IMFs
Kinetics equations
Catalysts
Types of rates
Half-life/Shelf-life
100

IMF found between any type of molecules

What is a London force?

100

The relationship between reaction rate and concentrations

What is a rate law?

100

Catalysts act on a reaction by lowering this energy.

What is activation energy?

100

Rate at time zero of the reaction

What is the initial rate?

100

Time required for the concentration of a reactant to get to half of its initial value.

What is half-life?

200

IMF found between polar molecules

What is a dipole-dipole force?

200

In the equation: Rate=k[A]m [B]n    k is ______  and  m and n are called ___________

What are the rate constant and the orders with respect to A and B?

200

The name of the plot of ln k versus 1/T

What is the Arrhenius plot?

200

Rate over an interval of time

What is an average rate?

200

Define the shelf-life of a drug.

What is the time required for 10% of the drug to decompose?

300

IMFs between molecules of CO2

What are London forces?

300

If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A.

Second

300

This is the name of the original model of the substrate-enzyme binding.

What is the lock-and-key model?

300

Change in concentration of reactant or product per unit time

What is a reaction rate?

300

The rate constant for the decomposition of N2O5 at a particular temperature is 7.8x10-3 s-1. Calculate the half-life of this first order process.

89 s

400

The molecule with the highest boiling point: Methane (CH4), Dichloromethane (CH2Cl2) or Butanol (CH3CH2CH2CH2OH)

What is butanol?
400

The rate law for a reaction is:  Rate = k [A][B]2 

If [B] is doubled, the reaction rate will increase by a factor of _________.

Four

400

The enzyme lysozyme causes the lysis of the bacterial cell walls by catalyzing the hydrolysis of this substrate.

What is a polysaccharide?

400

Rate at a single point in time

What is an instantaneous rate?

400

Rate = k[A]2,  [A]0 = 0.200 M,   k = 0.0214 M–1 sec–1
Calculate the half-life of this second-order reaction.

234 sec

500

The following molecules are NOT miscible with water: propanol (CH3CH2CH2OH), hexane (C6H14), benzene (C6H6), octanol (C8H17OH)

What are hexane, benzene and octanol?

500

N2(g)+O2(g)= 2 NO(g)

The concentration of nitrogen was 0.375 M at 50.0 s and 0.407 M at 65.7 s. Calculate the average rate of the reaction during this time period (units must be incuded in the answer)

1.0 x 10-3 M/s

500

The following pairs of rate constants and temperatures were measured for a reaction:

193 K and 34.0 M-1 s-1

198 K and 62.8 M-1 s-1

203 K and 112.8 M-1 s-1 

208 K and 196.7 M-1 s-1

Calculate the activation energy(in kJ/mol) and the frequency factor.

39.1 kJ/mol and 1.27 x 1012

500

H2(g) + I2(g) → 2HI(g)

The rate of H2 consumption is 0.02 mol/L s. Calculate the rate of HI production (include units)

0.04 mol/L s

500

The initial concentration of reactant A in a first order reaction is 0.64 M and the half-life is 30 s. How many half-lives does it take to get down to 0.04 M of reactant A?

Four

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