QUESTION 5The size of the equilibrium constant is linked to the spontaneity of the reaction. Pair the equilibrium constants to thecorrect conclusions.✓ 1.8 × 10-108.7 × 10-15▾ 4.5 ×10831013A. Spontaneous, many products formedB. Not spontaneous, few products formed QUESTION 4This lab has you measure the hydroxide ion concentration and then calculate the calcium ion concentration presentin the saturated solution of Ca(OH)2. If hydroxide ion concentration is 0.488 M, what is the calcium ion concentration,also in molarity?

Question 4.Step 1: Calcium hydroxide dissociates in water according to the chemical equation shown…

Answered: QUESTION 5 The size of the equilibrium…

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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The free energy of formation for C10H14(g) is 144.920 kJ/mol. What is the equilibrium constant at 25.0oC for its formation? 2.954e58 3.386e-59 4.085e-26 2.448e25
8. Discuss Le Chatelier's Principle as it applies to chemical equilibria. Consider the reaction that follows and detail how this equilibrium will be affected by changes in pressure and temperature. 4CO(g) + H2O(g) – CH.(g) + 3CO:(g) AH° =-571.4 kJ
Consider the reaction:2 NO( g) + O2( g)Δ2 NO2( g)The following data show the equilibrium constant for this reaction measured at several different temperatures. Use the data to find ΔH°rxn and ΔS°rxn for the reaction.Temperature Kp170 K 3.8 * 10- 3180 K 0.34190 K 18.4200 K 681
In a reversible reaction, a forward spontaneous reaction corresponds to a negative AG. O TRUE O FALSE
Using reaction free energy to predict equilibrium composition elld Consider the following equilibrium: N2 (g) + 3H2 (g) = 2NH3 (g) AGº = -34. kJ Now suppose a reaction vessel is filled with 6.04 atm of nitrogen (N2) and 9.12 atm of ammonia (NH3) at 892. °C. Answer the following questions about this system: ? rise x10 fall Under these conditions, will the pressure of N2 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of N2 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of N₂ will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm ☑ ⑤ 000 18 Ar Bi
7. Calculate A,G° for the reaction below at 25.0 °C CHA(g) + H20(g) →3 H2(g) + CO(g) given AG° [CH(g)] =-50.8 kJ/mol, AG° [H2O(g)] =-228.6 kJ/mol, AG° [H2(g)] = 0.0 kJ/mol, and AG° [CO(g)] = -137.2 kJ/mol. a. -416.3 kJ/mol-rxh b. -142.2 kJ/mol-rxn +142.2 kJ/mol-rxn %3D C. d. +315.0 kJ/mol-rxn +416.3 kJ/mol-rxn e.
Which reaction would produce more products when the pressure is increased?
A reaction has an equilibrium constant of 79 at 298 K. At 498 K, the equilibrium constant is 0.85. You may assume that Δ Hrxn and ΔSrxn stay the same at different temperatures. a. What is the Δ G°rxn at 298 K?b. What is the Δ Hrxn ?c. What is the ΔSrxn ?
Consider the gas phase reaction NO + %02=NO2 for which AH° = -57.05 kJ and K= 1.54 × 10° at 25°C. 18. What would be the effect on the amount of NO present of compressing the equilibrium system to a smaller volume, while keeping the temperature constant? a. The amount ofNO will increase. b. The amount of NO will decrease. c. The amount of NO will remain the same. d. Cannot be determined. e. Answer depends on the value of K.
13. For the decomposition of calcium carbonate CACO3 (s) = CaO (s) + CO2 (g) How will the amount (not concentration) of CaCO3 (s) change with the following stresses to ΔΗ175 kJ the system at equilibrium? a. CO2 (g) is removed. b. CaO (s) is added. c. The temperature is raised. d. The volume of the container is decreased.
The equilibrium constant of a reaction is found to fit the expression below, between 300 K and 600 K: lnK=−2.04(1176K/T)+(2.1∑a,b×10^7K^3)/T3. Find ΔrSΘ and ΔriHΘ a. ΔrSΘ = 6.67 J K-1 mol-1 and ΔrHΘ = 7.19 kJ mol-1 b. ΔrSΘ = 21 J K-1 mol-1 and ΔrHΘ = 19.5 kJ mol-1 c. ΔrSΘ = 6.67 J K-1 mol-1 and ΔrHΘ = 19.5 kJ mol-1 d.
For the reversible reaction: 22 2CO(g) + 2NO(g) = N2(g) + 2CO2(g) the following concentrations of reactants and products are found at equilibrium. What is the value of the equilibrium constant, K. under these conditions? [N2] = 1.57M, [CO2] = 0.668M, [CO] = 0.115M, [NO] = 0.227M

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