4. Consider the two reactions given below.ReactionREACTION AREACTION BEquation• 20,(g) = 3 0,(g)N,(g) + 0,(g) =2 NO(g)Picture1/K valueK = 3.5x10-89(very small)K = 1.0x1025(very large)[CWrite theK =equilibriumK =[A]<[B]constantexpression.Was the K>1or <1?Which is mnorecommon inthe reactionmixture:reactants orproducts?

Equilibrium is a position at which the reaction is not complete but the concentration of reactants…

Reaction REACTION A REACTION B Equation 20,(g) 는3 0,(g) N,(g) + 0,(g) =2 NO(g) Picture K value K = 3.5x10-89 (very small) K = 1.0x1025 (very large) Write the K = equilibrium K = [A]*[B] constant expression. Was the K>1 or <1? Which is more common in the reaction mixture: reactants or products?

Reaction REACTION A REACTION B Equation 20,(g) 는3 0,(g) N,(g) + 0,(g) =2 NO(g) Picture K value K = 3.5x10-89 (very small) K = 1.0x1025 (very large) Write the K = equilibrium K = [A]*[B] constant expression. Was the K>1 or <1? Which is more common in the reaction mixture: reactants or products?

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

The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?
Question 41 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 x 10 at a certain temperature. If a solid sample of CaCrO4 dissolves in solution, what will the equilibrium concentration of Ca in the solution be? CaCrO.(s)= Ca (aq) + CrO (aq) NEXT Based on the given values, set up ICE table in order to determine the unknown. CaCrO-(s) Ca-(aq) CrO. (aq) Initial (M) Change (M) +2x +2x Equilibrium (M) 7.1 x 10-2x +2x +2x RESET 7.1 x 10 +2x -2x 7.1 x 10 +* 7.1 x 10-r 7.1x 10+ 2x 7.1x 10-2x
35 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 3.01 × 10³ at 900 K. If an initial mixture of 0.0216 mol SO2 and 0.0148 mol O2 reacts in a 1.0 L vessel, what will be the concentration of SO3 at equilibrium? 2 SO:(g) + O2(g)= 2 SO:(g) 1 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. 2 SO:(g) O:(g) + 2 SO:(g) Initial (M) 0.0216 0.0148 Change (M) 0.0216 - 2x 0.0148 - x Equilibrium (M) 5 RESET 0.0216 0.0148 1.0 +x +2x -2x 0.0216 + x 0.0216 + 2x 0.0216 - x 0.0216 - 2x 0.0148 + x 0.0148 + 2x 0.0148 - x 0.0148 - 2x
R Manipulating Equilibrium Constant Expressions equilibrium constant for the following reaction is 63.3 at 378 °C. K 63.3 at 378 °C H₂(g) + 12(g) = 2 HI(g) culate the equilibrium constant for the following reactions at 378 °C. a) 2 HI(g) = H₂(g) + I2(g) K = (b) HI(g) 1/2 H₂(g) + 1/2 I2(g) Show Approach Show Tutor Steps Submit Submit Answer Try Another Version K = [References] 4 item attempts remaining Previous Next
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
Consider the equilibrium reaction. 3A +B= 2C After multiplying the reaction by a factor of 2, what is the new equilibrium equation? new equilibrium equation: 6A + 2B = 4C Create the equilibrium-constant expression, K, for the new equilibrium reaction. Answer Bank IAP Ke = [B) [B) LA Answer Bank [C] [AP K = [B] (B] [B] (A) If the initial reaction contains 1.79 M A, 1.53 M B, and 2.39 M C, calculate K, for the new equilibrium reaction. K = Incorrect
At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6. Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M. Your answer should have two significant figures.
Consider the following chemical equilibrium: N₂ (g) + 3H₂(g) 2NH3(g) с Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K₁ = 0 P 00 X 5 010
Q1) For the equilibrium: A B, if [A].0.569, [B].0.162, and Kea 47.8, what are [A]es and [B]ea? algebraic expression: [A]eq= Q2) For the equilibrium: 1221, if [2]. 1.26, [1].0, and Keq = 1.14 x10, what are [12]eg and [lleg? E algebraic expression: [H₂leq_ [12]eg [B]ea. algebraic expression: [12]ea. [eq M Q3) For the equilibrium: H₂ + 1₂2H1, if [H₂lo=0.546, [b]o 1.26, [HI].0, and Kea 45.3, what are [Halea, [lzles and [HI]eq? =0 [HI] eq = 0 0
At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6. Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M. Your answer should have two significant figures.
For the reaction 3 O2(g) 2 O3(g) The equilibrium constant, K, has the value 1.12 10-54 at a particular temperature. (b) If the equilibrium mixture is analyzed and [O2(g)] is found to be 3.71 10-2 M, what is the concentration of O3(g) in the mixture? M
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.