The Maxwell-Boltzmann distribution plot below is for the same substance with t +c0b1x)9rtmh pz kkk7he same c 1cmx 0k+hp 7rzk9b)tkoncentration at different temperatures. Which statement is correct about the total number of molecules for each temperature?

  What cannot be used to determine the rate expression for a reaction?

  Which of the following factors increases the rate of the reaction below?
$MG_ (s)$+$2HNO_3(aq)$→$Mg(NO_3)_2(aq)$+$H_2(g)$

  

  Which of the following determines the frequency factor, A, in the Arrhenius equation?

  Magnesium and excess hydrochloric acid react together to produce hydrogen gas. This experiment was conducted two times with different hydrochloric acid concentrations but with the same magnesium mass.
In both cases, the volume of hydrogen gas produced was measured at different times, and graphs 1 and 2 were plotted accordingly, as shown below. Choose the letter representing the stage where the rate of reaction is the fastest.

  Which change does not affect the position of equilibrium?

  Which of the following graphs would accurately represent a reaction with a rate expression rate = $\kappa$$[A]^2$

  

  $C_2H_6O$(l)+$3O_2(g)$→$2CO_2(g)$+$3H_2O$(g)

  If the unit of rate constant,$\kappa$, for a reaction is $mol^{-2}$ $dm^6$ $s^{-1}$, what is the overall order of the reaction?

  For a reaction that is first order with respect to $[M]$, the rate of the reaction is $0.5s^{-1}$ when the concentration of $[M]$is$1.0 mol dm^{-3}$. What would be the most likely rate when the concentration of $[M]$for the same reaction is$1.0 mol dm^{-3}$?

  If the rate expression for a reaction 2 X+Y→Zis rate = $\kappa$$[X]^2$, which of the following is most likely ture about"Rate determining step"or"Molecularity"?

  

  The rate equation for the thermal decomposition of hydrogen peroxide is $Rate$=$\kappa$$[H_2O-2]$.
Which of the following graphs shows the relationship between the rate and the temperature of this reaction?

  Sodium hydroxide and the ester ethyl acetate react with the rate equation:
$rate$=$\kappa$$[Ester][NaOH]$.
What are the units of the frequency factor, $A$, for this reaction? $\kappa$=$Ae^{-Ea/RT}$

$Na_2CO_3(s)$+$2HNO_3(aq)$$H_2O(l)$+$CO_2(g)$+$2NaNO_3(aq)$
1.State a method to measure the rate of reaction other than measuring the volume of gas collected.

2.1.Sketch a graph to show the volume of gas produced over time.
2.Explain the shape of your graph using the collision theory.

3.On the same graph as in part(bi), sketch another line to show the volume of gas collected over time at a concentration of 0.05 mol $dm^{-3}$of nitric acid and label it as X.

4.Suggest and describe a factor other than the concentration that can affect the rate of the above reaction.

The reactions of pollutants with ozone in xx 80bz td 3gog7pm7: ls .ei-ovfks1j4buq+)the atmosphere is studied to investigate the effects on the hu-e8j:)g1fz7 7+kvols ms .qdot 0xp4bg 3ibx ole in the ozone layer. One substance that reacts with ozone is nitrogen monoxide.
The reaction is: $O_3(g)$+$NO(g)$→$O_2(g)$+$NO_2(g)$

1.Use the data to determine the order of the reaction for each reactant, and the overall order of the reaction.

2.Give the rate expression for this reaction.Calculate$\kappa$for this reaction using a set of data from the table and determine its correct units.

3.What does the value of $\kappa$ suggest about this reaction in the atmosphere?

4.Suggest with a reason, a possible mechanism consistent with your rate expression.

​​In an experiment, the following data were collected at $25^{\circ}C$:

Trial	Concentration of $O_3$($mol$ $dm^{-3}$)	Concentration of $NO$($mol$ $dm^{-3}$)	Rate of reaction ($mol$ $dm^{-3}s^{-1}$)
1	$3.00\times 10^{-3}$	$1.00\times 10^{-3}$	$6.60\times 10$
2	$6.00\times 10^{-3}$	$1.00\times 10^{-3}$	$1.32\times 10^{2}$
3	$9.00\times 10^{-3}$	$1.00\times 10^{-3}$	$1.98\times 10^{2}$
4	$9.00\times 10^{-3}$	$2.00\times 10^{-3}$	$3.96\times 10^{2}$
5	$9.00\times 10^{-3}$	$3.00\times 10^{-3}$	$5.94\times 10^{2}$

