Question 1

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K? N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)

Accepted Answer

K_p = K_c(RT)^ΔnΔn = 2 - 4 = -2K_c = K_p/(RT)^Δn = 41/(0.0821 × 400)^-2 = 4.4 × 10⁴

Question 2

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[Br₂]_eq = 0.39 M,[HBr]_eq = 1.6 M. H₂(g)+ Br₂(g)⇌ 2 HBr(g)

Accepted Answer

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

Question 3

Express the equilibrium constant for the following reaction. 6 Na(s)+ 6 H₂O(l)⇌ 6 NaOH(aq)+ 3 H₂(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 5.0.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Accepted Answer

The equilibrium constant, K, can be written as:

K = P(isobutane) / P(butane)

At equilibrium, the pressures can be expressed as:

P(butane) = 5.0 - x 
P(isobutane) = x

where x is the change in pressure from the initial state.

Substituting these into the equilibrium expression:

25 = x / (5.0 - x)

Solving for x:

x = 0.165 atm

Therefore, the pressures at equilibrium are:

P(butane) = 5.0 - 0.165 = 0.19 atm 
P(isobutane) = 0.165 atm

Therefore, the best choice is A, which gives the correct pressures for butane and isobutane at equilibrium.

Question 5

Express the equilibrium constant for the following reaction. 5 P₄O₁₀(s)⇌ 5 P₄(s)+ 25 O₂(g)

Accepted Answer

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

Question 6

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

First, we need to use the equilibrium constant expression to find the equilibrium concentration of CO: K_c = [CO₂]² / [CO]²[O₂] Plugging in the given values: 1.4 × 10² = (0.400 mol / 3.00 L)² / [CO]²(0.100 mol / 3.00 L) Rearranging and solving for [CO]: [CO] = (0.400 / 3.00) * sqrt(1.4 × 10² / (0.100 / 3.00)) [CO] = 0.185 mol/L Multiplying by the total volume of the flask: moles of CO = 0.185 mol/L * 3.00 L = 0.555 mol Therefore, the answer is B.

Question 7

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2 I(g)K_p = 0.209 A reaction mixture contains 0.72 atm I₂ and 1.80 atm I.Which of the following statements is TRUE concerning this system?

Accepted Answer

The reaction will shift in the direction of reactants because the reaction quotient (Q) is greater than the equilibrium constant (Kp), indicating that there are too many products relative to reactants.

Question 8

For which reaction will K_p = K_c?

Accepted Answer

For reaction A, the number of moles of gas on both sides of the equation is the same (1 mole of O2 and 1 mole of CO2), so Δn = 0. Therefore, Kp = Kc.

Question 9

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 = 0.11 atm. 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g)

Accepted Answer

The equilibrium constant $K_p$ for the reaction $2 \text{NOCl}(g) \rightleftharpoons 2 \text{NO}(g) + \text{Cl}_2(g)$ is given by the expression $K_p = \frac{P(\text{NO})^2 \cdot P(\text{Cl}_2)}{P(\text{NOCl})^2}$. Substituting the given equilibrium pressures, we get $K_p = \frac{(0.10)^2 \cdot 0.11}{(0.22)^2} = 2.3 \times 10^{-2}$.

Question 10

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 = 0.033 M

Accepted Answer

The equilibrium expression for the given reaction is $K_c = \frac{[NO]^2}{[N_2O_4]}$. Given $K_c = 0.21$ and $[N_2O_4]_{eq} = 0.033 M$, we can solve for $[NO]$ by rearranging the equation to $[NO] = \sqrt{K_c \times [N_2O_4]}$. Substituting the given values, $[NO] = \sqrt{0.21 \times 0.033} = \sqrt{0.00693}$, which is approximately $0.0832 M$ or $8.3 \times 10^{-2} M$.

Question 11

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 200 K? 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g)

Accepted Answer

The answer of The reaction below has a K_c value...

Question 12

At a certain temperature,bromine and nitric oxide react to form nitrosyl bromide: Br₂(g)+ 2 NO(g)⇌ 2 NOBr(g). When initial amounts of Br₂,NO,and NOBr are mixed,the concentration of NOBr increases.Which statement below is TRUE?

