Question 1

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 2.00 atm of each gas,in what direction will the system shift to reach equilibrium?

Accepted Answer

The equilibrium constant (K) is greater than 1, indicating that the reaction favors the product (trans-2-butene). If the initial pressures of both isomers are the same, the system will shift towards the product side to reach equilibrium. Therefore, it will shift right.

Question 2

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). If a 3.50-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

From the given equilibrium constant, we can write the expression for the equilibrium constant in terms of the concentrations of the reactants and products: K = [CO₂]2 /[CO][O₂] At equilibrium, let the concentration of CO be x, then we have: [CO₂] = 0.400 mol / 3.50 L = 0.114 mol/L [O₂] = 0.100 mol / 3.50 L = 0.0286 mol/L Substituting these concentrations and the given equilibrium constant into the equilibrium expression, we get: 1.4 × 10² = (0.114 mol/L)2 / (x)(0.0286 mol/L) Solving for x, we get: x = 0.200 mol/L Therefore, the number of moles of CO present in the 3.50-L flask is: n(CO) = (0.200 mol/L)(3.50 L) = 0.700 mol Thus, the answer is B (0.200 mol)

Question 3

Express the equilibrium constant for the following reaction. Li ClO₃(s)⇌ Li ClO(s)+ O₂(g)

Accepted Answer

The answer of Express the equilibrium constant for the following...

Question 4

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

The equilibrium constant expression for the reaction is Kp = P(isobutane)/P(butane). Solving for equilibrium pressures using the initial conditions and Kp = 25, we find P(butane) = 0.77 atm and P(isobutane) = 19.2 atm.

Question 5

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 6

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s)⇌ 2 NH₃(g)+ CO₂(g)K_c = 1.58 × 10^-8 [NH₃]_eq = 2.7 × 10^-3 M

Accepted Answer

The answer of Consider the following reaction,equilibrium concentrations,and equilibrium constant...

Question 7

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2 NO₂(g)K_c = 0.21 [N₂O₄]_eq = 0.029 M

Accepted Answer

The equilibrium constant expression is Kc = [NO2]^2 / [N2O4]. Solving for [NO2], we get [NO2] = sqrt(Kc * [N2O4]) = sqrt(0.21 * 0.029) = 0.078 M.

Question 8

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PI₅]_eq = 0.56 M,[PI₃]_eq = 0.23 M,[I₂]_eq = 5.5 M. PI₅(g)⇌ PI₃(g)+ I₂(g)

Accepted Answer

The equilibrium constant expression for the reaction is:K_c = [PI₃][I₂]/[PI₅]Substituting the equilibrium concentrations into the expression, we get:K_c = (0.23)(5.5)/0.56 = 2.3Therefore, the value of K_c is 2.3.

Question 9

Consider the following reaction and its equilibrium constant: SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)K_c = 0.33 A reaction mixture contains 0.41 M SO₂,0.14 M NO_2, 0.12 M SO₃ and 0.14 M NO.Which of the following statements is TRUE concerning this system?

Accepted Answer

The reaction quotient Qc can be calculated as follows: Qc = [SO₃][NO] / [SO₂][NO_2,] Qc = (0.12)(0.14) / (0.41)(0.14) = 0.033 Since the equilibrium constant Kc is greater than Qc, the system is not at equilibrium and the reaction will shift in the direction of products to reach equilibrium. Therefore, the correct answer is choice C.

Question 10

For which reaction will K_p = K_c?

Accepted Answer

The answer of For which reaction will K_p = K_c? ...

Question 11

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 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

The answer of An equilibrium mixture of CO,O₂ and CO₂...

Question 12

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2I(g)K_p = 0.209 A reaction mixture contains 0.89atm I₂ and1.53 atm I.Which of the following statements is TRUE concerning this system?

Accepted Answer

To determine the direction of the reaction, we need to compare the reaction quotient (Q) with the equilibrium constant (K). Q = (I)^2 / (I₂) = (1.53 atm)^2 / (0.89 atm) = 2.63 atm Since Q > K, the system is not at equilibrium, and the reaction will shift in the direction of reactants to decrease Q and approach equilibrium. Therefore, the correct choice is A.

Question 13

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl)_eq = 0.22 atm,P(NO)_eq = 0.10 atm,P(Cl₂)_eq = 0.20 atm. 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g)

Accepted Answer

The answer of Determine the value of K_p for the...

