Provide clear explanation and show work for each chart. Thank you StressChp 13Chemical Equilibrium: Le Chatelier's Principle PracticeUse what you know about Le Chatelier's Principle to fill in the tables for each reaction below.2NO3 (g) + HEAT[N₂][0₂](1,↓, or same) (1,, or same)Add N₂Add NO3Remove O₂Remove N₂DecreaseTemperatureIncrease PressureStressAdd AgAdd AgBrIncreaseTemperatureExperiment 16 Prelaboratory AssDecrease PressureN2 (g) + 302 (g)Equilibrium shift(, → or none)AgBr(s) <> Ag (n)Equilibrium shift(←, → or none)+ Br (aq) + HEATAgBr(1,, or same)Bonus.1[Ag](1,, or same)[NO3](1,, or same)[Br](1,, or same)

The Le chatelier's principle states that , " When any chemical reaction is in equilibrium and a…

Chemical Equilibrium: Le Chatelier's Principle Practice Use what you know about Le Chatelier's Principle to fill in the tables for each reaction below. N2 (g) + 302(g) → 2NO3 + HEAT Stress Add N₂ Add NO3 Remove O₂ Remove N₂ Decrease Temperature Increase Pressure Equilibrium shift (→ or none) [N₂] (1,, or same) [0₂] (1,, or same) [NO3] (1,, or same)

Chemical Equilibrium: Le Chatelier's Principle Practice Use what you know about Le Chatelier's Principle to fill in the tables for each reaction below. N2 (g) + 302(g) → 2NO3 + HEAT Stress Add N₂ Add NO3 Remove O₂ Remove N₂ Decrease Temperature Increase Pressure Equilibrium shift (→ or none) [N₂] (1,, or same) [0₂] (1,, or same) [NO3] (1,, or same)

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 16Q: Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there...

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A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?
What is the value of the equilibrium constant expression for the change H2O(l)H2O(g) at 30 C?
Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At zero time, only A, B, and C are present. The reaction reaches equilibrium 10 min after the reaction is initiated. Partial pressures of A, B, and D are written as PA, PB, and PD. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) PD at 11 min PD at 12 min. (b) PA at 5 min PA at 7 min. (c) K for the forward reaction K for the reverse reaction. (d) At equilibrium, K Q. (e) After the system is at equilibrium, more of gas B is added. After the system returns to equilibrium, K before the addition of B K after the addition of B. (f) The same reaction is initiated, this time with a catalyst K for the system without a catalyst the system with a catalyst. (g) K for the formation of one mole of D K for the formation of two moles of D. (h) The temperature of the system is increased to 35C. PB at equilibrium at 25C PB at equilibrium at 35C. (i) Ten more grams of C are added to the system. PB before the addition of C PB after the addition of C.
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Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH3CO2HAceticacid+C2H5OHEthanolCH3CO2C2H5Ethylacetate+H2OK=2.2 For the following mixtures (a-d), will the concentration of H2O increase, decrease, or remain the same as equilibrium is established? a. [CH3CO2C2H5] = 0.22M, [H2O] = 0.10M, [CH3CO2H] = 0.010 M, [C2H5OH] = 0.010 M b. [CH3CO2C2H5] = 0.22 M, [H2O] = 0.0020 M, [CH3CO2H] = 0.0020 M, [C2H5OH] = 0.10 M c. [CH3CO2C2H5] = 0.88 M, [H2O] = 0.12 M, [CH3CO2H) = 0.044 M, [C2H5OH] = 6.0 M d. [CH3CO2C2H5] = 4.4 M, [H2O] = 4.4 M, [CH3CO2H] = 0.88 M, [C2H5OH] = 10.0 M e. What must the concentration of water be for a mixture with [CH3CO2C2H5] = 2.0M, [CH3CO2H] = 0.l0 M, and [C2H5OH] = 5.0 M to be at equilibrium? f. Why is water included in the equilibrium expression for this reaction?
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