Deck 15: Chemical Equilibrium

Question 1

At equilibrium, the forward reaction rate is greater than the reverse reaction rate.

Answer 1

False

Question 2

Identify the equilibrium constant expression for the following reaction: $2 \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } ( \mathrm {~g} ) + 25 \mathrm { O } _ { 2 } ( \mathrm {~g} ) f \quad 16 \mathrm { CO } _ { 2 } ( \mathrm {~g} ) + 18 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } )$

A) $\frac { \left[ \mathrm { CO } _ { 2 } \right] ^ { 16 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 18 } } { \left[ \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } \right] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 25 } }$
B) $\left[ \mathrm { CO } _ { 2 } \right] ^ { 16 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 13 } \left[ \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } \right] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 25 }$
C) $\left[ \mathrm { CO } _ { 2 } \right] ^ { 16 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 18 } - \left[ \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } \right] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 25 }$
D) $\left[ \mathrm { CO } _ { 2 } \right] ^ { 16 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 18 } + \left[ \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } \right] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 25 }$
E) $\frac { \left[ \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } \right] ^ { 2 } - \left[ \mathrm { O } _ { 2 } \right] ^ { 25 } } { \left[ \mathrm { CO } _ { 2 } \right] ^ { 16 } - \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 18 } }$

Answer 2

$\frac { \left[ \mathrm { CO } _ { 2 } \right] ^ { 16 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 18 } } { \left[ \mathrm { C } _ { 8 } \mathrm { H } _ { 18 } \right] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 25 } }$

Question 3

Identify the expression for $K _ { \mathrm { p } }$ for the reaction $\mathrm { CaCO } _ { 3 } ( \mathrm {~s} ) f \quad \mathrm { CaO } ( \mathrm { s } ) + \mathrm { CO } _ { 2 } ( \mathrm {~g} )$ .

A) $K _ { \mathrm { p } } = P _ { \mathrm { CO } _ { 2 } }$
B) $K _ { \mathrm { p } } = P _ { \mathrm { Ca0 } }$
C) $K _ { \mathrm { p } } = P _ { \mathrm { CaCO } _ { 3 } }$
D) $K_{\mathrm{p}}=\frac{\left(P_{\mathrm{CO}_{2}}\right)\left(P_{\mathrm{CaO}}\right)}{\left(P_{\mathrm{CaCO}_{3}}\right)}$
E) $K _ { \mathrm { p } } = \frac { \left( P _ { \mathrm { CaCO } } \right) } { \left( P _ { \mathrm { CO } _ { 2 } } \right) \left( P _ { \mathrm { CaO } } \right) }$

Answer 3

$K _ { \mathrm { p } } = P _ { \mathrm { CO } _ { 2 } }$

Question 4

The equilibrium constant of a reaction $\mathrm { A } + \mathrm { B } f$ $\quad$ $\quad$ $\mathrm { C }$ at 320 ${ } ^ { \circ } \mathrm { C }$ is 9.60 $\times 10 ^ { 5 }$ . At the same temperature, the equilibrium constant for the reverse reaction $\text { Cf } ~~~~~~\mathrm { A } + \mathrm { B }$ will be _____.

A) 0.000
B) 9.22 $\times 10 ^ { 11 }$
C) 4.80 $\times 10 ^ { 5 }$
D) 1.04 $\times 10 ^ { - 6 }$
E) 9.06 $\times 10 ^ { 5 }$

Question 5

K_p = K only if the moles of gaseous products and gaseous reactants are different.

Question 6

Calculate K_p for the reaction $2 \mathrm { SO } _ { 2 } ( \mathrm {~g} ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) f \quad 2 \mathrm { SO } _ { 3 } ( \mathrm {~g} )$ at a temperature of 439 ${ } ^ { \circ } \mathrm { C }$ , if K = 5.10 × 10⁴ at the same temperature.

A) 1.90 ×10²
B) 8.72 ×10²
C) 1.40×10³
D) 0.60 ×10³
E) 6.50 ×10²

Question 7

The unit of equilibrium constant is mol/L.

