Question 1

At a certain temperature,nitrogen and hydrogen react to form ammonia: N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g). When initial amounts of N₂,H₂,and NH₃ are mixed,the concentration of NH₃ increases.Which statement below is true?

Accepted Answer

The increase in concentration of NH₃ indicates that the reaction is proceeding in the forward direction. Therefore, the reaction quotient Q must be less than the equilibrium constant Kc. According to Le Chatelier's principle, when the system is not at equilibrium, it will adjust to reach equilibrium. Thus, the system will shift towards the products to increase the production of NH3 until Q=Kc. Since Q is less than Kc, it means that there are relatively more reactants than products, and the forward reaction is favored. Therefore, Kc>Q, and the correct answer is B.

Question 2

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. -Which picture (2)-(4)represents the equilibrium mixture when more solid CaCO₃ is added?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Question 3

For the reaction: N₂(g)+ 2 O₂(g)⇌ 2 NO₂(g),K_c = 8.3 × 10^-10 at 25°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Accepted Answer

The answer of For the reaction: N₂(g)+ 2 O₂(g)⇌ 2...

Question 4

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g)⇌ I₂(g)+ Cl₂(g). What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0-L flask?

Accepted Answer

The answer of At a certain temperature the equilibrium constant,K_c,equals...

Question 5

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250° 0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Accepted Answer

The equilibrium expression is Kc = [PCl3][Cl2]/[PCl5]. By setting up an ICE table and solving for x, the change in concentration, we find the equilibrium concentrations that satisfy Kc = 1.80.

Question 6

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. 
-Which picture (2)-(4)represents the equilibrium mixture at a higher temperature?

Accepted Answer

Picture (4) likely represents the equilibrium mixture at a higher temperature if it shows an increased concentration of products for an endothermic reaction or decreased concentration of products for an exothermic reaction, according to Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. For an endothermic reaction, increasing the temperature shifts the equilibrium to the right (producing more products), while for an exothermic reaction, it shifts the equilibrium to the left (producing more reactants).

Question 7

Cyclohexane,C₆H₁₂,undergoes a molecular rearrangement in the presence of AlCl₃ to form methylcyclopentane,CH₃C₅H_9, according to the equation: C₆H₁₂ ⇌ CH₃C₅H₉ If K_c = 0.143 at 25°C for this reaction,find the equilibrium concentrations of C₆H₁₂ and CH₃C₅H₉ if the initial concentrations are 0.200 M and 0.075 M,respectively.

Accepted Answer

The answer of Cyclohexane,C₆H₁₂,undergoes a molecular rearrangement in the presence...

Question 8

Picture (1)represents the equilibrium mixture for the reaction A + B ⇌ 2 AB at 298 K. 
-If this reaction is endothermic,which picture (2)-(4)represents the equilibrium mixture at 400 K?

Accepted Answer

Since the reaction is endothermic, we need to shift the equilibrium to the right to counteract the increase in temperature. Therefore, we need to choose the option where the concentration of the products is higher than at 298 K. Option (B) shows a higher concentration of AB compared to the other options, so it is the best choice.

Question 9

The decomposition of ammonia is: 2 NH₃(g)= N₂(g)+ 3 H₂(g).If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.10 atm and H₂ is 0.15 atm?

Accepted Answer

We can use the formula for equilibrium constant (Kp) in terms of partial pressures:

Kp = (P_{NS} * P_{H2}^3) / P_{NH3}^2

Substituting the given values:

1.5 × 10^13 = (0.10) * (0.15)^3 / P_{NH3}^2

Solving for P_{NH3}, we get:

P_{NH3}^2 = (0.10) * (0.15)^3 / 1.5 × 10^13

P_{NH3}^2 = 7.5 × 10^-17

P_{NH3} = 2.74 × 10^-9 atm (taking the positive square root)

Therefore, the partial pressure of ammonia at equilibrium is 2.74 × 10^-9 atm, which is closest to option B (4.7 × 10^-4 atm) when rounded to the nearest order of magnitude.

Question 10

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). If a 3.00-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

Accepted Answer

The equilibrium constant, K, can be found by plugging in the concentrations of the reactants and products at equilibrium into the equilibrium expression.