Accepted Answer

If the concentration of NOBr is increasing, it means that the reaction quotient Q is less than the equilibrium constant Kc. According to Le Chatelier's principle, the system will shift towards the products to reach equilibrium. Therefore, Kc must be greater than Q for the forward reaction to be favored, which corresponds to choice B.

Question 13

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 SO₂,0.13 M NO_2, 0.11 M SO₃ and 0.13 M NO.Which of the following statements is TRUE concerning this system?

Accepted Answer

The answer of Consider the following reaction and its equilibrium...

Question 14

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 = 2.3 × 10^-3 M

Accepted Answer

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

Question 15

Consider the following reaction and its equilibrium constant: I₂(g)+ Br₂(g)⇌ 2 IBr(g)K_c = 1.1 × 10² A reaction mixture contains 0.37 M I₂,0.30 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Accepted Answer

The answer of Consider the following reaction and its equilibrium...

Question 16

Express the equilibrium constant for the following reaction. RbBrO₃(s)⇌ RbBrO(s)+ O₂(g)

Accepted Answer

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

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]), we can solve for [CO]. Substituting the given values and solving gives [CO] = 8.4 × 10^-4 M.

Question 18

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PBr₅]_eq = 0.56 M,[PBr₃]_eq = 0.23 M,[Br₂]_eq = 6.6 M. PBr₅(g)⇌ PBr₃(g)+ Br₂(g)

Accepted Answer

The equilibrium constant expression for the given reaction is:K_c = [PBr₃][Br₂]/[PBr₅]Substituting the equilibrium concentrations into the expression, we get:K_c = (0.23)(6.6)/0.56 = 2.7Therefore, the value of K_c is 2.7.

Question 19

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 0.20 M CH₄,0.70 M CO₂and 1.5 M H₂O.Which of the following statements is TRUE concerning this system?

Accepted Answer

To determine the direction in which the reaction will shift, we need to compare the reaction quotient (Q) to the equilibrium constant (K). Q = ([CO₂] * [Cu]^4 * [H₂O]^2) / [CH₄]^4 Substituting the given values into the equation, we get: Q = (0.70 * 1.5^2) / 0.20^4 = 109.38 Since Q > K, the reaction will shift in the direction of reactants to reach equilibrium. Therefore, the correct answer is D.

Question 20

Express the equilibrium constant for the following reaction. 2 P₄(s)+ 10 O₂(g)⇌ 2 P₄O₁₀(s)

Accepted Answer

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

Quiz 15: Chemical Equilibrium

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K? N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[Br₂]_eq = 0.39 M,[HBr]_eq = 1.6 M. H₂(g) + Br₂(g) ⇌ 2 HBr(g)

Express the equilibrium constant for the following reaction. 6 Na(s) + 6 H₂O(l) ⇌ 6 NaOH(aq) + 3 H₂(g)

For the isomerization reaction: butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 5.0.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Express the equilibrium constant for the following reaction. 5 P₄O₁₀(s) ⇌ 5 P₄(s) + 25 O₂(g)

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?

Consider the following reaction and its equilibrium constant: I₂(g) ⇌ 2 I(g) K_p = 0.209 A reaction mixture contains 0.72 atm I₂ and 1.80 atm I.Which of the following statements is TRUE concerning this system?

For which reaction will K_p = K_c?

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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

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 = 0.033 M

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 200 K? 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

At a certain temperature,bromine and nitric oxide react to form nitrosyl bromide: Br₂(g) + 2 NO(g) ⇌ 2 NOBr(g) . When initial amounts of Br₂,NO,and NOBr are mixed,the concentration of NOBr increases.Which statement below is TRUE?

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 SO₂,0.13 M NO_2, 0.11 M SO₃ and 0.13 M NO.Which of the following statements is TRUE concerning this system?

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 = 2.3 × 10^-3 M

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2 IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.37 M I₂,0.30 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Express the equilibrium constant for the following reaction. RbBrO₃(s) ⇌ RbBrO(s) + O₂(g)

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?

