Chemistry1-9 please? 1.24.3.8.6.9.Write the equilibrium constant expression for each of the following reactions:2 NO: (A)a) Na (g)b) 2 C(s)c) la (aq)20; (g)3 Hz (g)la (4)Calle (K)2 NO(g)K=50x10¹0₂ (8)2 NO₂ (g)Calculate the equilibrium concentration of oxygen gas if the NO and NO₂concentrations are equal at equilibrium.5. For the following equilibrium reaction:N₂0 (g) 58.9 kJ 2NO(g)a one litre flask at 55°C is found to contain 3.6 moles of N:04 (g) in equilbrium with1.75 moles of NO: (g). Calculate the value of K for this reaction.K=18x10a) CHICOOH (aq)b) H(aq)H- (aq)• CHICOO- (aq)H₂S (aq)K=10x10+HSWhich of the above reactions would have the greatest amount of products present atequilibrium compared to reactants?For the reaction:Na (g) + 3 M₂ (g)2NHs (g) + 92kat an equilibrium temperature of 1000°C, a 1.00 L flask contains 0.120 moles ofammonia, 1.03 moles of nitrogen and 1.62 moles of hydrogen. Calculate theequilibrium constant at this temperature.7. At equilibrium at 1120°C the concentration of the reactants and products are found tobe CO=0.010M, H₂O- 0.020M, CO₂-0.010M, and H₂=0.010M. For the followingreaction, does the equilibrium favour the formation of the products or the reactants?CO (g) H₂0 (g) H₂(g) + CO₂(g)For the following reaction at equilibrium at 2000°C, K=1.6 x 10¹.2 NO(g) N (g) 0: (g)The concentration of NO is 0.13 mol/L. If the concentrations of Na and O₂ are equal,calculate the concentration of N₂.Consider the reaction: 2 IFs (g) + laF2 (g)31 (g) 6 F2 (g)6.0 mol of IFs and 8.0 mol of 1.F2 are placed in a 5.0 L container. At equilibrium,6.0 mol of Fa are present.Calculate K for this reaction.For the reaction: 250 (g)At equilibrium, [0₂] = 0.30 M.placed in the container?250: (g) 0: (g)K=0.2What was the initial concentration of SO, that was

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Answered: 1. Write the equilibrium constant…

1. Write the equilibrium constant expression for each of the following rea 2 NO. ( a) Na () b) 2 C(s) <) la (aq) 20, 3 Hi(K) Calle (x)

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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If at 400°C the equilibrium constant for the reaction NO2(g) + H2(g) = NO(g) + H₂O(g) has Kp = 7.28 x 10-6, what is AG for this reaction at 400°C? (1) 66.2 kJ/mol O (3) 654 kJ/mol O (4) 388 kJ/mol O (2) 39.3 kJ/mol # 3 A Moving to the next question prevents changes to this answer. E $ 4 R % 5 T C 6 MacBook Pro Y & 7 U * 8 - 9 K 0 0 L P Question 2 of + 11
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1) Given the following reaction what is the expression for K.? 2502 (9) + 02 (g) = 2503 (g) a) What is the expression for the equilibrium constant? b) If the equilibrium constant for this reaction is 3.70 X 10-7, are the products or the reactants favored? c) What is the equilibrium constant for the reverse reaction? d) What is the equilibrium constant for the reaction below? 6 SO; (g) 6 SO, (g)+ 3 O, (g)
At high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.
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1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) ΔΗ, 298
4 (a) Calculate the value of Kc for the reaction: PC15 ( PC13 ( + Cl2 (g) AH = Positive Given that when 8.4 mol of PC15 (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PC15 (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (i) Increasing temperature (ii) Lowering the concentration of chlorine (Cl₂) (iii) Addition of a catalyst
3. 3. Some CO, is removed from the equilibrium system shown below. Which of the following statements is/are true when the equilibrium responds to this stress? CO(NH)(g) + H,O(g) + E CO.(g) + 2 NH, a. heat is released as the equilibrium shifts to replace the removed CO, b. the quantity of NH, will rise twice as much as CO, c. the quantity of H,O(g) will rise d. both a and b are true e. both b and c are true
3. (a) (b) (c) (d) Write the expression for the equilibrium constant (K) of the following reactions: Fe2+ (aq) + 2OH(aq) Fe(OH)₂ (s) CH4 (g) + 3 H2O (g) = CO (g) + 3 H₂ (g) 2 NO(g) + O₂(g) = 2 NO₂ (g) 2+ Zn(s) + Cu²+ (aq) = Zn²+ (aq) + Cu(s)
Qq.60 . Subject :- Chemistry
G.92.