A 4.00 L flask at 25 °C is filled with 0.266 moles of X2 and 0.344 moles of Y2 and allowed to react according to the following reaction: 3X2 (g) +Y 2 (g) –→ 2Y X3 (g) When the reaction reaches equilibrium it has 0.0465 moles of YX3, what is the equilibrium constant Kc at 25 °C? O 1.34 O 14.3 O 2.95 O 0.0701 O 0.00581

A 4.00 L flask at 25 °C is filled with 0.266 moles of X2 and 0.344 moles of Y2 and allowed to react according to the following reaction: 3X2 (g) +Y 2 (g) –→ 2Y X3 (g) When the reaction reaches equilibrium it has 0.0465 moles of YX3, what is the equilibrium constant Kc at 25 °C? O 1.34 O 14.3 O 2.95 O 0.0701 O 0.00581

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

Consider the following equilibrium system at 539 K. 2CH2C12 (g) 2 CH, (g) + CCL4 (g) If an equilibrium mixture of the three gases at 539 K contains 4.99 × 10-² M CH2C12, 5.54 × 10-2 M CH4, and 4.90 × 10-2 M CC14, what is the value of the equilibrium constant K?
At a certain temperature, the equilibrium constant K for the following reaction is 6.0 x 10: co(e) + H,0(g) -co,() + H,(g) Use this information to complete the following table. Suppose a 31. L reaction vessel is filled with 1.1 mol of co, and 1.1 mol of H2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little CO and H,0. O There will be very little Co, and H,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] Co,(0)+H,(0) CO()+H,O(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 3 CO0g)+3H,0(9) 3 CO,(0)+3H,(9) 1.
When 3.00 mol of A and 1.00 mol of B are mixed in a 1.00 L vessel, the following reaction takes place: A(g) + B(g) →2 C(g). The equilibrium mixture contains 0.50 mol of C. What is the value of the equilibrium constant for the reaction? 0.24 8.3 O 0.20 0.12
Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 1.22×10-2 moles of COCl2(g), 0.591 moles of CO, and 0.561 moles of Cl2 are at equilibrium in a 15.3 L container at 789 K, the value of the equilibrium constant, Kc, is
At a certain temperature, the equilibrium constant K for the following reaction is 0.71: N2(g) + O2(g) =2 NO(g) Use this information to complete the following table. Suppose a 43. L reaction vessel is filled with 1.0 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K =0 2 NO(g) N,(9)+O2(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 3 N2(9)+30,(9) 6 NO(g)
At a certain temperature, the equilibrium constant K for the following reaction is 0.0017: CO(g)+ H₂O(g) CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 27. L reaction vessel is filled with 1.5 mol of CO and 1.5 mol of H₂0. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. CO,(9)+H,(9) CO(g)+H,O(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 CO(g) + 2H₂O(g) 2 CO₂(g)+2H₂(9) There will be very little CO and H₂O. There will be very little CO₂ and H₂. Neither of the above is true. K = 0
At a certain temperature, the equilibrium constant K for the following reaction is 0.0036: H₂(g) + 1₂(g) → 2 HI(g) Use this information to complete the following table. O There will be very little H₂ and I2. Suppose a 6.0 L reaction vessel is filled with 1.9 mol of H₂ and 1.9 mol of I₂. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little HI. ONeither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 HI(g) H₂(9)+1₂(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 H₂(g) +21₂(g) 4 HI(g) 0x10 ?
The following reaction has an equilibrium constant, Kc equal to 3.59 at 900 °C. CH4(g) + 2H₂S(g) — CS2(g) + 4 H2(g) At a particular time during the reaction, the following composition has been found: [CH4(g)] = 1.20 M, [CS2(g)] = 1.15 M, [H₂S(g)] = 1.31 M, [H2(g)] = 1.85. Predict the activity of the reaction during the particular time above. The reaction should go to the left (or reverse) The reaction should go to the right (or forward) The reaction is at a standstill The reaction activity cannot be determined There is no basis for prediction.
At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?
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=
Some CH,Cl, is placed in a sealed flask and heated to 589 K. When equilibrium is reached, the flask is found to contain CH,Cl2 (4.80×102 M), CH4 (4.04x10 2 M), and CCl, (4.36x102 M). What is the value of the equilibrium constant for this reaction at 589 K? 2CH;Cl½(g)= CHĄ(g)+ CC14(g) K=
explain step by step