction endothermic or exothermic? c) What is the endothermic or exothermic reaction favoured when temperature of an equilibrium system is increased? Explain using Le Chatelier's Principle. d) What would happen to the Keg for this reaction at a higher temperature? Why? e) What would happen when the temperature is decreased?

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

How much heat is given off when an 869 g iron (specific heat = 0.45 J/g. oC) bar cools from 94oC to 5.0oC? Is this endothermic or exothermic?
Which equation is correct for the formation reaction of nitric acid, HNO3? A) N₂(g) + H₂(g) + 30₂(g) → 2HNO3(aq) ΔΗ = 174 kJ B) N₂(g) + H₂(g) + 30₂(g) → 2HNO3(0) AH = -174 kJ C) NH3(g) + N₂(g) + 30₂(g) → 3HNO3(aq) D) 1/2N₂(g) + 1/2H₂(g) + 3/20₂(g) → HNO3(/) 1 E) N₂(g) + H₂(g) + O₂(g) → HNO3(/) ΔΗ = 174 kJ ΔΗ = -174 kJ ΔΗ = -174 kJ
The following thermochemical equation is for the reaction of carbon monoxide(g) with oxygen(g) to form carbon dioxide(g). 2CO(g) + O2(g)- →2CO2(g) AH=-566 kJ How many grams of CO(g) would have to react to produce 104 kJ of energy? grams
13. Determine the amount of heat (in kJ) given off when 320 g of NO, are produced according to the equation: 2 NO(g) + 0,(g) 2 NO,(g) ΔΗ - -114.6 kJ/mol (Molar mass of NO, = 46 g/mol) * -1.49 x 10+2 -6.48 x 10+2 -3.99 x 10+2 O -2.74 x 10*2 -5.23 x 10+2 If th
Which is not a factor of an endothermic reaction? OAHIS negative. O AH is on the reactant (left) side of the reaction. O Heat is absorbed. O AH is positive.
Which chemical reaction below yields the heat of formation of liquid ammonia (NH3)? 3H(g) + N(g) →→→ NH3(e) H₂ (g) + N2₂ (g)→→ NH3(e) 3/2 H₂ (g) + 1/2 N₂ (g)→ NH3 (e) 3H₂(g) + N₂ (g)→ 2NH3(e) 3/2 H₂(g) + N(g)→ NH3(e)
A certain reaction has Ho = -43.40 kJ and So = 23.20 J/K.(a) Is this reaction exothermic, endothermic or isothermic (neither)?This reaction is________ .(b) Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system?This reaction leads to_______ in the disorder of the system.
In the following reaction, how many grams of CH3OH are required to produce 1.578 x 10° kJ of heat? 2 CH3OH (1) +3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH = -1280. kJ/mol Please do not include units in your answer.
1) A 0.416 g sample of KCl is added to 56.5 g of water in a calorimeter. If the temperature decreases by 1.24°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? _____ J 2) Is the reaction exothermic or endothermic?
Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HCl(9) AH = -184.6 kJ Reaction 2: 20F2(g) → O2(g) +2F2(g) AH=-49.4 kJ Reaction 3: Na (g) +202 (9) 2NO2(g) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,409.0 kJ of energy is released from the system. Round to the nearest whole number .
When 25.0 g hydrogen gas react according to the following reaction, how many kJ of heat are released or consumed? CO (g) + 3 H2 (g) --> CH4 (g) + H2O (g) Delta Hrxn = – 206 kJ a. – 1.28 x 103 J b. – 25.5 J c. – 639 J d. – 2.55 x 103 J e. – 1.29 x 103 J f. none of these
A 7.37 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. What quantity in moles of the unknown salt were used in the reaction?