Question 14

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

Since the concentration of NH₃ increases, it means that the reaction is proceeding in the forward direction, or towards the formation of ammonia. Therefore, the reaction quotient Q must be smaller than the equilibrium constant K for the forward reaction. Thus, K_c > Q, so the answer is B.

Question 15

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] = 1.20 M,[O₂] = 0.45 M,and [SO₃] = 1.80 M,the system is

Accepted Answer

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

Question 16

What is △n for the following equation in relating K_c to K_p? Li BrO₃(s)⇌ Li BrO(s)+ O₂(g)

Accepted Answer

△n is the change in the number of moles of gas, which is the moles of gaseous products minus the moles of gaseous reactants. Here, there is 1 mole of O2(g) produced and no gaseous reactants, so △n = 1 - 0 = 1.

Question 17

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M. H₂(g)+ I₂(g)⇌ 2 HI(g)

Accepted Answer

The equilibrium constant expression for the reaction is: K_c = [HI]_eq / ([H₂]_eq x [I₂]_eq]) Substitute the given equilibrium concentrations into the expression: K_c = (1.6 M)_eq / [(0.14 M)_eq x (0.39 M)_eq] K_c = 46.86 ≈ 47 Therefore, the answer is choice C, 47.

Question 18

Consider the following reaction and its equilibrium constant: 4 CuO(s)+ CH₄(g)⇌ CO₂(g)+ 4 Cu(s)+ 2 H₂O(g)K_c = 1.10 A reaction mixture contains 0.22 M CH₄,0.70 M CO₂and 1.5 M H₂O.Which of the following statements is TRUE concerning this system?

Accepted Answer

The reaction quotient can be calculated as [CO₂]^1[Cu]^4[H₂O]^2/[CH₄]^4[CuO]^4. Substituting the given concentrations, we get Q = (0.70)(1.5)^2/(0.22)^4 < Kc, the equilibrium constant. This means the reaction is not at equilibrium, and it will shift in the direction of reactants to establish equilibrium. Therefore, option D is the correct choice.

Question 19

Express the equilibrium constant for the following reaction. 2 Na(s)+ 2 H₂O(l)⇌ 2 NaOH(aq)+ H₂(g)

Accepted Answer

The answer of Express the equilibrium constant for the following...

Question 20

Consider the following reaction and its equilibrium constant: I₂(g)+ Br₂(g)⇌ 2 IBr(g)K_c = 1.1 × 10² A reaction mixture contains 0.35 M I₂,0.31 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Accepted Answer

The reaction quotient, Qc, is calculated as:Qc = [IBr]^2 / [I2] [Br2] = (3.5 M)^2 / (0.35 M) (0.31 M) = 1.1 × 10^2Since Qc = Kc, the system is at equilibrium.

Quiz 16: Chemical Equilibrium

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 2.00 atm of each gas,in what direction will the system shift to reach equilibrium?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . If a 3.50-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?

Express the equilibrium constant for the following reaction. Li ClO₃(s) ⇌ Li ClO(s) + O₂(g)

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?

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8 [NH₃]_eq = 2.7 × 10^-3 M

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g) . N₂O₄(g) ⇌ 2 NO₂(g) K_c = 0.21 [N₂O₄]_eq = 0.029 M

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PI₅]_eq = 0.56 M,[PI₃]_eq = 0.23 M,[I₂]_eq = 5.5 M. PI₅(g) ⇌ PI₃(g) + I₂(g)

Consider the following reaction and its equilibrium constant: SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) K_c = 0.33 A reaction mixture contains 0.41 M SO₂,0.14 M NO_2, 0.12 M SO₃ and 0.14 M NO.Which of the following statements is TRUE concerning this system?

For which reaction will K_p = K_c?

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 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?

Consider the following reaction and its equilibrium constant: I₂(g) ⇌ 2I(g) K_p = 0.209 A reaction mixture contains 0.89atm I₂ and1.53 atm I.Which of the following statements is TRUE concerning this system?

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl) _eq = 0.22 atm,P(NO) _eq = 0.10 atm,P(Cl₂) _eq = 0.20 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

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?

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] = 1.20 M,[O₂] = 0.45 M,and [SO₃] = 1.80 M,the system is

What is △n for the following equation in relating K_c to K_p? Li BrO₃(s) ⇌ Li BrO(s) + O₂(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M. H₂(g) + I₂(g) ⇌ 2 HI(g)

Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH₄(g) ⇌ CO₂(g) + 4 Cu(s) + 2 H₂O(g) K_c = 1.10 A reaction mixture contains 0.22 M CH₄,0.70 M CO₂and 1.5 M H₂O.Which of the following statements is TRUE concerning this system?