K = [COS]/[CO][O2] = 1.4 × 10^12

Let x be the amount of CO at equilibrium. Then, the change in concentration of each species is:

[COS]: -2x mol
[CO]: +2x mol
[O2]: -x mol

At equilibrium,

[COS] = 0.400 - 2x
[O2] = 0.100 - x
[CO] = x

Using the equilibrium constant expression, we can set up an equation:

1.4 × 10^12 = ([COS]/[CO][O2])eq = ((0.400 - 2x)/x(0.100 - x))eq

Solving for x, we get x = 0.185 mol, which is the amount of CO at equilibrium.

Therefore, the answer is B) 0.185 mol.

Question 11

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. 
-Which picture (2)-(4)represents the equilibrium mixture when more solid CaO is added?

Accepted Answer

When more solid CaO is added, it reacts with gaseous COS to form more CaCOS. According to Le Chatelier's principle, the equilibrium will shift towards the reactants in order to counteract the addition of the product. As a result, the amount of CaCOS will increase, causing a decrease in the amount of CaO and COS. Picture (2) represents this shift in equilibrium as it shows an increase in the solid CaCOS and a decrease in the amounts of solid CaO and gaseous COS. Pictures (3) and (4) show a decrease in the amount of solid CaO, but they do not show an increase in solid CaCOS to the same extent as picture (2), so they are not the best choices.

Question 12

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Accepted Answer

We can use the equilibrium expression for this reaction: K_p=(Ptrans-2-butene)/(Pcis-2-butene) We can rearrange this expression to solve for Ptrans-2-butene: Ptrans-2-butene=K_p*Pcis-2-butene At equilibrium, the ratio of Ptrans-2-butene to Pcis-2-butene should be equal to the equilibrium constant, K_p: K_p=(Ptrans-2-butene)/(Pcis-2-butene) Let x be the change in pressure from the initial pressure for both cis-2-butene and trans-2-butene. Then the equilibrium pressures will be: Pcis-2-butene=0.250 - x Ptrans-2-butene=0.145 + x Substituting into the equilibrium expression: K_p = (0.145 + x)/(0.250 - x) Solving for x: x = 0.0787 atm Substituting x into the expressions for Pcis-2-butene and Ptrans-2-butene: Pcis-2-butene = 0.250 - 0.0787 = 0.171 atm Ptrans-2-butene = 0.145 + 0.0787 = 0.223 atm Therefore, the equilibrium pressure of cis-2-butene is 0.171 atm and the equilibrium pressure of trans-2-butene is 0.223 atm. The closest answer choice is D, which gives the correct values to two significant figures.

Question 13

The equilibrium constant,K_p,equals 3.40 at 25°C for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 5.00 atm of each gas,in what direction will the system shift to reach equilibrium?

Accepted Answer

Since K_p is greater than 1, the reaction favors the products, namely, trans-2-butene. Therefore, the system will shift to the right to reach equilibrium and increase the concentration of trans-2-butene.

Question 14

Cyclohexane (C₆H₁₂)undergoes a molecular rearrangement in the presence of AlCl₃ to form methylcyclopentane (MCP)according to the equation: C₆H₁₂ ⇌ MCP If K_c = 0.143 at 25°C for this reaction,predict the direction in which the system will shift if the initial concentrations of C₆H₁₂ and MCP are 0.0400 M and 0.0200 M,respectively.The system

Accepted Answer

The value of the equilibrium constant, Kc, is less than 1 (0.143), indicating the reactants are favored at equilibrium. Since the initial concentration of the product (MCP) is greater than that of the reactant (cyclohexane), the system is not at equilibrium. The system will shift towards the reactants to reach equilibrium, meaning it will shift to the left. Therefore, the answer is A.

Question 15

For the isomerization reaction: Butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Accepted Answer

Using the equilibrium constant expression:
Kp = P(isobutane) / (P(butane))^3

We can write an ICE table:
Initial        Change          Equilibrium
P(butane)    -x                20 - x
P(isobutane)  +x                x

At equilibrium:
Kp = P(isobutane) / (P(butane))^3
25 = x / (20 - x)^3
x = 3.58 atm

Plugging x into the equilibrium expressions, we get:
P(butane) = 0.77 atm
P(isobutane) = 19.2 atm

Therefore, the best choice is A.

Question 16

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. 
-Which picture (2)-(4)represents the equilibrium mixture when a catalyst is added?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Question 17

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). What is the equilibrium concentration of CO?

Accepted Answer

Using the equilibrium expression Kc = [CO2]^2 / ([CO]^2 * [O2]), and substituting the given values, solve for [CO].

Question 18

Picture (1)represents the equilibrium mixture for the gas-phase reaction A + B ⇌ 2 AB at 298 K.If the volume of the equilibrium mixture is decreased,which picture (2)-(4)represents the equilibrium at the reduced volume?

