Be sure to answer all parts. For the reaction 4A(g) + 3B(g) →→→ 2C(g) The following data were obtained at constant temperature: Experiment 1 2 3 4 Initial [A] Initial [B] (mol/L) (mol/L) 0.100 0.100 0.300 0.100 0.100 0.200 0.300 0.200 Reaction order for A: Initial Rate(mol/L*min) Reaction order for B: 5 45 10 Determine the reaction order with respect to each reactant. 90

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.450 0.50 0.300 1.00 0.225 1.50 0.180 2.00 0.150 2.50 0.130 3.00 0.115 3.50 0.100 4.00 0.090

10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.

Consider the following reaction performed at K and the given concentration and rate data: A products Experiment [A] Rate of reaction (M) (M/s) 1 0.78 0.0026988 2 1.56 0.0053976 3 3.12 0.0107952 First determine the rate law and rate constant. Based on this information; if you set up a new experiment where the [A]. (initial concentration of A) was 1.33 M, what would the concentration of A be after 144 s? [A](M) = number (rtol=0.01, atol=1e-08) ?

[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.

don't reject no honour code in this question