Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Step 1: Equilibrium constant
The equilibrium constant can be determined in terms of concentration, and pressure.
In terms of concentration, it is represented as Kc
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- 4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) 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 [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)arrow_forward1. Please don't write on a paper. I can't understand handwritten.arrow_forwardAt room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).arrow_forward
- An equilibrium reaction has a K = 3.2 x 10-4. What can be said about the reaction? [Reactants] [Products] [Reactants]> [Products] [Reactants] [Products] < =arrow_forwardConsider the reaction. А(аq) — 3 В(аq) K. = 2.15 x 10-6 at 500 K If a 4.80 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] =arrow_forwardDetermine the concentration of all species at equilibrium for each of the following original mixtures. At 40C K= 1.7*10^-5 2NOCl(g) ——-(reversible)—— 2NO(g) + Cl2(g) a) 2moles of NOCl 2 moles of NO 1 mole or Cl2 in 1.0L flask b) 1M concentration of all three gasesarrow_forward
- NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.arrow_forward6. Write the equilibrium constant expression for the following reactions. a. CHa (8) + 20; (B) → CO; (B) + 2H;0 (g) b. 4 NH3 (g) + 302 (g) → 2N2 (g) + 6H;0 (g) c. C (s) + 2H2 (g) CH4 (g)arrow_forward
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