Rate Law

Rate = k[M][N]² The rate of a certain chemical reaction between substances M and N obeys the rate law above. The reaction is first studied with [M] and [N] each 1x10^-3M. If a new experiment is conducted with [M] and [N] each 2x10^-3M, the reaction rate will increase by a factor of

• 2

• 4

• 6

• 8

• 16

Tags

NGSS.HS-PS1-5

An experiment was conducted to determine the rate law for the reaction A_2(g) + B_(g) --> A₂B(g). The table above shows the data collected. Based on the data in the table, which statement is correct?

• Since the rate law can be expressed as rate=k[A₂]², tripling the concentration of A₂ will cause a 9-fold increase in the rate of the reaction

• Since the rate law can be expressed as rate=k[A₂][B], doubling the concentrations of A₂ and B will quadruple the rate of the reaction.

• Since the rate law can be expressed as rate=k[A₂]²[B], tripling the concentration of A₂ while keeping the concentration of B constant will triple the rate of the reaction

• Since the rate law can be expressed as rate=k[A₂][B]², doubling the concentration of B while keeping the concentration of A₂ constant will double the rate of the reaction

Tags

NGSS.HS-PS1-5

The initial rates of the reaction represented by the equation shown above were measured for different initial concentrations of NO(g) and Cl₂(g). Based on the data given in the table above, which of the following is the rate law expressed for the reaction, and why?

• Rate = k[NO]², because the initail rate quadrupled when [NO] was doubled but remained constant when [Cl₂] was doubled.

• Rate = k[NO][Cl₂], because the initial rate doubled when either [NO] or [Cl₂] was doubled

• Rate = k[NO][Cl₂]², because the initial rate doubled when [NO] was doubled and quadrupled when [Cl₂] was doubled

• Rate = k[NO]²[Cl₂], because the initial rate quadrupled when [NO] was doubled and doubled when [Cl₂] was doubled

Tags

NGSS.HS-PS1-5

The rate law for the reaction of nitrogen dioxide and chlorine is found to be rate=k[NO₂]²[Cl₂]. By what factor does the rate of the reaction change when the concentrations of both NO₂ and Cl₂ are doubled?

• 2

• 3

• 4

• 6

• 8

Tags

NGSS.HS-PS1-5

In an aqueous solution, the reaction represented by the balanced equation shown above has the experimentally determined rate law: rate=[S₂O₈^2-][I^-]. If the concentration of [S₂O₈^2-] is doubled while keeping [I^-] constant, which of the following experimental results is predicted based on the rate law, and why?

• The rate of reaction will remain the same, because k will decrease by half

• The rate of reaction will double, because the rate is directly proportional to [S₂O₈^2-]

• The rate of reaction will increase by a factor of four, because two moles of SO₄^2- are produced for each mole of S₂O₈^2- consumed

• The rate of reaction will increase by a factor of four, because the reaction is second order overall

Tags

NGSS.HS-PS1-5