1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 2NH3 (8) 3H2 (8) If the equilibrium concentrations for all the reactants and products at 600°C are: С [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³ Construct an expression for K and calculate the numerical value of the equilibrium constant, K. N₂ (8) 2 + DH is negative С (ii) At 500°C K = 0.062 mol-2dm. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.

1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 2NH3 (8) 3H2 (8) If the equilibrium concentrations for all the reactants and products at 600°C are: С [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³ Construct an expression for K and calculate the numerical value of the equilibrium constant, K. N₂ (8) 2 + DH is negative С (ii) At 500°C K = 0.062 mol-2dm. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.

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 thermal decomposition of NO2 is 7.32 10-6 at 450 K. If a reaction vessel at this temperature initially contains 0.515 atm of NO2, what will the partial pressures of NO2, NO, and O2 be when equilibrium has been established? Since Kp is small, you can use simplifying assumptions. Be sure not to round your numbers during the calculation and use at least 3 sig figs.
When 0, 1 12 mol of NO and 0, 1 12 mol of Br2 are placed in a 1 ,00 dm3 reaction vessel and sealed, the mixture is heated to 350K and the following equilibrium is established:2 NO (g) + Br2 (g) 2 NOBr (g)If the equilibrium concentration of nitrosyl bromide (NOBr) is 0,0824 mol.dm-3 , what is the value of equilibrium constant(Kc) at 350K?
The equilibrium constant, Kc, for the following reaction is 1.25 at 659 K. 2NH3 (9) N2(g) + 3H₂(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 659 K, the equilibrium concentration of H₂(g) is found to be 0.609 M. Calculate the concentration of NH3 in the equilibrium mixture. [NH3] = Submit Answer Use the References to access important values if needed for this question. M Submit Answer Retry Entire Group 8 more group attempts remaining [Review Topics] [References] Use the References to access important values if needed for this question A student ran the following reaction in the laboratory at 679 K: H₂(g) + I₂(g) → 2HI(g) When she introduced 0.208 moles of H₂(g) and 0.237 moles of I2 (g) into a 1.00 liter container, she found the equilibrium concentration of I2 (g) to be 0.0625 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = | Retry Entire Group 8 more group attempts remaining'
Gas Initial Concentration (M) H2 0.030 I2 0.015 HI ? Samples of three gases, H2(g) , I2(g) , and HI(g) , were combined in a rigid vessel. The initial concentrations of H2(g) and I2(g) are given in the table above. (a) The original value of the reaction quotient, Qc , for the reaction of H2(g) and I2(g) to form HI(g) (before any reactions take place and before equilibrium is established), was 5.56 . On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas. Equilibrium was established at a certain temperature according to the following chemical equation. H2(g)+I2(g)⇄2HI(g)ΔH°rxn=−9.4kJ/molrxn;Kc=49 After equilibrium was established, the concentration of H2(g) was 0.020M . (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part ( a ). The curves must show how the concentration of each of the three gases changed…
A 2 L jar, equipped with a tight-fitting lid that contains a rubber septum, is half filled with water. At equilibrium, the air space has a volume of 1 L, a total pressure of 1 atm, and a temperature of 298 K. The i mg of formaldehyde (HCHO, MW = 30 g/mol) is injected through the septum into the water. Some of the formaldehyde escapes into the gas phase. Consider the situation when a new equilibrium is established. Determine (a) the equilibrium mass concentration of HCHO in water and (b) the equilibrium mole fraction of HCHO in air
Iodine and bromine react to give iodine monobromide, IBr. I1 (9) + Brz (9) = 2IB:(9) What is the equilibrium composition of a mixture at 154°C that initially contained 1.10 x 10- mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant K, for this reaction at 154°C is 130. [1:] =( M [Bra] =( M [IBr] = M
3. The following question is based on the chemical equilibrium shown below: (13 mins) NO2(g) N₂O4(g) (UNBALANCED EQUATION). A. Kp for this reaction is 9.3 x 10-7 at 25°C. What is the equilibrium concentration of N₂O4 in a flask that initially contains only 3.00 atm of NO₂? If any assumptions are made for your calculations, please state them and validate their use. B. What is the value of Kc for this reaction at the same temperature? C. What is the effect on Kp if 1.00 atm of neon gas is added to the system at equilibrium? Useful info: K₂=Kc(RT)An R = 0.08206 (L x atm)/ (mol x K)
Please show all steps clearly to this problem. Thanks
For the reaction, H2(g) + Cl2(g) 2 2 HCI(g), K. = 2.5 x 104 at 3000.0°C. The initial concentration of H2 and Cl2 in a closed container are 0.40 M, respectively. %3D H2lg) 2 HCI(g), a) write the values in the row 'change' (C). b) write the values corresponding to the row at the 'equilibrium' (E). ) calculate the concentrations of reactants and product at the equilibrium.
Acetic acid and water react to form hydronium cation and acetate anion, like this: HCH, CO, (aq)+H, o()- H,O"(aq)+CH;co,(aq) Imagine 67. mmol of CH, CO, are added to a flask containing a mixture of HCH, CO,, H, 0, H,0" and CH, CO, at equilibrium, and then answer the following questions. O Zero. What is the rate of the reverse O Greater than zero, but less than the rate of the forward reaction. reaction before any CH,CO, has been added to the flask? O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse O Greater than zero, but less than the rate of the forward reaction. reaction just after the CH;CO, has O Greater than zero, and equal to the rate of the forward reaction. been added to the flask? O Greater than zero, and greater than the rate of the forward reaction. O Zero. O Greater than zero, but less than the rate of the forward reaction. What is the rate of…
5:13 Question 1 of 17 Construct the expression for Kp for the following reaction. 2 C8H18 (1) + 25 O₂(g) = 16 CO₂(g) + 18 H₂O(l) 1 Kp = Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. PC₂H18 (PC₂H₁) 25 (PO₂)² 16(P co₂) 2(PH,o) 2(PC₂H₁z) Po₂ (P0₂) 25 (PcO₂)² 18(PH,o) Submit 25 (PC₂H₁) 2(P0₂) Pco₂ (PCO₂) 16 (PH₂0)² Tap here or pull up for additional resources RESET (PC₂H₂)² 25 (Po₂) 2(PCO₂) PH₂0 (PH₂0) ¹8
Solve correctly please, (Gpt/Ai wrong ans not allowed)