The elementary reaction 2 H₂O(g) 2 H₂(g) + O₂(g) proceeds at a certain temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.0200 atm, 0.00350 atm, and 0.00300 atm, respectively. What is the value of the equilibrium constant at this temperature? = Kp = D $ 4 Incorrect 1.84 X10-6 C R F Search or type URL % 5 V T MacBook Pro G A 6 B Y & N 7 H U N +00 8 J → I M ( 9 K O < -0 ) O L command P • V I' : ; t { option [ + 11 = ? 1 11 } ] C dele I

The elementary reaction 2 H₂O(g) 2 H₂(g) + O₂(g) proceeds at a certain temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.0200 atm, 0.00350 atm, and 0.00300 atm, respectively. What is the value of the equilibrium constant at this temperature? = Kp = D $ 4 Incorrect 1.84 X10-6 C R F Search or type URL % 5 V T MacBook Pro G A 6 B Y & N 7 H U N +00 8 J → I M ( 9 K O < -0 ) O L command P • V I' : ; t { option [ + 11 = ? 1 11 } ] C dele I

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...

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For the following reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.6 × 106 [SO2]= 0.025M [O2]=0.035M Calculate [SO3]eq 0.025 5.9 35 1400
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+ 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 CH₁, 2.8 mol H2S, 0.63 mol CS2, and 0.042 mol H2 at 93.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH(g) + 2 HS(g) = CS₂(s) + 4 H2(g) 1 2 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. Once the expression is constructed, solve for Kc. [0.042]4 Кс = [2.8]² [1.2] || 6.6 × 10-8 RESET [1.2] [2.8] [0.63] [0.042] [0.24] [0.56] [0.13] [0.0084] 2[2.8] [2.8]² 2[0.56] [0.56]² 4[0.042] [0.042]4 4[0.0084] [0.0084]* 0.063 16 6.6 × 10-8 1.5 × 107
tab esc An evacuated reaction vessel is filled with 0.80 atm of N and 1.68 atm 2 of Br. When equilibrium is established according to the reaction below, there are 1.42 atm of Br, remaining in the vessel. What is Kp for this reaction? 2 2 NBr. (g) = N₂(g) + 3 Br₂ (g) ! Q 2 F2 W #3 3 20 F3 E $ 4 888 R 67 80 % 5 Question 17 of 21 F5 < MacBook Air 6 F6 Y & 7 F7 U 8 F8 ( 9 F9 1 4 7 +/- O O 2 LO 5 4 F10 11.6 P 3 8 9 CO 6 0 F11
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Given that Kp - 3.0 x 10 for the reaction: 2 CO(g) C(graphite) + CO2(g). what is the partial pressure of CO2(g) at equilibrium if initially 4.00 atm of CO(g) is in contact with graphite? MA. 0.0024.atm B. 0.0060 atm C.0.0048 atm D.0.0012 atm E. 0.0096 atm
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Consider the reaction for the decomposition of hydrogen disulfide: 2H₂S(g) 2H2(g) + S2(g), 1.67 x 10-7 at 800°C K The reaction is carried out at the same temperature with the following initial concentrations: [H₂S] = [H₂] [S₂] 2.00 × 10-4M 0.00 M = 0.00 M Part A Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units. [S2] = 1.89 10-5 M Submit Previous Answers Request Answer ?