Question 8

Define chemical equilibrium.

Question 9

_____ constants are calculated using effective concentrations, or activities, of reactants and products.

A) Formation
B) Planck's
C) Dielectric
D) Faraday's
E) Equilibrium

Question 10

Values of equilibrium constant (K) greater than 10³ indicate a strong tendency for reactants to form products.

Question 11

_____ is the point at which the forward and reverse reaction rates become the same so that the net composition of the system no longer changes with time.

Question 12

The equilibrium constant for a reaction written in reverse is the same as that written originally.

Question 13

Which of the following is the expression to calculate the equilibrium constant for partial pressures?

A) $K _ { \mathrm { p } } = \frac { \left( P _ { \mathrm { C } } \right) ^ { \mathrm { c } } \left( P _ { \mathrm { D } } \right) ^ { \mathrm { d } } } { \left( P _ { \mathrm { A } } \right) ^ { \mathrm { a } } \left( P _ { \mathrm { B } } \right) ^ { \mathrm { b } } }$
B) $K _ { \mathrm { p } } = \left( P _ { \mathrm { C } } \right) ^ { \mathrm { c } } \left( P _ { \mathrm { D } } \right) ^ { \mathrm { d } } + \left( P _ { \mathrm { A } } \right) ^ { \mathrm { a } } \left( P _ { \mathrm { B } } \right) ^ { \mathrm { b } }$
C) $K _ { \mathrm { p } } = \left( P _ { \mathrm { C } } \right) ^ { \mathrm { c } } \left( P _ { \mathrm { D } } \right) ^ { \mathrm { d } } - \left( P _ { \mathrm { A } } \right) ^ { \mathrm { a } } \left( P _ { \mathrm { B } } \right) ^ { \mathrm { b } }$
D) $K _ { \mathrm { P } } = \left( P _ { \mathrm { C } } \right) ^ { \mathrm { c } } + \left( P _ { \mathrm { D } } \right) ^ { \mathrm { d } } \times \left( P _ { \mathrm { A } } \right) ^ { \mathrm { a } } + \left( P _ { \mathrm { B } } \right) ^ { \mathrm { b } }$
E) $K _ { \mathrm { p } } = \frac { \left( P _ { \mathrm { A } } \right) ^ { \mathrm { a } } - \left( P _ { \mathrm { B } } \right) ^ { \mathrm { b } } } { \left( P _ { \mathrm { C } } \right) ^ { \mathrm { c } } - \left( P _ { \mathrm { D } } \right) ^ { \mathrm { d } } }$

Question 14

Chemical _____ is a dynamic process that consists of a forward reaction, in which reactants are converted to products, and a reverse reaction, in which products are converted to reactants.

A) transition
B) change
C) equilibrium
D) bonding
E) transmutation

Question 15

_____ are the ratios of the measured concentrations to a standard state of 1 M.

Question 16

What does the law of mass action state?

A) The lowest-energy electron configuration for an atom is the one that has the maximum number of electrons with parallel spins in degenerate orbitals.
B) For the general balanced chemical equation $a \mathrm {~A} + b \mathrm {~B} f \quad c \mathrm { C } + d \mathrm { D }$ , the equilibrium constant expression is
$K = \frac { [ \mathrm { C } ] ^ { c } [ \mathrm { D } ] ^ { d } } { [ \mathrm {~A} ] ^ { a } [ \mathrm {~B} ] ^ { b } }$ .
C) No two electrons in an atom can have the same value of all four quantum numbers.
D) The energy of the universe is constant: ? E_universe = ? E_system + ? E_surroundings = 0.
E) The entropy of the universe remains constant in a reversible process, whereas the entropy of the universe increases in an irreversible process.

Question 17

Explain the relationship between the equilibrium constant and the rate constants for the forward and reverse reactions with an example.

Question 18

The composition of an equilibrium mixture is dependent on the direction from which equilibrium is approached.

