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Consider the follwing first order reaction:---------4PH3---> P4 + 6H2----------The half-life of the reaction is 35 seconds at 680 degrees Celcius. Calculate the rate constant for the reaction , and the time required for 95% of the PH3 to decompose.---------8.) The rate constant for the second order reaction below is .54 M^-1 * s^-1. How long in seconds would it take for the concentration of NO2 to decrease from .65 M to .18 M? ------------2NO2---->2NO+O2Show all steps with correct answer for 5 star rating. Thank you.

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Bunny GreenfelderLv2
28 Sep 2019
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Using excel, analyze the data graphically to decide if the reaction is zero, first or second order with respect to crystal violet.

1. was the reaction zero, first or second order, with respect to the concetration of crystal violet? Explain

2. Calculate the rate, K, using the slope of the linear regression line for your linear curve (k= --slope for zero and first order and K= slope for second order.) Be sure to include correct units for the rate constant

3. Write the correct rate law expression for the reaction, in terms of crystal violet (Omit OH-)

4. Using the data table, estimate the half-life of the reaction; select two points, one with an absorbance value that is about half of the other absorbance value. The time it takes the absorbance (or concentration) to be halved is known as the half life for the reaction

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