Rate Expression: In each case write the rate expression for the stated reaction and find the rates of all other species using the given rate. (Make sure reactions are balanced 2. Cr2O7(g) + C2H6O (g) -› CO2(g) + Cr(g) Rate of depletion of CO2 = 1.5 x10-2 M/s

How would each of the following change the rate of the reaction shown here? Drag the appropriate items to their respective bins. decreasing the temperature adding some NO(g) Reaction rate increases 2NO(g) + 2H₂(g) → N2(g) + 2H₂O(g) Submit Request Answer Reaction rate decreases removing some H₂(g) P Pearson adding a catalyst Reset Help Reaction rate remains the same.

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

O KINETICS AND EQUILIBRIUM = 3/5 Using first- and second-order integrated rate laws Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (1.3 M¹-s¯¹) [₂0₁] olo Suppose a vessel contains N₂O5 at a concentration of 1.20M. Calculate the concentration of N₂O5 in the vessel 7.30 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X Explanation Check Chelsea V @ EH

3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640

6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order

Rate Expression: In each case write the rate expression for the stated reaction and find the ratesof all other species using the given rate. (Make sure reactions are balanced)1.C2H2(g) + O2(8)--- › CO2(8) + H2O(g)Rate of formation of O2 = 0.814 M/s

Part A Consider the balanced chemical equation. H2O2(aq) + 3I¯ (aq) + 2H+(aq) → I3 (aq) + 2H20(1) Predict the rate of change in the concentration of H2O2 (A[H2O2]/At). In the first 12.0 s of the reaction, the concentration of I drops from 1.000 M to 0.773 M . Express the rate to three significant figures and include the appropriate units. You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. ? A[H2O2]/At = Value Units

For the simple decomposition reaction: AB(g) A(g) + B(g), the rate = k{AB}? ({ = [) and k = 0.78 1/M•s. How long (in seconds) will it take for the concentration of AB to reach one-third of its initial concentration of 1.07? Enter to 2 decimal places.

Given the following reaction, 2 NH3(g) → N2(g) + 3 H2(g) Which of the following relates the appearance of H2 to the disappearance of NH3? A) rate of appearance H2 = 3/2 ( △NH3 / △t ) B) rate of appearance H2 = 1/2 ( △NH3 / △t ) C) rate of appearance H2 = - 2/3 ( △NH3 / △t ) D) rate of appearance H2 = - 3/2 ( △NH3 / △t ) E) rate of appearance H2 = - 1/2 ( △NH3 / △t )