Rate laws can be entered as strings in the answer box. For example, for aA(aq) + bB(aq) → CC(aq) with the rate being second order in A and first order in B you enter k*[A]^2*[B] for aA(g) + bB(g) cC(g) with the rate being second order in A and first order in B using pressures you enter k*P_{A}^2*P_{B}. and The reaction 2NO(g) + O2(g) → 2NO2(g) is second order in NO and first order in 02. Write the rate law for the reaction in terms of pressures PNO and Po2 Let us agree not to use subscripts on subscripts. So, to enter the pressure of 02 use P_{02} and not P_{O_2}. r = Units can be entered using mol/(L s) note the parenthesis and the space between L and s. Enter the units of r when the pressure is measured in bar and time in min. (use the backslash / but be sure to use () when more than one unit is is the denominator) Units of r = Enter the units of r when the amount is measured in mol L-1 and time in min (use the backslash / but be sure to use () when more than one unit is is the denominator and a space or * to mean the product, for example: L/(mol s) or L/(mol*s) or L/(s mol) or L/(s*mol) ) Units of r =

- 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.

5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T

Be sure to answer all parts. The rate law for 2 NO(g) + O2(g)→ 2 NO2(g) is rate = k[NO]°[O2l. %3D The following mechanisms have been proposed: I. 2 NO(g) + O2(g)→ 2 NO2(g) II. 2 NO(g) = N½O2(g) [fast] N,O2(g) + O2(g) → 2 NO,(g) [slow] III. 2 NO(g) = N,(g) + O2(g) [fast] N2(g) + 2 O2(g) → 2 NO2(g) [slow] (a) Which of these mechanisms is consistent with the rate law? Check all that apply. I. II. III. None of the above (b) Which of these mechanisms is most reasonable? I. II. III.

Questions 2A 2B and 2C please

Give answer to all parts

A value of k is found from the rate equation Rate = k[A]m[B]n. If m=1 and n=4 and -1 the unit for the initial rate is M/h. The unit of k is found to be MX h-¹ (M to the power of x h to the power of minus 1). What is the value of x?

The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 73 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.1 ug/mL. What will the concentration be 365 minutes later? Round your answer to 2 significant digits. ug x10 mL ?

6. To observe the effect of temperature on reaction rate, the reaction between MnO, ag) and C204(ag) in acidic media is performed according to the given redox reaction: 2 MnO4 (aq) + 16 H*(aq) + 5 C204²(aq) → 10 CO2(g) + 2 Mn²"(aq) + 8 H2O(1) At various temperatures, the rate constants were determined experimentally as follows: k (M s') 5.03x105 T (°C) 20 35 3.68×104 60 6.71×103 90 0.119 (a) Determine Ea for this reaction by a graphical method (see the graph given below). (b) Determine E. using Arrhenius equation using tabulated data. (c) Calculate the value of the rate constant, k at 100°C. -2 -4 兰 -6 -8 -10 -12 0.0025 0.0027 0.0029 0.0031 0.0033 0,0035 1/T (K)