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PBr₅]_eq = 0.56 M,[PBr₃]_eq = 0.23 M,[Br₂]_eq = 6.6 M. PBr₅(g) ⇌ PBr₃(g) + Br₂(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 0.20 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 P₄(s) + 10 O₂(g) ⇌ 2 P₄O₁₀(s)

Quiz 15: Chemical Equilibrium

The reaction below has a Kp value of 41.What is the value of Kc for this reaction at 400 K? N2(g) + 3 H2(g) ⇌ 2 NH3(g)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M,[Br2]eq = 0.39 M,[HBr]eq = 1.6 M. H2(g) + Br2(g) ⇌ 2 HBr(g)

Express the equilibrium constant for the following reaction. 6 Na(s) + 6 H2O(l) ⇌ 6 NaOH(aq) + 3 H2(g)

For the isomerization reaction: butane ⇌ isobutane Kp equals 25 at 500°C.If the initial pressures of butane and isobutane are 5.0.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Express the equilibrium constant for the following reaction. 5 P4O10(s) ⇌ 5 P4(s) + 25 O2(g)

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?

Consider the following reaction and its equilibrium constant: I2(g) ⇌ 2 I(g) Kp = 0.209 A reaction mixture contains 0.72 atm I2 and 1.80 atm I.Which of the following statements is TRUE concerning this system?

For which reaction will Kp = Kc?

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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)

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 = 0.033 M

The reaction below has a Kc value of 1.0 × 1012.What is the value of Kp for this reaction at 200 K? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

At a certain temperature,bromine and nitric oxide react to form nitrosyl bromide: Br2(g) + 2 NO (g) ⇌ 2 NOBr (g) . When initial amounts of Br2,NO ,and NOBr are mixed,the concentration of NOBr increases.Which statement below is TRUE?

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 SO2,0.13 M NO2, 0.11 M SO3 and 0.13 M NO.Which of the following statements is TRUE concerning this system?

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 = 2.3 × 10-3 M

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 102 A reaction mixture contains 0.37 M I2,0.30 M Br2 and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Express the equilibrium constant for the following reaction. RbBrO3(s) ⇌ RbBrO(s) + O2(g)

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?

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [PBr5]eq = 0.56 M,[PBr3]eq = 0.23 M,[Br2]eq = 6.6 M. PBr5(g) ⇌ PBr3(g) + Br2(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 0.20 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 P4(s) + 10 O2(g) ⇌ 2 P4O10(s)

The reaction below has a K_p value of 41.What is the value of K_c for this reaction at 400 K? N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[Br₂]_eq = 0.39 M,[HBr]_eq = 1.6 M. H₂(g) + Br₂(g) ⇌ 2 HBr(g)

Express the equilibrium constant for the following reaction. 6 Na(s) + 6 H₂O(l) ⇌ 6 NaOH(aq) + 3 H₂(g)

For the isomerization reaction: butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 5.0.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Express the equilibrium constant for the following reaction. 5 P₄O₁₀(s) ⇌ 5 P₄(s) + 25 O₂(g)

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?

Consider the following reaction and its equilibrium constant: I₂(g) ⇌ 2 I(g) K_p = 0.209 A reaction mixture contains 0.72 atm I₂ and 1.80 atm I.Which of the following statements is TRUE concerning this system?

For which reaction will K_p = K_c?

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 = 0.11 atm. 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g)

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 = 0.033 M

The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 200 K? 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

At a certain temperature,bromine and nitric oxide react to form nitrosyl bromide: Br₂(g) + 2 NO(g) ⇌ 2 NOBr(g) . When initial amounts of Br₂,NO,and NOBr are mixed,the concentration of NOBr increases.Which statement below is TRUE?

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 SO₂,0.13 M NO_2, 0.11 M SO₃ and 0.13 M NO.Which of the following statements is TRUE concerning this system?

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 = 2.3 × 10^-3 M

Consider the following reaction and its equilibrium constant: I₂(g) + Br₂(g) ⇌ 2 IBr(g) K_c = 1.1 × 10² A reaction mixture contains 0.37 M I₂,0.30 M Br₂and 3.5 M IBr.Which of the following statements is TRUE concerning this system?

Express the equilibrium constant for the following reaction. RbBrO₃(s) ⇌ RbBrO(s) + O₂(g)

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?

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PBr₅]_eq = 0.56 M,[PBr₃]_eq = 0.23 M,[Br₂]_eq = 6.6 M. PBr₅(g) ⇌ PBr₃(g) + Br₂(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 0.20 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 P₄(s) + 10 O₂(g) ⇌ 2 P₄O₁₀(s)