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Question 2 Select reaction rate equations for this chemical reaction: A+B 3C +2D Rate Δ[Α] 1...
PART A ) Consider the reaction:4A + 6B → 3C + 2D If the rate of change of D at a given point in time is 0.180 M/s, what is the rate of change of B at this same time? PART B) For the following reaction: 2A + B → 2 C The rate law is determined to be: rate = 0.4357 [A][B] What will be the initial rate (in M/s) if initial concentrations are: [A] = 0.500 M, [B]...
Consider the reaction: Cl2(g)+3F2(g)→2ClF3(g) Δ[Cl2]/Δt = -0.012 M/s . 1)Find Δ[F2]/Δt 2)Find Δ[ClF3]/Δt 3)Find the rate of the reaction.
For the overall hypothetical reaction A + 5B → 4C, the rate of appearance of C given by Δ[C]/Δt is the same as Select one: a. Δ[A]/Δt b. -(5/4)(Δ[B]/Δt) c. -(4/5)(Δ[B]/Δt) d. none of the above
Question 2 1 pt Which of the following chemical equations indicates that the reaction can achieve equilibrium? OA->B O A<-->B A --> -->A A-->A Question 3 1 pts Select all of the ways that one can increase the rate of a reaction. Increase the concentration of products Increase the temperature Increase the concentration of reactants Add a catalyst
Given the information A+B⟶2D. Δ?∘=−670.8. ΔS∘=380.0 J/K C ⟶D. Δ?∘ = 424.0 kJ Δ?∘=−121.0 J/K calculate Δ?∘ at 298 K for the reaction A+B⟶2C
a) Which of the following is NOT a rate? kg/hour mol/g mol/second g/minute b) Which is a valid way to express reaction rate for N2(g) + 3 H2(g) → 2 NH3(g)? rate = - Δ[N2]/Δt, rate = -1/3 Δ[H2]/Δt, rate = 1/2 Δ [NH3]/Δt rate = Δ[N2]/Δt, rate = 1/3 Δ[H2]/Δt, rate = -1/2 Δ [NH3]/Δt rate = - Δ[N2]/Δt, rate = -3 Δ[H2]/Δt, rate = 2 Δ [NH3]/Δt rate = Δ[N2]/Δt, rate = 3 Δ[H2]/Δt, rate = -2 Δ...
Consider the 2 following reactions: A +B --> C+2D (Δ G r x n= 525 k J) 2B -->3D (Δ G r x n = 490 k J) What is the Equilibrium constant of the reaction A+D --> C+B at T=298K? Instruction: Write your answer in units of 10-7
Question 36 Select the major product formed during this reaction Δ O to do a b d е a. 0 b. 0 C. 0 d. O e.
For the hypothetical reaction 2A + B --> 3C + D, the rate was determined to be: rate = k[A]3[B]1. What is the order of reaction with respect to A? _______ with respect to B? _______ What is the overall order of the reaction? __________
The rate of a chemical reaction can be measured as the rate of appearance of any of the products or as the rate of disappearance of any of the reactants. These relative rates of reaction are related through the stoichiometry of the overall reaction. For example, the rate of the reaction shown below can be determined by measuring the initial rate of disappearance of I, -A[I/At. Cl03-(aq) + 91. (aq)+ 6 H+ (aq) → 31.3 (aq) + Cl-(aq) + 3H20...