Express the equilibrium constant for the following reaction. 2 Na(s) + 2 H₂O(l) ⇌ 2 NaOH(aq) + H₂(g)

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2 IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.35 M I₂,0.31 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Quiz 16: Chemical Equilibrium

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 2.00 atm of each gas,in what direction will the system shift to reach equilibrium?

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) . If a 3.50-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?

Express the equilibrium constant for the following reaction. Li ClO3(s) ⇌ Li ClO(s) + O2(g)

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?

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g) . NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) Kc = 1.58 × 10-8 [NH3]eq = 2.7 × 10-3 M

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO2(g) . N2O4(g) ⇌ 2 NO2(g) Kc = 0.21 [N2O4]eq = 0.029 M

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PI5]eq = 0.56 M,[PI3]eq = 0.23 M,[I2]eq = 5.5 M. PI5(g) ⇌ PI3(g) + I2(g)

Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) Kc = 0.33 A reaction mixture contains 0.41 M SO2,0.14 M NO2, 0.12 M SO3 and 0.14 M NO.Which of the following statements is TRUE concerning this system?

For which reaction will Kp = Kc?

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0015 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?

Consider the following reaction and its equilibrium constant: I2(g) ⇌ 2I(g) Kp = 0.209 A reaction mixture contains 0.89atm I2 and1.53 atm I.Which of the following statements is TRUE concerning this system?

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl) eq = 0.22 atm,P(NO) eq = 0.10 atm,P(Cl2) eq = 0.20 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

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?

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] = 1.20 M,[O2] = 0.45 M,and [SO3] = 1.80 M,the system is

What is △n for the following equation in relating Kc to Kp? Li BrO3(s) ⇌ Li BrO(s) + O2(g)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M,[I2]eq = 0.39 M,[HI]eq = 1.6 M. H2(g) + I2(g) ⇌ 2 HI(g)

Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH4(g) ⇌ CO2(g) + 4 Cu(s) + 2 H2O(g) Kc = 1.10 A reaction mixture contains 0.22 M CH4,0.70 M CO2 and 1.5 M H2O.Which of the following statements is TRUE concerning this system?

Express the equilibrium constant for the following reaction. 2 Na(s) + 2 H2O(l) ⇌ 2 NaOH(aq) + H2(g)

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 102 A reaction mixture contains 0.35 M I2,0.31 M Br2 and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

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 2.00 atm of each gas,in what direction will the system shift to reach equilibrium?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . If a 3.50-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?

Express the equilibrium constant for the following reaction. Li ClO₃(s) ⇌ Li ClO(s) + O₂(g)

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?

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g) . NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) K_c = 1.58 × 10^-8 [NH₃]_eq = 2.7 × 10^-3 M

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g) . N₂O₄(g) ⇌ 2 NO₂(g) K_c = 0.21 [N₂O₄]_eq = 0.029 M

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PI₅]_eq = 0.56 M,[PI₃]_eq = 0.23 M,[I₂]_eq = 5.5 M. PI₅(g) ⇌ PI₃(g) + I₂(g)

Consider the following reaction and its equilibrium constant: SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) K_c = 0.33 A reaction mixture contains 0.41 M SO₂,0.14 M NO_2, 0.12 M SO₃ and 0.14 M NO.Which of the following statements is TRUE concerning this system?

For which reaction will K_p = K_c?

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 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?

Consider the following reaction and its equilibrium constant: I₂(g) ⇌ 2I(g) K_p = 0.209 A reaction mixture contains 0.89atm I₂ and1.53 atm I.Which of the following statements is TRUE concerning this system?

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl) _eq = 0.22 atm,P(NO) _eq = 0.10 atm,P(Cl₂) _eq = 0.20 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

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?

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] = 1.20 M,[O₂] = 0.45 M,and [SO₃] = 1.80 M,the system is

What is △n for the following equation in relating K_c to K_p? Li BrO₃(s) ⇌ Li BrO(s) + O₂(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M. H₂(g) + I₂(g) ⇌ 2 HI(g)

Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH₄(g) ⇌ CO₂(g) + 4 Cu(s) + 2 H₂O(g) K_c = 1.10 A reaction mixture contains 0.22 M CH₄,0.70 M CO₂and 1.5 M H₂O.Which of the following statements is TRUE concerning this system?

Express the equilibrium constant for the following reaction. 2 Na(s) + 2 H₂O(l) ⇌ 2 NaOH(aq) + H₂(g)

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2 IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.35 M I₂,0.31 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?