(a)
Interpretation:
A graph of ln k v/s 1/T is to be constructed for the given data of decomposition of PAN.
0 °C | k = |
10 °C | k = |
20 °C | k = |
30 °C | k = |
Concept introduction:
- Arrhenius equation relates the rate constant (k) of the reaction to its absolute temperature as-
Where
A − Pre-exponential factor
Ea- Activation energy
T- Absolute temperature in Kelvins
R- Universal gas constant
(b)
Interpretation:
The activation energy (Ea ) is to be calculated for the given data of decomposition of PAN.
0 °C | k = |
10 °C | k = |
20 °C | k = |
30 °C | k = |
Concept introduction:
- Arrhenius equation relates the rate constant (k) of the reaction to its absolute temperature as-
Where
A − Pre-exponential factor
Ea- Activation energy
T- Absolute temperature in Kelvins
R- Universal gas constant
(c)
Interpretation:
The half-life for the decomposition of PAN at 40°C is to be calculated.
0 °C | k = |
10 °C | k = |
20 °C | k = |
30 °C | k = |
Ea =
Concept introduction:
- At two different temperatures, Arrhenius equation can be modified as:
Where k − rate constants
Ea- Activation energy
T- Absolute temperature in Kelvins
R- Universal gas constant
Want to see the full answer?
Check out a sample textbook solutionChapter 20 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
- The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?arrow_forwardWhy are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?arrow_forwardIn Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If this reaction is so product-favored, why can large piles of yellow sulfur exist in our environment (as they do in Louisiana and Texas)?arrow_forward
- . Suppose that for the reaction 2N2O(g)+O2(g)4NO((g))it is determined, at a particular temperature, that the equilibrium concentrations arc [NO(g)]=0.00341M,[N2O(g)]=0.0293M, and [O2(g)]=0.0325M. Calculate the value of K for the reaction at this temperature.arrow_forward5.12. True or false: If all the partial pressures of reactants and products drop by half, the value of Q drops by half. Give an example of a chemical reaction to support your answer.arrow_forwardSilicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.arrow_forward
- A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.arrow_forward. Hydrogen gas and chlorine gas in the presence of light react explosively to form hydrogen chloride H2(g)+Cl2(g)2HCl(g)The reaction is strongly exothermic. Would an increase in temperature for the system lend to favor or disfavor the production of hydrogen chloride?arrow_forwardSubstances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?arrow_forward
- . Suppose a reaction has the equilibrium constant K=1.7108at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?arrow_forwardFor the reaction: CH,CH3(g) + 2H,0(g) +Ni(s) 5 2CO(g) + 5H2(g) +Ni(s) AH= +300 kJ/mol (a) Write the equilibrium constant expression in Kp and Kc. (b) Will an increase in the reaction temperature of the system favor the formation of the products? (c) What is the effect on the rate of the reaction when the Ni is removed? (d) If the reaction was done in a 1000 mL flask, what would be the effect on the equilibrium if the volume of the flask is decreased to 500 mL?arrow_forwardConsider the elementary reactions and their rate constants. kf = 4.99 × 10–2s-1 k, = 3.67 × 10-' s-' A(g) + B(g) → C(g) + D(g) C(g) + D(g) A(g) + B(g) What is the equilibrium constant (K) of the following generic reaction? A(g) + B(g) = C(g) + D(g) Ke = Which statement correctly describes the partial pressures of the reactants and products at equilibrium? The partial pressures of the reactants are greater than the partial pressures of the products at equilibrium. The partial pressures of the products are greater than the partial pressures of the reactants at equilibrium. The partial pressures of the reactants and products are equal at equilibrium.arrow_forward
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning