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Relative rates of reaction

The rate of a reaction may be expressed in terms of the change in the amount of any reactant or product, and may be simply derived from the stoichiometry of the reaction. Consider the reaction represented by the following equation:

2NH 3 ( g ) N 2 ( g ) + 3H 2 ( g )

The stoichiometric factors derived from this equation may be used to relate reaction rates in the same manner that they are used to related reactant and product amounts. The relation between the reaction rates expressed in terms of nitrogen production and ammonia consumption, for example, is:

Δmol NH 3 Δ t × 1 mol N 2 2 mol NH 3 = Δmol N 2 Δ t

We can express this more simply without showing the stoichiometric factor’s units:

1 2 Δmol NH 3 Δ t = Δmol N 2 Δ t

Note that a negative sign has been added to account for the opposite signs of the two amount changes (the reactant amount is decreasing while the product amount is increasing). If the reactants and products are present in the same solution, the molar amounts may be replaced by concentrations:

1 2 Δ [ NH 3 ] Δ t = Δ [ N 2 ] Δ t

Similarly, the rate of formation of H 2 is three times the rate of formation of N 2 because three moles of H 2 form during the time required for the formation of one mole of N 2 :

1 3 Δ [ H 2 ] Δ t = Δ [ N 2 ] Δ t

[link] illustrates the change in concentrations over time for the decomposition of ammonia into nitrogen and hydrogen at 1100 °C. We can see from the slopes of the tangents drawn at t = 500 seconds that the instantaneous rates of change in the concentrations of the reactants and products are related by their stoichiometric factors. The rate of hydrogen production, for example, is observed to be three times greater than that for nitrogen production:

2.91 × 10 −6 M /s 9.71 × 10 −6 M /s 3
A graph is shown with the label, “Time ( s ),” appearing on the x-axis and, “Concentration ( M ),” on the y-axis. The x-axis markings begin at 0 and end at 2000. The markings are labeled at intervals of 500. The y-axis begins at 0 and includes markings every 1.0 times 10 superscript negative 3, up to 4.0 times 10 superscript negative 3. A decreasing, concave up, non-linear curve is shown, which begins at about 2.8 times 10 superscript negative 3 on the y-axis and nearly reaches a value of 0 at the far right of the graph at the 2000 marking on the x-axis. This curve is labeled, “[ N H subscript 3].” Two additional curves that are increasing and concave down are shown, both beginning at the origin. The lower of these two curves is labeled, “[ N subscript 2 ].” It reaches a value of approximately 1.25 times 10 superscript negative 3 at 2000 seconds. The final curve is labeled, “[ H subscript 2 ].” It reaches a value of about 3.9 times 10 superscript negative 3 at 2000 seconds. A red tangent line segment is drawn to each of the curves on the graph at 500 seconds. At 500 seconds on the x-axis, a vertical dashed line is shown. Next to the [ N H subscript 3] graph appears the equation “negative capital delta [ N H subscript 3 ] over capital delta t = negative slope = 1.94 times 10 superscript negative 6 M / s.” Next to the [ N subscript 2] graph appears the equation “negative capital delta [ N subscript 2 ] over capital delta t = negative slope = 9.70 times 10 superscript negative 7 M / s.” Next to the [ H subscript 2 ] graph appears the equation “negative capital delta [ H subscript 2 ] over capital delta t = negative slope = 2.91 times 10 superscript negative 6 M / s.”
This graph shows the changes in concentrations of the reactants and products during the reaction 2 NH 3 3 N 2 + H 2 . The rates of change of the three concentrations are related by their stoichiometric factors, as shown by the different slopes of the tangents at t = 500 s.

Expressions for relative reaction rates

The first step in the production of nitric acid is the combustion of ammonia:

4 NH 3 ( g ) + 5 O 2 ( g ) 4 NO ( g ) + 6 H 2 O ( g )

Write the equations that relate the rates of consumption of the reactants and the rates of formation of the products.

