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27 Sep 2018

Ni(CO)4 (s) = 4CO (g) + Ni (s)

At 66.0C, the rate constant for this reaction is 1.873 s^-1

a) what is the reaction order for this process

b) Write the rate law expression for this reaction based on youranswer to part a.

c) Determine the time required for half of the Ni(CO)4 todecompose

d) determine the time required for 90% of the Ni(CO)4 todecompose

please show as much work as possible and provide explanation ifpossible, so that i am able to do it on my own in the future. ThankYou.

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27 Sep 2018

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Please help im so confused on this part of the problem!! here isthe equation:

Ni(s)+ 4CO(g) <---->Ni(CO)4 (g)

d)The first step of the Mond process involves equilibratingimpure nickel with CO(g) and Ni(CO)4(g) at about 50 degrees C. Thepurpose of this step is to convert as much nickel as possible intothe gas phase. Calculate the equilibrium constant for the precedingreaction at 50 degrees C.

e)in the second step of the Mond process, the gaseous Ni(CO)4 isisolated and heated to 227 degrees C. the equilibrium constant forthe above reaction at 227 degrees C is 1.21 x 10^ - 4 . why istemperature increased for the second step of the Mond process?

Could you please answer these questions

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The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

Show transcribed image text The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

A starch solution is stirred in a 1500 mL cooking pot. The crystalline starch (CS) is converted into gel-like starch (GS) by heat and time following a reaction as CS â GS. An inlet stream of crystalline starch enters at 3.6 mL/s with a concentration of 4.8 mol CS/mL and is introduced into the tank at time t = 0. At this time, the pot contains 475 mL of solution with a concentration of CCS = 1.9 mol/mL. The gelled starch solution is removed from the pot starting at t = 0 at the same volumetric flow rate as the inlet stream. The reaction rate law is: rCS = -0.054 CCS [mol CS mL-1 s-1].

1. Find an expression for the concentration of crystalline starch as a function of time. Format your expression as C_CS = f(t) and include units for each constant.

2. Determine the concentration in the pot after 30 s.

3. Calculate the concentration of crystallized starch at steady state.

4. Find the time when the concentration reaches 90% of the steady state concentration.

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