Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 102 M to 2.5 x 10²M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. T' T. O Word(s) III !!!

Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 102 M to 2.5 x 10²M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. T' T. O Word(s) III !!!

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 for the reaction 2SO,(g) + O2(g) = 250;(g) is 3.1 x 102 at a certain temperature. Determine the equilibrium concentration of sulfur trioxide [SO3], if the equilibrium conce sulfur dioxide [SO2] and oxygen [O2] are 0.0191 M and 0.041 M, respectively.
Nitrogen oxides are air pollutants produced by the reaction of nitrogen and oxygen at high temperatures. At 2000 °C, the value of the equilibrium constant for the reaction, N2(g)+O2(g)=2NO(g), is 4.1 x 10-4. Find the concentration of NO(g) in an equilibrium mixture with air at 1 atm pressure at this temperature. In air, [N,] = 0.036 mol/L and [O,] 0.0089 mol/L.
The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Kc? Cl₂(g) + H₂O(g) = 2 HCl(g) + 1/2 O₂(g) K = 7.52 × 10-2 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) OK= 5.66 x 10-3 OK= 13.3 OK= 0.150 OK = 177 OK = 3.65 K = ?
At a certain temperature, the equilibrium constant K for the following reaction is 6.09 × 10 °: N,(3) + O,(g) =2 NO(g) Use this information to complete the following table. Suppose a 28. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N2 and O2. 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 = ] 2 NO(g) N3(9)+O2(9) 1L What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2N2(9)+20,(9) 4 NO(g)
Suppose a 500. mL flask is filled with 1.7 mol of Cl₂, 1.1 mol of CHCl3 and 1.3 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HC1(g) +CC14 (g) The equilibrium constant K for this reaction is 9.41 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. 10999
Write the pressure equilibrium constant expression for this reaction. 2CH3OH(l)+3Os(g) --> 2CO2(g)+4H2O(g)
Suppose a 250. mL flask is filled with 1.6 mol of Br₂, 0.70 mol of OC12 and 0.50 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrCl(g) The equilibrium constant K for this reaction is 2.87 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places. M Ś
Consider the following equilibrium. N2(s) + O2(g) 2 NO(g) At 2300 K, the equilibrium constant K - 1.7 x 10. Suppose that 0.015 mol NO(g), 0.16 mol N, (9), and 0.16 mol O, (9) are placed into a 10.0 L flask and heated to 2300 K. (a) Is the system at equilibrium? If the system is not at equilibrium, in which direction must the reaction proceed to reach equilibrium? The system is at equilibrium. OThe system is not at equilibrium. The reaction must proceed to the left. The system is not at equilibrium. The reaction must proceed to the right (b) Calculate the equilibrium concentrations of all three substances. (Enter unrounded answers.) [02 - [NO M
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 2 H₂O(g) 2 H₂(g) + 2NO(g) = -9 K₂=3.x 107 He fills a reaction vessel at this temperature with 15. atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. O yes O no 0 atm 0 10 X