Question 19

Calculate the equilibrium constant K₃ for the reaction $\mathrm { CO } ( \mathrm { g } ) + 2 \mathrm { H } _ { 2 } \mathrm {~S} ( \mathrm {~g} ) f \quad \mathrm { CS } _ { 2 } ( \mathrm {~g} ) + \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) + \mathrm { H } _ { 2 } ( \mathrm {~g} )$ at 785 ${ } ^ { \circ } \mathrm { C }$ . Given that the equilibrium constant K₁ for the reaction $\mathrm { CO } ( \mathrm { g } ) + 3 \mathrm { H } _ { 2 } ( \mathrm {~g} ) f \quad \mathrm { CH } _ { 4 } ( \mathrm {~g} ) + \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } )$ is 7.34 $\times 10 ^ { - 2 }$ and the equilibrium constant K₂ for the reaction $\mathrm { CH } _ { 4 } ( \mathrm {~g} ) + 2 \mathrm { H } _ { 2 } \mathrm {~S} ( \mathrm {~g} ) f \quad \mathrm { CS } _ { 2 } ( \mathrm {~g} ) + 4 \mathrm { H } _ { 2 } ( \mathrm {~g} )$ is 2.89 $\times 10 ^ { 4 }$ .

A) 2.53 $\times 10 ^ { 2 }$
B) 7.34 $\times 10 ^ { - 2 }$
C) 2.89 $\times 10 ^ { 4 }$
D) 4.45 $\times 10 ^ { 3 }$
E) 2.12 $\times 10 ^ { 3 }$

Question 20

In the reaction $\mathrm{A}+\mathrm{B} f$ $\quad$ $\quad$ $\mathrm{C}$ , values of the equilibrium constant at various temperatures were found to be $K _ { 50 ^ { \circ } \mathrm { C } } = 4.60 \times 10 ^ { 32 }$ , $K _ { 160 ^ { \circ } \mathrm { C } } = 2.30 \times 10 ^ { 3 }$ and $K _ { 256^{?} \mathrm { C } } = 5.80$ . At what temperature would the proportion of A and B in the equilibrium mixture be the highest?

A) 206 ${ } ^ { \circ } \mathrm { C }$
B) 256 ${ } ^ { \circ } \mathrm { C }$
C) 150 ${ } ^ { \circ } \mathrm { C }$
D) 110 ${ } ^ { \circ } \mathrm { C }$
E) 160 ${ } ^ { \circ } \mathrm { C }$

Question 21

If $Q = K$ the system is at equilibrium.

Question 22

Explain the Le Châtelier's Principle.

Question 23

Explain the method to calculate an equilibrium constant from equilibrium concentrations with an example.

Question 24

A system whose reactants, products, or both are in more than one phase is a _____ equilibrium.

Question 25

Calculate K_p for the reaction $\mathrm { H } _ { 2 } ( g ) + \mathrm { I } _ { 2 } ( g ) f \quad 2 \mathrm { HI } ( g )$ . Given that the mixture of H₂ and I₂ was maintained at 740 K until the system reached equilibrium, and the equilibrium mixture contained 3.68 × 10^?2 M HI, 8.31 × 10^?3 M H₂, and 7.72 × 10^?4 M I₂.

A) 3.68 × 10^?2
B) 2.11 × 10²
C) 5.73 × 10³
D) 1.74 × 10^?4
E) 8.31 × 10^?3

Question 26

A large _____ constant implies that the reactants are converted almost entirely to products.

Question 27

If K > Q, then the ratio of the concentrations of products to the concentrations of reactants is greater than at equilibrium.

Question 28

The equilibrium constant K for the reaction $\mathrm { H } _ { 2 } ( \mathrm {~g} ) + \mathrm { CO } _ { 2 } ( \mathrm {~g} ) f \quad \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) + \mathrm { CO } ( \mathrm { g } )$ is 0.213 at 640 K. A mixture of gases that initially contains 0.0260 M H₂ and 0.0260 M CO₂ is allowed to equilibrate at 700 K. Calculate the final concentration of CO₂.