Solution

Considering the stoichiometry of this homogeneous reaction, the rates for the consumption of reactants and formation of products are:

1 4 Δ [ NH 3 ] Δ t = 1 5 Δ [ O 2 ] Δ t = 1 4 Δ [ NO ] Δ t = 1 6 Δ [ H 2 O ] Δ t

Check your learning

The rate of formation of Br 2 is 6.0 × 10 −6 mol/L/s in a reaction described by the following net ionic equation:

5Br + BrO 3 + 6H + 3Br 2 + 3H 2 O

Write the equations that relate the rates of consumption of the reactants and the rates of formation of the products.

Answer:

1 5 Δ [ Br ] Δ t = Δ [ BrO 3 ] Δ t = 1 6 Δ [ H + ] Δ t = 1 3 Δ [ Br 2 ] Δ t = 1 3 Δ [ H 2 O ] Δ t

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Reaction rate expressions for decomposition of h 2 O 2

The graph in [link] shows the rate of the decomposition of H 2 O 2 over time:

2H 2 O 2 2H 2 O + O 2

Based on these data, the instantaneous rate of decomposition of H 2 O 2 at t = 11.1 h is determined to be
3.20 × 10 −2 mol/L/h, that is:

Δ [ H 2 O 2 ] Δ t = 3.20 × 10 −2 mol L −1 h −1

What is the instantaneous rate of production of H 2 O and O 2 ?

Solution

Using the stoichiometry of the reaction, we may determine that:

1 2 Δ [ H 2 O 2 ] Δ t = 1 2 Δ [ H 2 O ] Δ t = Δ [ O 2 ] Δ t

Therefore:

1 2 × 3.20 × 10 −2 mol L −1 h −1 = Δ [ O 2 ] Δ t

and

Δ [ O 2 ] Δ t = 1.60 × 10 −2 mol L −1 h −1

Check your learning

If the rate of decomposition of ammonia, NH 3 , at 1150 K is 2.10 × 10 −6 mol/L/s, what is the rate of production of nitrogen and hydrogen?

Answer:

1.05 × 10 −6 mol/L/s, N 2 and 3.15 × 10 −6 mol/L/s, H 2 .

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Key concepts and summary

The rate of a reaction can be expressed either in terms of the decrease in the amount of a reactant or the increase in the amount of a product per unit time. Relations between different rate expressions for a given reaction are derived directly from the stoichiometric coefficients of the equation representing the reaction.

Key equations

  • relative reaction rates for a A b B = 1 a Δ [ A ] Δ t = 1 b Δ [ B ] Δ t

Chemistry end of chapter exercises

What is the difference between average rate, initial rate, and instantaneous rate?

The instantaneous rate is the rate of a reaction at any particular point in time, a period of time that is so short that the concentrations of reactants and products change by a negligible amount. The initial rate is the instantaneous rate of reaction as it starts (as product just begins to form). Average rate is the average of the instantaneous rates over a time period.

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Ozone decomposes to oxygen according to the equation 2O 3 ( g ) 3O 2 ( g ) . Write the equation that relates the rate expressions for this reaction in terms of the disappearance of O 3 and the formation of oxygen.

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In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in the separation of uranium isotopes. Chlorine trifluoride is prepared by the reaction Cl 2 ( g ) + 3F 2 ( g ) 2ClF 3 ( g ) . Write the equation that relates the rate expressions for this reaction in terms of the disappearance of Cl 2 and F 2 and the formation of ClF 3 .

rate = + 1 2 Δ [ CIF 3 ] Δ t = Δ [ Cl 2 ] Δ t = 1 3 Δ [ F 2 ] Δ t

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A study of the rate of dimerization of C 4 H 6 gave the data shown in the table:
2C 4 H 6 C 8 H 12

Time (s) 0 1600 3200 4800 6200
[C 4 H 6 ] ( M ) 1.00 × 10 −2 5.04 × 10 −3 3.37 × 10 −3 2.53 × 10 −3 2.08 × 10 −3

(a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s.