  Two experiments were conducted, and the rates of reac.nd :glb8f d,uwd;/r- z6tcuctions were measured. In the first experimenccr -fbndtu/.;,gdwl u6d:z8 t, 50$cm^3$of 0.010$mol$ $dm^{-3}$of sulfuric acid was added to 0.200$g$of zinc metal at $25^{\circ}C$. In the second experiment, 50 $cm^3$of 0.010 $mol$ $dm^{-3}$of sulfuric acid was added to 0.200$g$$25^{\circ}C$, followed immediately by 100$cm^3$of distilled water. What happened to reaction rate in the second experiment, and why?

The equation below shows the reaction between concentrated sulfuric acid and magnesium at$25^{\circ}C$ .
$Mg(s)$+$H_2SO_4(aq)$→$MgSO_4(aq)$+$H_2(g)$
1.List 2 characteristics that reactant molecules should have for a reaction to occur.
2.The experiment is repeated at $36^{\circ}C$. Sketch the Maxwell-Boltzmann curve for the reactions at $25^{\circ}C$ and $35^{\circ}C$.
3.Using kinetic particle theory, explain how increasing the temperature will increase the rate of reaction.

Sulfuric acid is made through the Contact Px/nj o8q: y5r:c: ntobrocess. One of the steps in the Contact Process is shown below and it usnt:/: 8:y5j qnxcbro oes vanadium(V) oxide,$V_2O_5$as a catalyst.$2SO_2$+$O_2(g)$⇌$2SO_3(g)$
$\Delta$H = -196 kJ $mol^{-1}$.
1.Define activation energy

  What set of descriptions is correct about the following energy level diagram?

  In the Arrhenius plot shown below, what is the correct labeling of the x and y axes, respectively?

• State the complete balanced equation for the reaction between sulphuric acid and copper (II) oxide.
• State the complete balanced equation for the reaction between ethanoic acid and potassium carbonate.
• Outline two ways to monitor the rate of reaction for reaction (b) above.
  

$2H_2O_2(aq)$→$2H_2O(l)$+$O_2(g)$
1.Suggest how the rate of the reaction could be measured.
2.The proposed mechanism for the reaction involves two steps.
Step1:
$H_2O_2(aq)$+$I^{-}(aq)$→$H_2O(l)$+$IO^{-}(aq)$

Step 2:
$H_2O_2(aq)$+$IO^{-}(aq)$→$H_2O(l)$+$I^{-}(aq)$+$O_2(g)$
The energy level diagram for this mechanism is shown.

1.Explaining your reasoning, use the energy level diagram to deduce the rate-determining step (RDS).
2.Estimate the activation energy for the reaction, $kJ$ $mol^{-1}$.
$E_a$:_______________$kJ$$mol^{-1}$
3.The reaction rate is measured at different reactant concentrations. Explain how this experiment could be used to prove or disprove the proposed reaction mechanism.
3.The reaction can also be catalyzed by the enzyme catalase. The activation energy for this reaction, $E_a$, is 21.3 $kJ$$mol^{-1}$and the frequency factor, A, is$41\times 10^{10}$$mol^{-1}dm^{3}s^{-1}$.Calculate the value of the rate constant at $20^{\circ}C$, in units of $mol^{-1}dm^{3}s^{-1}$. Use sections 1 and 2 of the data booklet.
$\kappa$=_____________$mol^{-1}dm^{3}s^{-1}$

  Which graph below represents a second-order reaction?

  The rate law for the reaction$2NO(g)$+$O_2(g)$→$2NO_2(g)$, is determined to be second-order with respect to $NO$ and first order with respect to$O_2$​.
Which of the mixtures below would create the fastest initial rate?

$Time(s)$	$[NaOH](M)$
0	0.100
50	0.082
100	0.067
200	0.045
400	0.020

2.Calculate the initial rate of reaction using the graph.
3.Calculate the rate of reaction at the$300^{th}$ second. Compare this value with the value calculated in part (b). Comment on the rate of reaction.

