Using the following rate law and the experimental values given in the question figures, calculate k (with units): Rate = k[F2][ClO2]Rate = k[F2][ClO2]   [F2] (M) [ClO2] (M) Initial Rate (M/s) Experiment 1 0.50  0.50  0.300  Experiment 2 0.80  0.80  0.768  Experiment 3 0.50  0.80  0.480

* Question Completion Status: A Moving to another question will save this response. Question 18 The mechanism for NO2 (g) + CO (g) → NO (g) + CO2 (g) is thought to be: 2 NO2 → NO3 + NO NO3 + CO → NO2+ CO2 (slow) (fast) The rate law for the overall reaction is: Rate = k[NO3][CO] O Rate = k[NO2] Rate = k[NO2]2 O Rate = k[NO2][CO] O Rate = k[NO3][NO] A Moving to another question will save this response. MacBook Air 吕0 F6 esc F3 F4 F5 F1 F2 #3 $4 % 3 4. 6. 回2 Breathe easy

Consider the rate law: Rate = k [A]2[B][C]1/2. How does the rate of the reaction change if the concentration of C is doubled? The rate increases by a factor of 1.414 The rate increases by a factor of 1.732 The rate reduces by a factor of 1.732 The rate triples The rate reduces by a factor of 1.414

The data below were collected for this reaction: CH3Cl (g)         +     3 Cl2(g)     →        CCl4 (g)              +              3 HCl (g)   Expt. [CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 1 0.050 0.050 0.014 2 0.100 0.050 0.029 3 0.100 0.100 0.057   Provide the rate law for this reaction. Include the numerical value of the specific rate constant, k.     Rate = - Δ [Cl2]3 / Δ t     Rate = Δ [HCl] / 3 Δ t     Rate = k [CH3Cl] [Cl2]2     Rate = -Δ [CH3Cl] / 3 Δ t     Rate = 5.7 [CH3Cl] [Cl2]

For the given equation at 800 °C: CO(g) + Ch(g) > COCh(g), the following data were collecica Experiment (COL(M) 0.96 1.92 0.96 (CH] (M) 1.60 1.60 3.20 Rate of appearance COCh (M/s) 0.121 0.242 0.484 Determine the Rate Law for the reaction From your Rate Law determined in question #1 above, determine the value of the rate constant WITH THE APPROPRIATE UNITS. ONLY If you could not answer #1 above, use this "mock" data to solve for k: Rate = K[ARB]?, with [A] = 1.00 M and B]o = 1.50 M, with a rate of 2.50 x 10-2 M/s.

A chemistry graduate student is studying the rate of this reaction: She fills a reaction vessel with and measures its concentration as the reaction proceeds: time (seconds) Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant . Round your answer to significant digits. Also be sure your answer has the correct unit symbol.

The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?

What is the rate constant without units?

Rate laws are determined experimentally by varying the concentrations of the reactants and observing the effect on the initial rate. Concentration and rate data are provided in the table below for the reaction shown. 2NO(g) + Cl2(g) -> 2NOCl(g) Experiment [NO](M) [Cl2] (M) Initial Rate (M/s)        1     0.20       0.10    0.63        2     0.20       0.30    5.70        3     0.80       0.10    2.58        4     0.40       0.20       ? Predict the rate for experiment 4, given the other concentration/rate data provided.  _____M/s

The data below were collected for the following reaction: CH3CI (g) + 3 Cl2 (g) → CCI4 (g) + 3 HCI (g) [CH3CI](M) [Cl2](M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.029 0.100 0.100 0.041 0.200 0.200 0.115 What is the order of the reaction with respect to CH3CI? What is the order of the reaction with respect to Cl2? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Write an expression for the reaction rate law.