reaction. (Table 1)Fill in the table to determine the order of a reaction given to these data and draw a diagram of those variables. (Table 2) Table 1 Experiment [A] [B] Rate (M/s) 1 0.100 0.100 3.0 x 10 -3 2 0.100 0.200 6.0 x 10 -3 0.200 0.100 6.0 x 10 Table 2 a. [A]vs time b. In [A] vs time c. 1/[A]vs time Time (s) [A] In [A] 1/ [A] 0.320 10 0.251 20 0.208 40 0.154 60 0.122 Section Hint. Whichever gives a straight line, tells you its order. If [A] vs time graph is straight, it is a zeroth order. • If In [A] vs time graph is straight, it is a first order. • If 1/ [Al vs time graph is straight, it is a second order 3.

For the reaction: 4NH3 (g) + 7O2 (g) → 4NO2 (g) + 6H2 (g), if H2 is produced at a rate of 3.5 x 10-3 M/s, O2 is consumed at a rate of... A. -2.5 x 10-2 M/s B. -4.1 x 10-3 M/s C. -2.1 x 10-2 M/s D. -3.0 x 10-3 M/s E. -5.8 x 10-4 M/s

Assignment 1. The reaction 2NO (g) t CL (g) 2NOCI (g) was studied at- 10 C. The following results were obtained where Rate =- A[CI1 At [2NO], (mol / L) (Ch], (mol/L) Initial Rate (mol /L min) 0.18 0.10 0.10 0.10 0.20 0.36 0.20 0.20 145 a) What is the rate law b) What is the value of the rate constant

please include correct units included, correct number of significant digits.

The following data was collected over four different experiments. for this reaction: aA + bB → CC Experiment [A] M [B] M 1 0.200 0.200 2 0.200 0.400 3 0.400 0.200 4 0.300 0.100 The initial rate of the first reaction was 0.650 mol/L min. The second reaction was 2 times that rate, the third reaction was 8 times the rate of the first reaction, and the fourth reaction was 1.7 times the rate of the first reaction. Determine the value for the constant k. Your Answer: 2031.25

Consider the following reaction and information:   A + 2B → 3C rate = k{B}   Time (min.) B (M) A (M)0 0.72 0.5030 0.25 0.2660 0.087 0.18 What is the concentration of B after 27 minutes?

tter What solid was formed: Copper (II) ions (from CuSO4) react with solid Appearance of copper sulfate: Appearance of zinc: Appearance after 10 min: Appearance after 20 min: Balanced reaction: Type of reaction: 0 min Lab 5 pg. 3 Zinc metal Cu²+ (aq) + Zn () About 10-20 mL of copper sulfate solution are added to two beakers. Note the appearance of the solution. Zinc is added to one beaker (the other is reference control). Note the appearance after 10 and 20 minutes in comparison to 0 min. (reference control). 10 min CuSO4 (aq) + 20 min Zn (s) → Ed: January 2032 ZnSO4 (aq) + Cu (s) In general, salts are soluble in water. In some cases, the forces that hold the salt together are too strong for the water molecules to pull apart. These are called insoluble salts. You can tell if you have an insoluble salt by the formation of a precipitate when combining solutions of soluble salts, or a gas is evolved (observed as gas bubbles, or a foam). For the following reactions, the indicated solutions…

Consider a hypothetical chemical reaction: A+B → C+D (In this equation A, B, C and D stand for some unknown chemical formulas.) Here is an energy diagram for the reaction: energy (kJ/mol) 400 300 200 100 0 C + D SCA A + B reaction coordinate Use the energy diagram to answer these questions. What is the heat of reaction? Is the reaction exothermic or endothermic? Can you determine the activation energy? Can you determine the activation energy of the reverse reaction? C+DA+B kJ/mol Exothermic Endothermic Neither Yes, No. it's No. kJ/mol Yes, it's kJ/mol

Which of the following statements is true about reaction rates? A Reaction rates can be predicted from the coefficients of the balanced equation. B Reactants usually disappear faster than the products appear. C Reactants usually disappear slower than the products appear. D Reaction rates can only be determined by experimentation.

Use the following data to answer questions 3, 4, 5, and 6. The initial rates listed in the following table were determined for the reaction: 2 NO + Clzue) - 2 NOCl) Exp [NO], Initial Rate (M/s) 0.13 0.20 1.0 x 102 0.26 0.20 4.0 x 102 0.13 0.10 5.0 x 103 Which,of the following is the correct rate law? Select one: O a. rate = k[NOJ?{Cl,] O b. rate = k[NOJ[Cl] c. rate = k[NO][CI,J? O d. rate = k[NOJICH¥ Using your answer to # 3. What is the initial rate when the intial concentrations of both reactants are 0.12 M? The units will be M/s, but do not include them in your answer. Your answer should have two significant figures. Answer: