We follow the speed of the following reacton: A => 2 Y + 32V The experimental data has been plotted. 1) What is the reaction order with respect to "A"? 2) What is the value of T1/2? 3) What is the value of the speed constant "k"?

Consider the following reaction: 2A + B + 3C. (a) Write an expression for the overall rate; (b) What are the rates at which A and B are consumed and generated if C is created at a rate of 0.015 M/min?

The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)

The gas phase reaction between hydrogen and iodine is proposed to occur as follows: step 1: 12 →21 step 2: step 2 H₂ + 2 I (a) Identify the molecularity of each step in the mechanism. step 1 → 2 HI + (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + (c) Identify any intemediates in this mechanism. Intermediate: Enter formula. If none, leave box blank:

a) What are the units of the rate constant for a zero-order reaction?b) What are the units of the rate constant if rate =k[A]5[B]3[C]?c) What is the order of reaction for part (b) of this question?

For a reaction 3A + 4B -> 5C What is the global order of reaction? 3 7 12 Cannot be determined with this information

9:21 < A) s-¹ B) M-¹s-¹ The reaction, 2 NO(g) + O₂(g) → 2 NO₂(g) has a rate law, rate = k{NO] [O₂]. If the rate of the reaction is 0.60 M/s when [NO] is 1.5 M and [O₂] is 2.0 M, what are the units of the rate constant, k? C) Ms-¹ Question 5 of 20 D) M-²S-¹ E) None of these. 11 Tap here or pull up for additional resources Submit