This process is exothermic and in exothermic process as the temperature is decreased the process shift forwards
As the reaction proceeds forward more product will form
so correct answer is More products will formed
For the following reaction at equilibrium with a given AHºrxn = -207 kJ/mol: N2(g) + 3H2(g)...
Question 5 0/1 point The equilibrium constant for the gas phase reaction N2 (g) + 3H2(g) + 2NH3 (B) is Keq - 4,34 x 10-3 at 300 °C. At equilibrium, Question 5 The equilibrium constant for the gas phase reaction N2 (8) + 3H2 (g) – 2N63 (g) is keq = 4.34 x 10-3 at 300 °C. At equilibrium, products predominate only reactants are present roughly equal amounts of products and reactants are present only products are present reactants predominate
AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g) This calculation was for the reaction under standard conditions—that is, with all gases present at a partial pressure of 1 atm and a temperature of 25°C. Calculate AG for the same reaction under the following nonstandard conditions: . PN2 = 2.00 atm, PH2 = 7.00 atm, PNH3 = 0.021 atm, . and T = 100°C.
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g) What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
Given the following data for heats of reaction N2(g) + 3H2(g) ----> 2NH3(g) H = -91.8 kJ C(graphite) + 2H2(g) -------> CH4(g)H = -74.9kJ H2(g) + 2C(graphite) + N2(g) --------> 2HCN(g) H = 270.3 kJ Calculate H for the reaction used to make HCN CH4(g) + NH3(g) --------> HCN(g) + 3H2(g)
The equilibrium constant, K, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 10.1 L container at 723K contains 0.410 mol of NH3(g) and 0.250 mol of N2, the equilibrium concentration of Hy is M.
The equilibrium constant, Kc, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 15.7 L container at 723K contains 0.284 mol of NH3(g) and 0.437 mol of N2, the equilibrium concentration of H2 is__________ M.
5. Given ΔG =-16.5 kJ/mol for the reaction ½ N2 + 3/2 H2 → NH3, find the equilibrium constant for: (a) the above reaction as written (b) the reaction N2+ 3H2 → 2NH3
The equilibrium constant kc for the reaction N2(g)+3H2(g) ⇌ 2NH3(g), which corresponds to the formation of ammonia by the Haber process, is 2.13 x 106 at 288k and 1.75 x 105 at 308 k. Calculate the standard enthalpy at 298k Answer: -92,2 kJ/mol
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
For the following exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + heat. In which direction does equilibrium shift if the temperature of the reaction vessel is raised. Select one: a. Reaction shifts towards products. b. There is no effect. c. reaction shifts towards reactants