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Section 3: Reaction Rate Laws

Reaction Rate Laws


1.	The rate law for the reaction between nitrogen monoxide and hydrogen is Rate = k[NO₂]2[H₂]. What happens to the rate if the concentration of nitrogen doubles? Need a Hint?
		A)	The rate doubles.
		B)	The rate triples.
		C)	The rate quadruples.
		D)	The rate is reduced by half.


2.	In the rate-law expression, Rate = k[A], what does the symbol k represent? Need a Hint?
		A)	instantaneous rate
		B)	concentration
		C)	specific rate constant
		D)	reaction order


3.	The exponents in a rate-law expression define the __________, which describes how the rate is affected by the concentration of the reactant. Need a Hint?
		A)	instantaneous rate
		B)	concentration
		C)	specific rate constant
		D)	reaction order


4.	What is the reaction order for each reactant in the following rate-law expression? Rate = k[A][B]²[C]³ Need a Hint?
		A)	first order for A, first order for B, first order for C
		B)	first order for A, second order for B, first order for C
		C)	first order for A, second order for B, third order for C
		D)	first order for A, second order for B, second order for C


5.	What is the overall reaction order for the following rate-law expression? Rate = k[A][B]²[C]³ Need a Hint?
		A)	4
		B)	5
		C)	6
		D)	7


6.	What is the most common experimental method for evaluating a reaction order called? Need a Hint?
		A)	method of final rates
		B)	method of instantaneous rates
		C)	method of initial rates
		D)	method of experimental rates


7.	How are the rate law and the order for a complex reaction determined? Need a Hint?
		A)	by calculation
		B)	by experimentation
		C)	by trial and error
		D)	by estimation