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ID: 542230 • Letter: N
Question
ngagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator assignment-takeätakeAssignment SessionLoca This question has multiple parts. Work all the parts to get the most points. pt The reactiorn pt pt 1 pt 1 pt 1 pt 2N0(g) +2H2(g) N2(g) + 2 H20(g) was studied at 904 °C, and the data in the table were collected. Reaction Concentration (mol/L) Rate of Appearance of N NO 0.418 0.209 0.209 0.105 0.175 0.175 0.350 0.700 (moVL s) .193 0.0483 0.0966 0.0488 1 pt Determine the onder of the teaction for each reactant. reaction order in [NO- reaction order in Ha] b Write the rate equation for the reaction. (Use k for the rate constant.) Rate kINO TH21 MacBook Air : 0 FS -F6Explanation / Answer
In order to calculate the rate law expression for a A+B reaction, we need to apply Initial Rates Method.
Note that the generic formula goes as follows:
r = k [A]^a [B]^b
Note that if we got at least 3 sets of point, in which we have A and B constant, then we could use:
r1 / r2 = (k1 [A]1^a [B]1^b) / (k2 [A]2^a [B]2^b)
If we assume K1 and K2 are constant, then K1= K2 cancel each other
r1 / r2 = ([A]1^a [B]1^b) / ( [A]2^a [B]2^b)
Then, order according to [A] and [B]
r1 / r2 = ([A]1/[A2])^a * ([B]1/[B]2)^b
If we get two points in which A1 = A2, then we could get B, and vise versa for A...
From the data shown in YOUR table
choose point 1 and 2 so H2 cancel
0.193/0.0483 = (0.418/0.209)^no
no = ln(0.193/0.0483) / ln(0.418/0.209) = 1.998 = 2
2nd order with respect to NO
now, choose point 2 and 3 so NO cancels
(0.0483/0.0966) = (0.209/0.209) * (0.175/0.35)^h2
ln(0.5 ) / ln(0.5) = h2
h2 = 1
1st order with respect to H2
then
b)
Rate order:
Rate = k*[NO]^2[H2]
c)
get k choosing any point
rate = k*[NO2]^2[H2]
0.0488 = k*(0.105^2)(0.70)
k = 0.0488 /((0.105^2)(0.70))
k = 6.3232
d)
get rate for:
Rate = k * [NO]^2 *[H2]
Rate = 6.3232*(0.34^2)(0.27)
Rate = 0.19735 M/s
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