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13 Dec 2019

The reaction:

N2O2(g) ? 2NO(g)

is first order in the concentrationof N2O2.

Derive an expression for the time dependent behavior of theproduct concentration, [NO].

Given that: (i) the volume of the reaction is constant, (ii) theinitial concentration of N2O2 is

1.0 mol/L and no NO is present atthe start of the reaction, and (iii) the rate constant isk =

1.25 x 10?2 s?1, plot on the samegraph the concentrations of N2O2 and NO as a function of time.

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Related questions

Nitrogen monoxide gas reacts with oxygen gas according to the following balanced chemical equation:

2NO(g)+O2(g)=2NO2(g)

Based on the reaction, what statements are true and which are false?

a. If the rate constant, k, for the forward reaction is 2.32 x 10^-2 L^2*mol^-2*s-1, the overall order of this reaction should be 3rd order.

b. The rate of disappearance of O2 (g) should be twice the rate of disappearance of NO(g).

c. At 25degreesC and 1.0 atm, this reaction should be exothermic

d. If the initial rate of the reaction doubles when the concentration of O2(g) is doubled aand the concentration of NO(g) is kept constant, the exponent for the [O2] in the rate law expression should be one.

I need help with parts c and d

The rate of the reaction of nitrogen monoxide with oxygen wasmeasured at 25 degrees C. starting with various initialconcentrations of reactants NO and O2.

2NO(g) + O2(g)---> 2NO2(g)

initial concentrations reaction rate

mol/L mol/l.s

NO(g) O2(g)

Trial #1 .020 .010 .028

Trial #2 .020 .020 .057

Trial #3 .040 .020 .227

A. Calculate the rate constant for the reaction and reactionorders.

B.Write the complete rate equation using the calculated values forthe rate constant and reaction order.

c. Calculate the reaction rate for this reaction at 25 degrees C,when the inital concentration of NO is 0.010 mol/l and that of O2is 0.020 mol/l.

Please show the calculations on how you came to the followinganswers. I have alot allready figured out, but am missing somepeices to complete my answers. Thank you

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