A) 1.779 × 10^-2
B) 8.203 × 10^-3
C) 0.213 × 10^-2
D) 0.026 × 10^-3
E) 0.052 × 10^-2

Question 29

The Le Châtelier's principle states that if stress is applied to a system at equilibrium, the composition of the system remains unchanged.

Question 30

Which of the following statements is true about Q and K?

A) If Q < K, then the ratio of the concentrations of products to the concentrations of reactants is more than the ratio at equilibrium.
B) If Q = K, then the system is at equilibrium.
C) if Q > K, then the ratio of the concentrations of products to the concentrations of reactants is less than at equilibrium.
D) If Q < K, then products are formed at the expense of the reactants.
E) If Q < K, then reactants are formed at the expense of products.

Question 31

A small equilibrium constant implies that the reactants are converted almost entirely to products.

Question 32

_____ are responsible for the scents associated with fruits such as oranges and bananas.

A) Crown ethers
B) Amalgams
C) Cryptands
D) Esters
E) Catalysts

Question 33

For the following reaction $A ( g ) + B ( g ) f \quad 2 C ( g )$ , $K _ { \mathrm { p } } = 1.8 \times 10 ^ { - 25 }$ at 30 ${ } ^ { \circ } \mathrm { C }$ . If $P _ { \mathrm { A } }$ = 0.56 atm and $P _ { B }$ = 0.18 atm, what will be the partial pressure of C in equilibrium with A and B at 1 atm?

A) 0.18
B) 0.56
C) 6.7 $\times 10 ^ { - 25 }$
D) $1.8 \times 10 ^ { - 25 }$
E) 1.3 $\times 10 ^ { - 13 }$

Question 34

Which of the following denotes the reaction quotient Q?

A) $[ A ] ^ { a } [ B ] ^ { b } + [ C ] ^ { c } [ D ] ^ { d }$
B) $[ A ] ^ { a } [ B ] ^ { b } × [ C ] ^ { c } [ D ] ^ { d }$
C) $[ \mathrm { C } ] ^ { \mathrm { c } } [ \mathrm { D } ] ^ { \mathrm { d } } - [ \mathrm { A } ] ^ { \mathrm { a } } [ \mathrm { B } ] ^ { \mathrm { b } }$
D) $\frac { [ \mathrm { C } ] ^ { \mathrm { c } } [ \mathrm { D } ] ^ { \mathrm { d } } } { [ \mathrm { A } ] ^ { \mathrm { a } } [ \mathrm { B } ] ^ { \mathrm { b } } }$
E) $[ \mathrm { C } ] ^ { \mathrm { c } } + [ \mathrm { D } ] ^ { \mathrm { d } } + [ \mathrm { A } ] ^ { \mathrm { a } } + [ \mathrm { B } ] ^ { \mathrm { b } }$

Question 35

Given that at equilibrium $[ \mathrm { A } ]$ =0.072 M and $[ \mathrm { B } ]$ =0.089 M at 40 ${ } ^ { \circ } \mathrm { C }$ , calculate the equilibrium constant $K$ from the equilibrium concentrations for the reaction $A ( g ) f \quad B ( g )$ .

A) $K = 0.072$
B) $K = 0.161$
C) $K = 1.23$
D) $K = 0.006$
E) $K = 0.089$

Question 36

Define reaction quotient

Question 37

_____ occurs when any change in a system affects the magnitude of Q or K.

A) Suspension
B) Activity
C) Stress
D) Cracking
E) Reforming

Question 38

Which of the following statements refer to the LeChâtelier's Principle?

A) If a stress is applied to a system at equilibrium, the composition of the system will change to relieve the applied stress.
B) The uncertainty in the position of a particle multiplied by the uncertainty in its momentum is greater than or equal to Planck's constant divided by 4π.
C) The energy of electromagnetic radiation is directly proportional to its frequency and inversely proportional to its wavelength.
D) No two electrons in an atom can have the same value of all four quantum numbers.
E) Matter and energy have properties typical of both waves and particles.

