Consider the following reaction: 3A+2B-->2C+4D If the rate of change of [A] at a

Question

Consider the following reaction: 3A+2B-->2C+4D If the rate of change of [A] at a given point in time is -1.0 M/s, what is the rate of change of [C] at that same point in time? A--(-1ms), B--(+.67 ms), C--(+1 ms), D--(+1.3 ms), or E--(-1.3 ms)???? -----Next question-------Consider the rate law: rate = k [A]2 What will the units of k be for this rate law? A---(1/s), B---(m/s), C---(1/m^2 *s), D---(1/m*s), E---(s/m)??????-----Next question---Identify the intermediate(s) in the following reaction mechanism:

1) NO+Cl2=NOCl2, 2) NOCl2+NO--->2NOCl? A---(NO), B--(Cl2), C---(NOCl2), D---(NOCl), E---(NO and NOCl2)????-----Next question-----The rate law for the reaction: A + 2 B ? Cis: rate = k[A][B] If k = 0.318/M*s , and initial concentrations of reactants are: [A] = 0.50 M and [B] = 0.35 M, what will be the initial rate of this reaction? A---(0.019 M/s), B--(.056 m/s), C---(.32 m/s), D---(.35 m/s), E---(.85 m/s)????-------Next question--------The following reaction:CH3CHO ? CH4+ COIs first order with k = 0.0693 / min If the initial CH3CHO concentration is 0.435 M, what will be the CH3CHO concentration after 37 minutes? A---(.289 M), B---(.568 M), C---(.218 M), D---(.118 M), E---(.0335 M)

Explanation / Answer

for given reaction -1/3[A] =1/2[C] => for [C] it is 0.67.....unit of k = [unit of rate]/[unit of concentration]^2 =M^-1*sec^-1 = 1/ms

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