13.48. Determine the overall order of the following rate laws and the order with respect to...
For each of the following rate laws, determine the order with respect to each reactant and the overall reaction order. Rate = [A]°[B]2 Order with respect to B = Overall order = Order with respect to A = Submit Answer Tries 0/99 Rate = [A]2[B] Order with respect to B = Overall order = Order with respect to A = Submit Answer Tries 0/99 Rate = [A]”[B]3. Order with respect to B = Overall order = Order with respect to...
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (For each answer, enter an exact number as an integer or decimal.) rate = k [X]"m[2]2 Overall Overall [zi* rate = k Overall
Use the following data to determine the order of reaction with respect to each reactant and the overall order: A + 5B + 6C + 3D + 3E Experiment [A] (M) [B] (M) [C] (M) -4 1 0.35 0.35 0.35 2 0.70 0.35 0.35 Initial Rate (M/s) 8.0 x 10 3.2 x 10-3 6.4 x 10-3 3.2 x 10-3 3 0.70 0.70 0.35 4 0.70 0.35 0.70 1) Order with respect to A = 2) Order with respect to B...
Which of the following rate laws represents a reaction that is second order overall? A. rate = k [A][B]2[C] B. rate = k [A]2[B]2[C]2 C. rate = k [A][B] D. none of these E. rate = k [A]2 [B]
ine the overall orders of the reactions to which the following rate laws apply: (a) rate-kfNO2F, (b) rate-k, (c) rate-klH|[ Brat (d) rate-HNO]2 [에
3. A reaction has two reactants A and B. What is the order with respect to each reactant and the overall order of the reaction described by each of the following rate expressions? a) rate = ki[A] b) rate = k2[A][B] A=3 A=1 B=0 B=1 c) rate = k3[A][B] d) rate = ka[B] A=0 B=a B=1 What are the units of the rate constants in Question 3 if the rate is expressed in mol/L*min? a) b) 4. b)
Give the individual reaction orders for all of the following substances and the overall reaction order from the following rate law: Rate = k[BrO_3^-][Br^-][H^+]^2 Order with respect to BrO_3^-: Order with respect to Br^-: Order with respect to H^+: Order overall:
2- The integrated form of the pseudo rate law depends on thereaction order with respect to CV. The integrated rate laws for y=1 (1st order) and 2 (2nd order) are given in Equations 3 and 4. Compare each with the general form of a linear equation, y=mx+b. In[CV]t = - k't + In[CV]0 (3) 1/[CV]t = k't + 1/[CV]O (4)
+ Using Integrated Rate Laws The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mx + b. Slope Order O 1 2 Integrated Rate Law Graph [A] = - kt + [A] [A] vs. t In[A] = -kt + In[A], In[A] vs. t LÀ=kt + TA LÀ vs. t -k Review Constants Periodic Table Part A The reactant concentration in a zero-order reaction was...
Integrated Rate Laws: Working with First Order Reactions What is the rate constant (min-1) of a first order reaction where the concentration of the reactant decreases by one fourth in 28.0 minutes?