Accepted Answer

The answer of Picture (1)represents the equilibrium mixture for the...

Question 19

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g). If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

Accepted Answer

The answer of The equilibrium constant is equal to 5.00...

Question 20

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. -Which picture (2)-(4)represents the equilibrium mixture after addition of four more CO₂ molecules?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Quiz 13: Chemical Equilibrium

At a certain temperature,nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) . When initial amounts of N₂,H₂,and NH₃ are mixed,the concentration of NH₃ increases.Which statement below is true?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaCO₃ is added?

For the reaction: N₂(g) + 2 O₂(g) ⇌ 2 NO₂(g) ,K_c = 8.3 × 10^-10 at 25°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) . What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0-L flask?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250° 0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture at a higher temperature?

Picture (1) represents the equilibrium mixture for the reaction A + B ⇌ 2 AB at 298 K. -If this reaction is endothermic,which picture (2) -(4) represents the equilibrium mixture at 400 K?

The decomposition of ammonia is: 2 NH₃(g) = N₂(g) + 3 H₂(g) .If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.10 atm and H₂ is 0.15 atm?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . If a 3.00-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaO is added?

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

The equilibrium constant,K_p,equals 3.40 at 25°C for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 5.00 atm of each gas,in what direction will the system shift to reach equilibrium?

For the isomerization reaction: Butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when a catalyst is added?

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . What is the equilibrium concentration of CO?

Picture (1) represents the equilibrium mixture for the gas-phase reaction A + B ⇌ 2 AB at 298 K.If the volume of the equilibrium mixture is decreased,which picture (2) -(4) represents the equilibrium at the reduced volume?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) . If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture after addition of four more CO₂ molecules?

Quiz 13: Chemical Equilibrium

At a certain temperature,nitrogen and hydrogen react to form ammonia: N2(g) + 3 H2(g) ⇌ 2 NH3(g) . When initial amounts of N2,H2,and NH3 are mixed,the concentration of NH3 increases.Which statement below is true?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaCO3 is added?

For the reaction: N2(g) + 2 O2(g) ⇌ 2 NO2(g) ,Kc = 8.3 × 10-10 at 25°C.What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g) . What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0-L flask?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 0.125 M PCl5 is added to the flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture at a higher temperature?

Picture (1) represents the equilibrium mixture for the reaction A + B ⇌ 2 AB at 298 K. -If this reaction is endothermic,which picture (2) -(4) represents the equilibrium mixture at 400 K?

The decomposition of ammonia is: 2 NH3(g) = N2(g) + 3 H2(g) .If Kp is 1.5 × 103 at 400°C,what is the partial pressure of ammonia at equilibrium when N2 is 0.10 atm and H2 is 0.15 atm?

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) . If a 3.00-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium,how many moles of CO are also present in the flask?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaO is added?

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

The equilibrium constant,Kp,equals 3.40 at 25°C for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 5.00 atm of each gas,in what direction will the system shift to reach equilibrium?

For the isomerization reaction: Butane ⇌ isobutane Kp equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture when a catalyst is added?

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) . What is the equilibrium concentration of CO?

Picture (1) represents the equilibrium mixture for the gas-phase reaction A + B ⇌ 2 AB at 298 K.If the volume of the equilibrium mixture is decreased,which picture (2) -(4) represents the equilibrium at the reduced volume?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) . If initial concentrations are [SO2] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 M,the system is

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture after addition of four more CO2 molecules?

At a certain temperature,nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) . When initial amounts of N₂,H₂,and NH₃ are mixed,the concentration of NH₃ increases.Which statement below is true?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaCO₃ is added?

For the reaction: N₂(g) + 2 O₂(g) ⇌ 2 NO₂(g) ,K_c = 8.3 × 10^-10 at 25°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) . What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0-L flask?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250° 0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture at a higher temperature?

The decomposition of ammonia is: 2 NH₃(g) = N₂(g) + 3 H₂(g) .If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.10 atm and H₂ is 0.15 atm?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . If a 3.00-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaO is added?

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?

The equilibrium constant,K_p,equals 3.40 at 25°C for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene. If a flask initially contains 5.00 atm of each gas,in what direction will the system shift to reach equilibrium?

For the isomerization reaction: Butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 20.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when a catalyst is added?

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . What is the equilibrium concentration of CO?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) . If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture after addition of four more CO₂ molecules?