1. A chemical reaction is observed to convert Molecule A into Molecule B. The ac
ID: 837107 • Letter: 1
Question
1. A chemical reaction is observed to convert Molecule A into Molecule B. The accompanying graph plots the change in concentration for both molecules against the change in time. Use this graph to determine the stoichiometry of this equation, if it is written as:
A ? xB
a. x = 1/2
b. x = 1
c. x = 2
d. x = 3
2. Using the following data from a study of how the rate of a reaction was affected by the concentration of the reactants:
run # [ClO2], mol/L [OH-], mol/L rate, mol/L s
# 1 0.100 0.200 0.460
# 2 0.200 0.200 1.84
# 3 0.200 0.100 0.920
Calculate the rate constant k (units mol-2 L2 s-1), given the following rate law:
rate = k [ClO2]2[OH-]
3. Nitric oxide reacts with bromine gas at elevated temperatures according to the equation,
2 NO(g) + Br2(g) ? 2 NOBr(g)
The experimental rate law is rate = k[NO][Br2]. In a certain reaction mixture the rate of formation of NOBr(g) was found to be 4.50 x 10-4 mol L-1 s-1. Which unit below is the correct unit for the rate constant in this case?
a. mol L-1 s-1
b. mol2 L-2 s-1
c. s-1
d. mol-2 L2 s-1
e. mol-1 L s-1
Explanation / Answer
1.a.x=1/2
you can easily observe for greater decrease in concentration of reactant there is a smaller increase in the concentration of product. so for every one mole of reactant you should get lesser amount of product in the options only 1/2 is lesser....
2. k = 230
substitute any one of the given values in the rate equation. you should get the same value of k for all data sets as rate constant remains constant at a given temperature.
3.e
units of rate is mol/lit/sec
units of concentration is mol/lit
substitute the units in the equation...after simplification you will get the units of rate constant
comment if you want detailed explanation
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