Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 2.0 L reaction vessel contained a mixture of 1.2 mol Fe, 1.0 × 10-³ mol O₂, and 2.0 mol of Fe₂O, at 2000.0 °C. What are the values of Kc and Kp for this reaction? 4Fe(s) + 30₂(g) = 2Fe₂O₂(s) NEXT Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [1.2] Once the expression is constructed, solve for Kc. Complete Parts 1-2 before submitting your answer. 2[2.0] 2[1.2] [1.0 × 10³] [0.50] 8.0 × 10⁰ Кс 1 = [2.0] [5.0 x 10²] 1.0 × 10⁹ [1.2]¹ [0.50]* 1.3 x 10-1⁰ [1.0 × 10.³1³ [5.0 × 10.¹1³ 2 = [2.0]² [1.2]² 4[1.2] 4[0.50] > RESET 3[1.0 × 10³] 3[5.0 x 10+]

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 2.0 L reaction vessel contained a mixture of 1.2 mol Fe, 1.0 × 10-³ mol O₂, and 2.0 mol of Fe₂O, at 2000.0 °C. What are the values of Kc and Kp for this reaction? 4Fe(s) + 30₂(g) = 2Fe₂O₂(s) NEXT Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [1.2] Once the expression is constructed, solve for Kc. Complete Parts 1-2 before submitting your answer. 2[2.0] 2[1.2] [1.0 × 10³] [0.50] 8.0 × 10⁰ Кс 1 = [2.0] [5.0 x 10²] 1.0 × 10⁹ [1.2]¹ [0.50]* 1.3 x 10-1⁰ [1.0 × 10.³1³ [5.0 × 10.¹1³ 2 = [2.0]² [1.2]² 4[1.2] 4[0.50] > RESET 3[1.0 × 10³] 3[5.0 x 10+]

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 constant, K, for the following reaction is 10.5 at 350 K. 2CH,Cl2(g) ? CH,(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43x10-2 M CH,Cl,, 0.176 M CH, and 0.176 M CCL. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.124 mol of CH,(g) is added to the flask? [CH,Cl,] = M [CH4) M [CCL] M
A sample of IBr decomposes according to the following equation: 2 IBr(g) 1 I2(g) + 1 Br2(g) An equilibrium mixture in a 1-L vessel at 1926 oC, contains 0.00946 g of IBr, 0.0122 g of I2, and 0.00475 g of Br2.(a) Calculate KP for this reaction at this temperature.KP = (b) What is the total pressure exerted by the equilibrium mixture of gases?Ptotal = atm.
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
The reaction H2(g) + I2(g) 2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 3.01 atm and H2 at a pressure of 2.62 atm. Calculate the equilibrium pressure of I2(g) in this mixture.
At 1560 oC the equilibrium constant for the reaction: 2 IBr(g) I2(g) + Br2(g) is KP = 0.846. If the initial pressure of IBr is 0.00674 atm, what are the equilibrium partial pressures of IBr, I2, and Br2?p(IBr) = p(I2) = p(Br2) =
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)
Some quantity of NOBr is added to an otherwise empty flask. The reaction: 2 NOBr (g) ⇄ 2 NO (g) + Br2 (g) takes place at a particular temperature for which KP is 3.5 x 10-5. Assuming an equilibrium pressure of NOBr = 2.46atm, what is the equilibrium pressure of NO?
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=
The equilibrium constant Kp for the reaction PC15(g) = PC13(g) + Cl₂(g) is 1.05 at 250°C. The reaction starts with a mixture of PC15, PC13, and Cl₂ at pressures 0.177 atm, 0.233 atm, and 0.161 atm, respectively, at 250°C. When the mixture comes to equilibrium at that temperature, which pressure(s) will have decreased? Cl₂ PC13 PC15
The equilibrium constant Kp for the reaction,2 SO3(g) <-------> 2 SO2(g) + O2(g)is 7.880 at 759 °C. If a vessel at this temperature initially contains pure SO3 and if the partial pressure of SO3 at equilibrium is 0.109 atm, what is the partial pressure of O2 in the flask at equilibrium? What was the initial pressure of SO3 in the flask?
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.2 mol CH₄, 2.8 mol H₂S, 0.63 mol CS₂, and 0.042 mol H₂ at 93 °C. What are the values of Kc and Kp for the reaction at this temperature? CH₄(g) + 2 H₂S(g) ⇌ CS₂(s) + 4 H₂(g)