1)
rate of reaction = (1/2)*rate of formation of NH3 = (1/3)*rate of disappearance of H2 = rate of disappearance of N2
USE:
(1/3)*rate of disappearance of H2 = (1/2)*rate of formation of NH3
rate of disappearance of H2 = (3/2)*rate of formation of NH3
rate of disappearance of H2 = (3/2)*0.04 mol/L.min
= 0.06 mol/L.min
Use:
rate of disappearance of N2 = (1/2)*rate of formation of NH3
= (1/2)*0.04 mol/L.min
= 0.02 mol/L.min
2)
rate of reaction = (1/5)*rate of consumption of Bromide = (1/3)*rate of formation of H2O
Use:
(1/3)*rate of formation of H2O = (1/5)*rate of consumption of Bromide
rate of formation of H2O = (3/5)*rate of consumption of Bromide
= (3/5)*0.20 mol/L.s
= 0.12 mol/L.s
Please answer as many questions as you can Thanks 1. For the reaction, N2(g) 3H2(g)2NH3(g). if...
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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
1/ The Following data was obtained while observing a reaction between nitric oxide and hydrogen: F2(g) + 2CLO2(g) -----> 2FCLO2(g) Experiment Initial(F2) Initial(CLO2) Initial rate (mol/L) (mol/L) (mol/L*s) 1/ 0.10 0.010 1.2 x 10^-3 2/ 0.10 0.040 4.8 x 10^-3 3/ 0.20 0.010 2.4 x 10^-3 A/ write the rate law for this reaction B/ calculate the rate constant for the reaction C/ what is the order of this reaction 2/ consider the reaction N2(g) + 3H2(g) ----> 2NH3(g). At...
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.
Consider the reaction: N2(g) + 3H2(g) <---> 2NH3(g) The Gibbs free energy of formation ((delta)Gfo) for ammonia is -16.5 kJ/mol and the reaction is exothermic. Calculate the (delta)Gorxn and the equilibrium constant for the reaction and clearly state whether K increases or decreases with temperature.
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.
Study the chemical reaction. N2(g) + 3H2(g) + 2NH3(g) How many moles of Nz will react with 1.5 moles of H2? O 1.5 mol 1.0 mol 2.0 mol O 0.5 mol
Consider this reaction: N2(g) + 3H2(g) <==> 2NH3(g) If the Kc for the reaction is 4.5 x 10^4 at 127 degrees celsius, what is the equilibrium constant, Kp at the same temperature?
1. An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.15 mol/L of N2 and 0.20 mol/L of H2, she finds that the H2 concentration has fallen to 0.10 mol/L after 20. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). 2. What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). 3. Estimate the N2...
Calculate KC in terms of molar concentration for the reaction N2(g) + 3H2(g) 2NH3(g) when the equilibrium concentration moles per liter are: N2 = 0.02, H2 = 0.01, NH3 = 0.10.