URGENT If 2AB+10kJ-->A2+B2 then the production of 2A2:
produces 20kJ
requires 10kJ
Produces 10kJ
requires 20kJ
URGENT If 2AB+10kJ-->A2+B2 then the production of 2A2: produces 20kJ requires 10kJ Produces 10kJ requires 20kJ
cos2θ = (2ab)/(a2 + b2). Find the values of a and b.
Consider the reaction A2 + B2 ⇌ 2AB. If the initial concentration of both A2 and B2 is 4.0 M, and after 10 minutes the reaction appears to stop. The concentration of [A2] is now 2.0M. d. We can discuss the rate in terms of [A2], [B2], or [AB]. How are they related to each other? - Δ[A2]/Δt = e. What is the difference between Δ[A2]/Δt and d[A2]/dt ? f. At t = 15 minutes has the reaction actually...
2. Consider the reaction A2 + B2 ⇌ 2AB. If the initial concentration of both A2 and B2 is 4.0 M, and after 10 minutes the reaction appears to stop. The concentration of [A2] is now 2.0M. a. Draw a graph of [A2] vs. time, over the span of 20 minutes. b. On the same axes draw a graph of [B2] v time, over a span of 20 minutes. c. On the same axes draw a graph of [AB] v...
2. Consider the reaction A2+ B2 = 2AB. If the initial concentration of both A2 and B2 is 4.0 M. and after 10 minutes the reaction appears to stop. The concentration of [A2) is now 2.0M. a. Draw a graph of [A2) vs. time, over the span of 20 minutes. 09. (M concertuohon 5 15 20 time (min) b. On the same axes draw a graph of [B2] v time, over a span of 20 minutes. c. On the same...
For the reaction A2(g) + B2(g) <=> 2AB(g), calculate the value for Kc at 25oC if [A] = 1.073M, [B] = 1.112M, and [AB] = 24.1M. (assume a minimum of 3 significant figures for each molarity).
CHEMWORK For a reaction of the type A2(g) + B2(8) 2AB(g) with the rate law: d[A2] _ = k[A][B] dt The value of the rate constant at 302°C is 2.45 x 10-4 L/mol s and at 508°C the rate constant is 0.0875 L/mol s. The value of R is 8.3145 J/K mol. Calculate the value of the rate constant for this reaction at 375°C. L/mol s Submit
My reaction is as follows: 2A2 + B2 --> 2A2B A and B represent elements. Based on the following table, choose the appropriate rate law for this reaction! [A2] [B2] Rate 1.0M 1.0M 5.0 Ms-1 2.0M 1.0M 20.0 Ms-1 3.0M 3.0M 233.8 Ms-1 rate = [A2]1[B2]2 rate = [A2]1[B2]1 rate = [A2]2[B2]1 rate = [A2]0[B2]1 rate = [A2]2[B2]2 rate = [A2B]1 rate = [A2]1.5[B2]2 rate = [A2]2[B2]1.5 rate = [A2]1.5[B2]1.5 None of these answers are correct.
Determine which of the formulas hold for all invertible n X n matrices A and B B. (A B2- A2 + B2 +2AB D.A +B is invertible E.ABA-1B F9A is invertible Determine which of the formulas hold for all invertible n X n matrices A and B B. (A B2- A2 + B2 +2AB D.A +B is invertible E.ABA-1B F9A is invertible
3 pts Question 2 Consider the following hypothetical reaction Az (g) + B2 (g) + 2AB (g) [AB where Kc = Ag][B2] 4 AB (g) is The equilibrium constant for the reaction 2A2 (g) +2B2 (8) 1/[Kc^4) o Kc^4 sqrt(Kc) Kc2
Problem 7 The gas-phase reaction, 2A2 + B2 2A2B, is carried out in a constant- volume reactor (volume V) at temperature T. No g-moles each of A2 and B2 are charged to the reactor, which is evacuated initially, and the reaction proceeds to equilibrium. The equilibrium constant Ka of the reaction-which is based on the pure-component standard state of 1 atm and temperature T-is known. The reaction mixture behaves as an ideal-gas mixture. (a) Express the conversion of A2 and...