A student used an online simulation to coll+,zmwt-kc( 7*qk gv8rvmdvmi 0m a, 8xect the following data on kinetics of a clock reaction, timing the reaction until a dark blue colour appeared suddenly. They kept all other factors constant, including the concentrations of the otvm(,r mvi z+w0ga88- ,mkmq dxtvc*k7her reactants$([H_2SO_4]=0.10mol dm^{-3},[Na_2S_2O_3]=0.030mol dm^{-3},[starh]=0.001mol dm^{-3})$

Trial	$[H_2O_2]$, $mol$$dm^{-3}$	$[KI]$, $mol$$dm^{-3}$	$Reaction Time (s)$	$Rate of Reaction$
1	0.045	0.100	3.59
2	0.045	0.050	7.20
3	0.045	0.025	14.00
4	0.0225	0.100	7.05

1.Fill in the table with the respective rate of reaction for each trial.
2.Sketch the graph for rate vs [KI] and state the order of reaction with respect to KI.
3.Determine the order of reaction with respect to hydrogen peroxide using the data table.
4.Suggest two further experiments that could be done to determine the rate expression.
5.Suggest an advantage or a disadvantage about using a simulation to collect data.

  A reaction involvingy+pz4a9 ,-c(8:lq47 eh vtbyan ogrve $X$ and $Y$ is measured and the following data is found:

Trial	$[X]$$(mol dm^{-3})$	$[Y]$$(mol dm^{-3})$	$Rate$$(s^{-1})$
1	0.10	0.50	0.20
2	0.20	0.50	0.40
3	0.20	0.25	0.40

What possible mechanism is consistent with the data?

A student adds excess zinc pellets txw gnd63 civrzmxvm02m 435:x o0.100$mol dm^{-3}$$HNO_3$in a beaker. The student tracks the reaction's progress by monitoring the mixture's pH in the beaker over time. The data is collected and graphed. The results are shown below:
$Zn(s)$+$2HNO_3(aq)$→$Zn(NO_3)_2(aq)$+$H_2(g)$

2.1.The change of pH over time is related to the disappearance of the$HNO_3$.If the rate of disappearance of$HNO_3$ is determined to be$5.53\times 10^{-3}$$mol dm^{-3}s^{-1}$,what is the rate of appearance of $Zn^2$+$ions$?
2.Propose an observation of a different substance in this chemical reaction that could be used to determine the rate of the reaction. Describe both the substance observed and the measurement taken.
3.1.On the energy profile diagram below, label lines$A$and$B$. Then, state if the reaction is endothermic or exothermic and justify your response.

2.If the energy profile diagram above represents the reaction with a catalyst, sketch how the curve would change if the reaction proceeded without a catalyst.
​

​

The enzyme carbonic anhydrase catalyzes the reaction of dissolved336b pcc a9bodrnsfi6l p69n, carbon dioxide with water 6, nrpsa9bn fip96lb6 o3c d3cto form carbonic acid.
$CO_2(aq)$+$H_2O(l)$→$H_2CO_3(aq)$
1.State one reason that the use of an enzyme causes the rate constant to increase.
2.The rate constant was measured over a range of temperatures. Three of the measurements are shown in the table.

Temperature/$^{\circ}C$	$\kappa$/$s^{-1}$
20	$6.0\times 10^{5}$
40	$1.5\times 10^{6}$
80	$1.2\times 10^{5}$

Explain why the rate constant changes as the temperature increases.
3.Consider the plot of $ln$($\kappa$) against $\frac{1}{T}$ for this reaction.

Use the graph and sections 1 and 2 of the data booklet to calculate the activation energy,$E_a$,in $kJ$ $mol^{-1}$

  Experimental data was collected for the following reactio)0/siv4xsny k n.
$NO(g)$+$NO_2(g)$+$O_2(g)$→$N_2O_5(g)$

$Experiment$	$[NO]$	$[NO_2]$	$[O_2]$	$Rate$$(mol dm^{-3}s^{-1})$
1	0.050	0.050	0.050	$4.8\times 10^{-3}$
2	0.10	0.050	0.050	$9.6\times 10^{-3}$
3	0.10	0.15	0.10	$2.88\times 10^{-2}$
4	0.050	0.050	0.10	$4.8\times 10^{-3}$

Using this data, determine the rate law.

  Reaction 1 has a larger frec,rcpa 5/5-+u xits8epooy;p:-ntan quency factor, $A$, than reaction 2 but a smaller activation energy,$E_a$Which of the following graphs is correct?$ln$$\kappa$=$\frac{-E_a}{RT}$+$lnA$