Which of the following equations would you use to solve for k, the true rate constant, using the experimental data? - O In[Bleach] = -kt + In[Bleach]o Ok = k[Bleach]P - 1 = kt + 1 [Bleach], [Bleach]o - O [Bleach] = -kt + [Bleach]0

For each of the following, suggest appropriate rate units Driving from one place to another Drying dishes by hand The heating wings of a mosquito Eyes blinking

Explain how a species might be part of a rate law but not part of a balanced chemical reaction.

The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- → H₂(g) + ½ I₂(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.64×10-³ M-¹ s-¹ and a y-intercept of 0.418 M-¹. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M-¹ S-¹.

In chemical kinetics there is an equation similar to the Clausius-Clapeyronequation: ln(k)=(Ea/R)(1/T) + ln(A). Ea is very difficult to measure. Instead, you measure temperature (T) and the rate constant (k) and use graphical analysis to calculate Ea. Comparing this new equation a straight line (y=mx+b):a. Which variable in this equation would you plot on the y-axis?b. Which variable in this equation would you plot on the x-axis?c. What does the slope, m, of the straight line represent in this equation?d. Show how you would calculate Ea using the slope of the line (inequation form...you do not need to calculate an actual value).

The rate equation for the hydrolysis of sucrose to fructose and glucose C12H22O11(aq) + H2O(ℓ) → 2 C6H12O6(aq) is -Δ [sucrose]/Δt = k[C12H22O11]. After 27 minutes at 27 °C, the sucrose concentration decreased from 0.0146 M to 0.0132M. Find the rate constant, k.

For an autocatalytic reaction :  A  → B + ……        where   -d[A]/dt = k[A][B]. Assume that [B]o ≠0             Letting    [A] = Ao – x     and [B] = Bo +x                       -d[A]/dt = -d[Ao -x]/dt = dx/dt                        and dx/dt  = k[Ao- x] [Bo + x] Show that  [B] =  {[A]o   +  [B]o } / [Ao/Bo] exp{- [A]o  + [B]0 }kt + 1

For the gas phase decomposition of t-butyl bromide, (CH3)3 CBr → (CH3)2C=CH₂+ HBr the rate constant in 8¹ has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.04 x 104 K and a y-intercept of 30.6. The value of the rate constant for the gas phase decomposition of t-butyl bromide at 546 K is 170 (Enter your answer to one significant figure.) s-1.

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!