The following reaction is second-order in A and first-order in B: 2 A+B → A₂B What is the reaction rate if k = 2.55 M-²s¹ and [A] = 1.60 M [B] = 0.70 M? Hint: Write down the correct differential rate law based on the order with respect to A and B, then plug in the concentrations and k to calculate rate (R). Your Answer: Answer units

The gas phase reaction of hydrogen with iodine H₂+ 12 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form [A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate In an experiment to determine the rate law, the rate constant was determined to be 2.39 x 10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2]=0.0636 M and [12]=0.0154 M would be M/s. Submit Answer Retry Entire Group more group attempts remaining

Part B Consider the second-order reaction: 2HI(g)→H₂(g) + I₂(g) Use the simulation to find the initial concentration [HI], and the rate constant k for the reaction. What will be the concentration of HI after t = 5.44x10¹0 s ([HI]) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ► View Available Hint(s) for Part B for Part do for Part redo for Part B res@or Part B keyboard shortcuts for Part B help for Part B [HI] = 1.6810³ Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining mol L

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Butadiene, C,H, (used to make synthetic rubber and latex paints) dimerize C3H12 with a rate law of rate = 0.014 L/mo[• s [CH]². If the remäining %3D concentration of CaH, is 0.028 M after 0.35 hours, what is the initial concentration of C4H, in molar? Report a numerical value with 3 decimal places, without units.

The rate constant for the second order reaction 2 NO2 - 2 NO + O2 is 0.24 M's. If a 1.38 M sample of NO2 reacts for 47.7 seconds, what concentration of NO2 wil remain? Report your answer to two decimal places. |Al = - kt +|Alo InJAl = - kt + InlAlo TAI = kt + TAlo

Fe3+ (aq) + 7.00 SCN- (aq) →  Fe(SCN)7.00 3+ (aq) 1.)Find the rate where SCN- is consumed, if Fe3+ is consumed at 1.00 M/min.  2.) Find the rate and the overall order of the rate law

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Be sure to answer all parts. Consider the reaction A+BProducts From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. A. JA] (M) (BỊ (M) Rate (Mis) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10

Be sure to answer all parts. The reaction of peroxydisulfate ion (S2O82−)with iodide ion (I− is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant.  Experiment [S2O82−](M) [I−](M) Initial Rate [M/s] 1 0.0200 0.0520 4.80 × 10−4 2 0.0200 0.0260 2.40 × 10−4 3 0.0400 0.0260 4.80 × 10−4 (a) Which of the following equations represents the rate law for this reaction?  A. rate = k[S2O82−][I−]   C. rate = k[S2O82−][I−]2 B. rate = k[S2O82−]2[I−]   D. rate = k[S2O82−]2[I−]2                    (b) What is the rate constant for the reaction? k =