What is the rate law for this reaction? (b) If the rate constant for this reaction at a certain temperature is 9.70e+04, what is the reaction rate when [NO(g)] = 0.0560 M and [H2(g)] = 0.119 M? Rate =  M/s. (c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.112 M while the concentration of H2(g) is 0.119 M?

Be sure to answer all parts. Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first- order process to methane and ketene (CH,=C=0). At 600°C, the rate constant is 8.7 x 103 s1. (a) What is the half-life of the reaction? Give your answer in scientific notation. x 10 (select) A (b) How long does it take for 42% of a sample of acetone to decompose? (c) How long does it take for 82% of a sample of acetone to decompose? Give your answer in scientific notation. x 10 (select) O S

The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?

(a) Suppose the rate of formation of Br2 is 4.0 x 10° M/s in a reaction in water described by the following net ionic equation: 5Br +BrO3¯ + 6H* → 3B12 + 3H20. What are the rates of reaction of each of the reactants and the reaction velocity? 14. (b) List two possible scenarios that may lead to zero-order reactions.

The reaction of nitric oxide with hydrogen at 1280oC is 2NO(g) + 2H2(g) --  N2(g) + 2H2O(g)   From the following data collected at this temperature, determine (a) the rate law, (b) the rate constant, and (c) the rate of the reaction when [NO] = 12.0 x 10-3 M and [H2] = 6.0 x 10-3 M.   Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 5.0 x 10-3 2.0 x 10-3 1.3 x 10-5 2 10.0 x 10-3 2.0 x 10-3 5.0 x 10-5 3 10.0 x 10-3 4.0 x 10-3 10.0 x 10-5

Consider the following proposed mechanismHBr + HBr ⇄ H2Br2(fast, equilibrium)HBr + R ⇄ ES(fast, equilibrium)H2Br2 +ES→P+2HBr(slow) (1a) What is the overall reaction? (1b) Identify all catalysts and intermediates in this reaction mechanism. (1c) What is the rate law derived from this mechanism? (1d) If the experimentally determined rate law is rate = k [HBr]3[R]1 what conclusion can be drawn? (1e) If the experimentally determined rate law is rate = k [HBr]2 what conclusion can be drawn? The equilibrium constant (KC) is 10.0 x 10-10 at

3. (a) The following data were collected for the reaction between hydrogen and nitric oxide at 700 degrees Celsius: (i) Determine the order of the reaction. (ii) Calculate the rate constant. (b) Consider the reaction ( ) 3 ( ) 2 ( ) N2 g  H2 g  NH3 g Suppose that at a particular moment during the reaction molecular hydrogen is reacting at the rate of 0.074 M/s. (i) At what rate is ammonia being formed? (ii) At what rate is molecular nitrogen reacting?

For the decomposition of gaseous dinitrogen pentaoxide,2N₂O₅(g) →4NO₂(g) +O₂(g), the rate constant is k=2.8X10⁻³ s⁻¹at 60°C. The initial concentration of N₂O₅ is1.58 mol/L. (a) What is [N₂O₅] after 5.00 min? (b) What frac-tion of the N₂O₅ has decomposed after 5.00 min?

Consider the following hypothetical reaction: 2P + Q→ 2 R + S. The following mechanism is proposed for this reaction: P + P = T (fast) Q + T → R+ U (slow) U-R + S (fast) Substances T and U are unstable intermediates. What rate law is predicted by this mechanism? (a) Rate = k[P]? (b) Rate = k[P][Q] (c) Rate = k[P]°[QI (d) Rate = k[P][Q? (e) Rate = k[U]

The decomposition of nitrous oxide, N2O, is believed to occur by a two-step mechanism:N2O(g)----->N2(g) + O(g) (slow)N2O(g) + O(g)---->N2(g) + O2(g) (fast)(a) Write the equation for the overall reaction. (b) Write the rate law for the overall reaction.