Question 39

In the reaction $\operatorname { HBr } ( g ) + \operatorname { NaH } ( \mathrm { s } ) f \quad \operatorname { NaBr } ( \mathrm { s } ) + \mathrm { H } _ { 2 } ( g )$ ,the concentration of H₂(g) will _____ when the concentration of HBr is decreased by a factor of 4.

A) increase by about a factor 2
B) decrease by about a factor 4
C) remain unchanged
D) decrease by about a factor 2
E) increase by about a factor 4

Question 40

A 1.00 mol sample of A was placed in a 2.00 L reactor and heated to 342 ${ } ^ { \circ } \mathrm { C }$ until the system reached equilibrium. The contents of the reactor then contained 0.0488 mol of C. What is K for the reaction 2A(g) $f$ 2B(g) +C(g) at the same temperature?

A) 1.45 $\times 10 ^ { - 3 }$
B) 4.37 $\times 10 ^ { - 4 }$
C) 2.64 $\times 10 ^ { - 4 }$
D) 2.85 $\times 10 ^ { - 4 }$
E) 3.59 $\times 10 ^ { - 3 }$

Question 41

If Q > K, then the ratio of the concentrations of products to the concentrations of reactants is _____ than at equilibrium.

Question 42

Explain the effect of the changes in temperature on the equilibrium of the system.

Question 43

Explain the effect of changes in total pressure or volume on the equilibrium of the system.

Question 44

The concentration of any gaseous reactant or product is inversely proportional to the applied pressure (P).

Question 45

What would be the reaction quotient for the reaction $2 \mathrm {~A} ( g ) f \quad 2 \mathrm {~B} ( g ) + \mathrm { C } ( g )$ if the pressure is decreased by a factor of 2 at constant temperature?

A) $Q = \frac { 1 } { 4 } K$
B) $Q = 2 K$
C) $Q = \frac { 1 } { 2 } K$
D) $Q = 4 K$
E) $Q = K$

Question 46

If a balanced chemical equation contains different numbers of gaseous reactant and product molecules, the _____ will be sensitive to changes in volume or pressure.

Question 47

Which of the following statements is true about the effect of changes in temperature on the equilibrium of the system?

A) Increasing the temperature will shift the exothermic reaction to the right.
B) Increasing the temperature decreases the magnitude of the equilibrium constant for an endothermic reaction.
C) Increasing the temperature increases the equilibrium constant for an exothermic reaction.
D) Increasing the temperature has no effect on the equilibrium constant for a thermally neutral reaction. HYPERLINK "http://catalog.flatworldknowledge.com/bookhub/reader/4309?e=averill_1.0-ch08" \l "averill_1.0-ch15_s05_s03_t01"
E) Increasing the temperature will shift the endothermic reaction to the left.

Question 48

In all reactions, if a _____ is applied to a system at equilibrium, the composition of the system will change to counteract the applied stress.

Question 49

Which of the following statements is true about the effect of changes in total pressure or volume on the equilibrium of a system?

A) The concentration of any gaseous reactant or product is directly proportional to the total volume and inversely proportional to the applied pressure.
B) The change in pressure above a liquid solution has little effect on the concentrations of dissolved substances.
C) The concentrations of gases remain constant with pressure.
D) The equilibrium compositions of systems that contain gaseous substances are insensitive to changes in pressure and volume.
E) The change in external pressure has a tremendous effect on an equilibrium system that contains only solids or liquids.

Question 50

What would be the effect of adding carbon dioxide on $[ \mathrm { CO } ]$ in the reaction, $\mathrm { CuO } ( \mathrm { s } ) + \mathrm { CO } ( \mathrm { g } ) f \mathrm { Cu } ( \mathrm { s } ) + \mathrm { CO } _ { 2 } ( \mathrm {~g} )$ ?

A) $[ \mathrm { CO } ]$ remains constant
B) $[ \mathrm { CO } ]$ increases
C) $[ \mathrm { CO } ]$ becomes zero
D) $[ \mathrm { CO } ]$ becomes insignificant
E) $[ \mathrm { CO } ]$ decreases

Question 51

Which of the following signifies the relationship between the concentration of a gas and its pressure?

