Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 1.5 L reaction vessel contained a mixture of 5.0 × 10-² M SO3, 3.5 × 10-3 M O2, and 3.0 × 10-³ M SO₂ at 800.0 K. What are the values of Kc and Kp for the reaction at this temperature? 2 SO₂(g) + O₂(g) = 2 SO³(g) Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [5.0 x 10-²] [3.0 x 10-³1² Once the expression is constructed, solve for Kc. Complete Parts 1-2 before submitting your answer. [3.5 x 10-³] 2[5.0 x 10-²] 1 Кс = [3.0 x 10-³] 2[3.5 × 10-³] [3.3 x 10-²] 2[3.0 x 10-³] 2 [2.3 x 10-³] 7.9 x 104 [2.0 × 10-³] 1.3 x 10-5 [5.0 x 10-²1²2 NEXT 2.1 x 10-4 RESET [3.5 x 10-³1² 4.8 x 10³

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 1.5 L reaction vessel contained a mixture of 5.0 × 10-² M SO3, 3.5 × 10-3 M O2, and 3.0 × 10-³ M SO₂ at 800.0 K. What are the values of Kc and Kp for the reaction at this temperature? 2 SO₂(g) + O₂(g) = 2 SO³(g) Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [5.0 x 10-²] [3.0 x 10-³1² Once the expression is constructed, solve for Kc. Complete Parts 1-2 before submitting your answer. [3.5 x 10-³] 2[5.0 x 10-²] 1 Кс = [3.0 x 10-³] 2[3.5 × 10-³] [3.3 x 10-²] 2[3.0 x 10-³] 2 [2.3 x 10-³] 7.9 x 104 [2.0 × 10-³] 1.3 x 10-5 [5.0 x 10-²1²2 NEXT 2.1 x 10-4 RESET [3.5 x 10-³1² 4.8 x 10³

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

103 kJ + 2HBr(g) = H₂(g) + Br₂(g) A system at equilibrium contains the following pressures of gases. PHBr 107.7 atm PH₂ = 2.5 x 10-8 atm PBr₂ = 2.5 x 10-8 atm What is the equilibrium constant for the reaction at this temperature? K=[?] x 101 Coefficient (green) Exponent (yellow) Enter
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 3.0 L reaction vessel contained a mixture of 1.37 x 10-2 M HI, 6.47 × 10-3 M H2, and 5.94 × 10-4 M I, at 740 K. What are the values of Kc and Kp for the reaction at this temperature? H2(g) + 12(g) = 2 HI(g) 1 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. K. = 2 RESET [1.37 x 10-2] [6.47 x 10-3] [5.94 × 10-4] [4.57 × 10-3] [2.16 х 10-3] [2.31 x 10-4] 2[1.37 x 10-2] 2[6.47 x 10-3] 2[5.94 x 10-4] [1.37 х 10-7)2 [6.47 x 10-312 [5.94 x 10-4]2 3.56 x 103 2.81 × 10-4 48.8 2.05 x 10-2
write your answer in scientific notation
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
Consider the following reaction at a certain temperature: 4 Fe(s) + 3 O2(g)→ 2 Fe203(s) An equilibrium mixture contains 1.2 mol Fe, 0.00090 mol O2, and 2.0 mol Fez03 all in a 2.0-L container. Calculate the value of K for this reaction. K =
Some NOBR is placed in a sealed flask and heated to 385 K. When equilibrium is reached, the flask is found to contain NOBR (9.30×103 M), NO (1.27x102 M), and Br2 (1.18×102 M). What is the value of the equilibrium constant for this reaction at 385 K? 2NOBR(g)=2NO(g) + Br2(g) K=
Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 1 atm of NOBr is sealed in a flask. At equilibrium, the partial pressure of NOBr is 0.82atm. What is the equilibrium constant, Kp, for the reaction?
Consider the following reaction where K = 77.5 at 600 K. CO(g) + Cl₂(g) 2 CoCl₂(g) A reaction mixture was found to contain 1.89×10-² moles of CO(g), 4.43×10-² moles of Cl₂(g) and 0.106 moles of COCI₂(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBR(g) =2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 298K contains NOBR at a pressure of 0.200 atm and NO at a pressure of 0.347 atm, the equilibrium partial pressure of Br2 is atm.
Q2
At 900 K, the following reaction has Kp = 0.345: 2 SO2(g) + O2(g) ⇋ 2 SO3(g). In an equilibrium mixture, the partial pressure of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?
The equilibrium constant for the following reaction is 49 at 450 °C. If 0.22 mole of I2 , 0.22 mole of H2 , and 0.66 mole of HI were put into an evacuated 1.00-liter container, would the system be at equilibrium? If not, what must occur to establish equilibrium? H2 (g) + I2 (g) = 2HI (g)