The question is based on your experimentally determined rate law, how would doubling the concentration of crystal violet affect the reaction rate? The reaction rate was second order and crystal violet we used was 1.5×10^–5 M crystal violet solution

- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

The hydrolysis of a substance is specifically catalyzed by hydrogen ions, and the rate constant is given by the equation: k/dm^3 mol^-1 s^-1 = 4.7 x 10^-2([H+]/mol din^-3) When the substance was dissolved in a 10^-3 M solution of an acid, HA, the rate constant was 3.2 x 10^-5- dm^3 mol^-1 s^-1. What is the dissociation Constant of HA?

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=67.0 kJ/mol. If the rate constant of this -1 −1 reaction is 3.9 M •S at 99.0 °C, what will the rate constant be at 178.0 °C? Round your answer to 2 significant digits. - 1 -1 ☐ k = M • S ? x10 X Ś

(a) Select all of the correct statements about reaction rates from the choices below. 1.The lower the rate of a reaction the longer it takes to reach completion.2 The rate of a reaction is independent of temperature.3 Slow reactions can be speeded up by raising the temperature.4. Reaction rates increase with increasing temperature.5. Solid catalysts do not affect reaction rates.6. Reactions involving very unstable combinations of chemicals have large rate constants.7. A balanced chemical reaction is necessary to relate

3. Suppose we found that the reaction of Red #3 with bleach is first-order in hypochlorite. The observed rate constant (kobs) was determined to be 4.00 x 10-3 s-1. If the concentration of hypochlorite was held fixed at 0.134 M, find the specific rate constant (k).

Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, fınd the rate law. 0–H [RCOOH], M [R'OH], M (HA], M Initial Rate, Ml·min' || R-c-o–H 0.35 0.35 0.50 4.60 0.50 + HA - R-Ć+ k2 0.62 0.35 8.14 A- 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A + R -0–H R—С—0—Н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R'-o+ A- Rate = k[R'OH] Group 2 H Rate = k[RCOOH] 0–H k5 R—С—0—н R-C-0–R' + H2O + HA R-o+ A- Group 3 H. Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 Step 1

Please solve the entire question - I already know that the reaction order in NO is 2 and the reaction order in O2 is 1 - making the overall reaction order 3.

Another common component of reaction mechanism is a catalyst. These are compounds that change the reaction mechanism and provide a pathway with a lower activation energy, and correspondingly faster reaction rate. They are a reactant in an early step in the mechanism and a product in a later step. They do not appear in the overall reaction but do appear in the rate law. 3. A reaction occurs by the following mechanism; Step 1 Ce4+ + Mn²+ →→ Ce³+ + Mn³+ Step 2 Ce4+ + Mn³+ → Ce³+ + Mn²+ Step 3 Tit+ Mn+→ Ti³+ + Mn²+ a. Write the overall reaction. b. Identify each of the components as a reactant, product, intermediate, or catalyst; Mn²+ Mn³+ Ce4+ Ce ³+ Mn4+ Tit Ti³+ C. Assuming that the catalyst is involved in the rate determining step, what is the rate law for this reaction? 4. Under certain conditions, the reaction: 2 NO + Cl₂ → 2 NOCI is found to be second order in NO and first order Cl₂. Given the following mechanism; Step 1 NO + Cl2 → NOCI₂ Step 2 NOCI₂ + NO 2 NOCI a. What are the…