A) $C = ( R T ) ^ { P }$
B) $C = P R T$
C) $C = P - R T$
D) $C = \frac { P } { R T }$
E) $C = \frac { R T } { P }$

Question 52

Changing the pressure above a liquid solution has a drastic effect on the concentrations of dissolved substances.

Question 53

A reaction with an unfavorable equilibrium constant can be driven to completion by continually removing one of the _____ of the reaction.

Question 54

_____ states that if a stress is applied to a system at equilibrium, the composition of the system will adjust to counteract the stress.

Question 55

The equilibrium compositions of systems that contain _____ substances are quite sensitive to changes in pressure, volume, and temperature.

Question 56

The _____ has the same form as the equilibrium constant expression, but it is derived from concentrations obtained at any time.

Question 57

Increasing the pressure of a system favors the side of the reaction that has fewer gaseous molecules.

Question 58

A reaction can be forced to go essentially to completion, regardless of the magnitude of K, by continually removing one of the products from the reaction mixture.

Question 59

What would be the effect of decreasing the temperature for the reaction $\mathrm { A } ( g ) + 3 \mathrm {~B} ( g ) f \quad 2 \mathrm { C } ( g )$ given that $\Delta H _ { \mathrm { rMM } } = - 145 \mathrm {~kJ} / \mathrm { mol }$ ?

A) Equilibrium shifts to the left
B) There is no effect on the reaction
C) Formation of C is favored
D) Decomposition of C is favored
E) C remains constant

Question 60

How can a reaction with an unfavorable equilibrium constant be driven to completion?

A) By continually removing one of the products of the reaction
B) By keeping the temperature of the system constant
C) By keeping the pressure of the system constant
D) By continually removing one of the reactants of the reaction
E) By maintaining equal concentration of the reactants

Question 61

Removing heat from an _____ reaction favors the formation of products.

Question 62

Explain the Sohio acrylonitrile process.

Question 63

_____ control consists of adjusting conditions so that at equilibrium only the desired products are present in significant quantities.

Question 64

Differentiate between kinetic and thermodynamic control.

Question 65

Identify the following kinetically controlled reaction: $\mathrm{CH}_{2}=\mathrm{CHCH}_{3}(\mathrm{~g})+\mathrm{NH}_{3}(\mathrm{~g})+\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{2}=\mathrm{CHC} \equiv \mathrm{N}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$

A) The Haber-Bosch process
B) The Ostwald process
C) The water-gas shift reaction
D) The contact process
E) The Sohio acrylonitrile process

Question 66

_____ is the building block of the polymer called polyacrylonitrile.

Question 67

The altering of reaction conditions so that a single desired product or set of products is present in significant quantities at equilibrium is known as _____ control.

A) potential
B) ionic
C) electrostatic
D) kinetic
E) thermodynamic

Question 68

Which of the following is the thermodynamic controlled reaction that produces ammonia?

A) The contact process
B) The Haber-Bosch process
C) The Ostwald process
D) The water-gas shift reaction
E) The Sohio acrylonitrile process

Question 69

CH2=CHC≡N(g) is the product formed in the Haber-Bosch process.

Question 70

Which of the following is the kinetically controlled reaction that produces $\mathrm { CH } _ { 2 } = \mathrm { CHC } \equiv \mathrm { N } ( \mathrm { g } )$ ?

A) The Sohio acrylonitrile process
B) The contact process
C) The water-gas shift reaction
D) The Haber-Bosch process
E) The Ostwald process

Question 71

The altering of reaction conditions to control reaction rates, thereby obtaining a single desired product or set of products is known as _____ control.

A) thermodynamic
B) potential
C) electrostatic
D) kinetic
E) ionic

Question 72

The Sohio acrylonitrile process involves the reaction of nitrogen and hydrogen to form ammonia.

Question 73

The industrial Haber-Bosch process uses Fe₂O₃/K₂O as the mixed oxide catalyst to enable the reaction to proceed at a significant rate at temperatures of 400°C-530°C.