(b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C 4 H 6 ]. What are the units of this rate?

(c) Determine the average rate of formation of C 8 H 12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).

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A study of the rate of the reaction represented as 2 A B gave the following data:

Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0
[ A ] ( M ) 1.00 0.952 0.625 0.465 0.370 0.308 0.230

(a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s.

(b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [ A ]. What are the units of this rate?

(c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.

(a) average rate, 0 − 10 s = 0.0375 mol L −1 s −1 ; average rate, 12 − 18 s = 0.0225 mol L −1 s −1 ; (b) instantaneous rate, 15 s = 0.0500 mol L −1 s −1 ; (c) average rate for B formation = 0.0188 mol L −1 s −1 ; instantaneous rate for B formation = 0.0250 mol L −1 s −1

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Consider the following reaction in aqueous solution:
5Br ( aq ) + BrO 3 ( aq ) + 6H + ( aq ) 3Br 2 ( aq ) + 3H 2 O( l )

If the rate of disappearance of Br ( aq ) at a particular moment during the reaction is 3.5 × 10 −4 M s −1 , what is the rate of appearance of Br 2 ( aq ) at that moment?

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Questions & Answers

what are oxidation numbers
Idowu Reply
pls what is electrolysis
Idowu Reply
Electrolysis is the process by which ionic substances are decomposed (broken down) into simpler substances when an electric current is passed through them. ... Electricity is the flow of electrons or ions. For electrolysis to work, the compound must contain ions.
AZEEZ
thanks
Idowu
what is the basicity of an atom
Eze Reply
basicity is the number of replaceable Hydrogen atoms in a Molecule. in H2SO4, the basicity is 2. in Hcl, the basicity is 1
Inemesit
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2.8.1
david
1s²2s²2p⁶3s¹
Haile
2, 6, 2, 1
Salman
1s2, 2s2, 2px2, 2py2, 2pz2, 3s1
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1s2,2s2,2py2,2
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1s2,2s2,2p6,
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1s2,2s2,2px2,2py2,2pz2,3s1
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Austin Reply
cathode is a negative ion why is it that u said is negative
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cathode is a negative electrode while cation is a positive ion. cation move towards cathode plate.
king
CH3COOH +NaOH ,complete the equation
david Reply
compare and contrast the electrical conductivity of HCl and CH3cooH
Sa Reply
The must be in dissolved in water (aqueous). Electrical conductivity is measured in Siemens (s). HCl (aq) has higher conductivity, as it fully ionises (small portion of CH3COOH (aq) ionises) when dissolved in water. Thus, more free ions to carry charge.
Abdelkarim
HCl being an strong acid will fully ionize in water thus producing more mobile ions for electrical conduction than the carboxylic acid
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differiante between a weak and a strong acid
david
how can I tell when an acid is weak or Strong
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an aqueous solution of copper sulphate was electrolysed between graphite electrodes. state what was observed at the cathode
Bakanya Reply
write the equation for the reaction that took place at the anode
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what is enthalpy of combustion
Bakanya
Enthalpy change of combustion: It is the enthalpy change when 1 mole of substance is combusted with excess oxygen under standard conditions. Elements are in their standard states. Conditions: pressure = 1 atm Temperature =25°C
Abdelkarim
Observation at Cathode: Cu metal deposit (pink/red solid).
Abdelkarim
Equation at Anode: (SO4)^2- + 4H^+ + 2e^- __> SO2 + 2H2O
Abdelkarim
Equation : CuSO4 -> Cu^2+ + SO4^2- equation at katode: 2Cu^2+ + 4e -> 2Cu equation at anode: 2H2O -> 4H+ + O2 +4e at the anode which reacts is water because SO4 ^ 2- cannot be electrolyzed in the anode
Niken
Practice Key Terms 5

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Source:  OpenStax, Chemistry. OpenStax CNX. May 20, 2015 Download for free at http://legacy.cnx.org/content/col11760/1.9
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