Question 1

Consider the equilibrium reaction: H₂(g) + Br₂(g) ⇄ 2HBr(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

Accepted Answer

The relationship between $K_p$ and $K_c$ for a reaction is given by the equation $K_p = K_c(RT)^{\Delta n}$, where $\Delta n$ is the change in moles of gas between products and reactants. For the given reaction, $\Delta n = 0$ (2 moles of gas on both sides), so $K_p = K_c$.

Question 2

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) ⇄ 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) ⇄ ½Br₂(g) + ½Cl₂(g)

Accepted Answer

The answer of The equilibrium constant for the reaction of...

Question 3

About half of the sodium carbonate produced is used in making glass products because it lowers the melting point of sand, the major component of glass. When sodium carbonate is added to water it hydrolyses according to the following reactions. CO₃²⁻(aq) + H₂O(l) ⇄ HCO₃⁻(aq) + OH⁻(aq) K₁ HCO₃(aq) + H₂O(l) ⇄ H₂CO₃(aq) + OH⁻(aq) K₂ These can be combined to yield CO₃²⁻(aq) + 2H₂O(l) ⇄ H₂CO₃(aq) + 2OH⁻(aq) K₃ What is the value of K₃?

Accepted Answer

The combined equilibrium constant for a reaction that is the sum of two reactions is the product of the equilibrium constants of those two reactions.

Question 4

At 500°C the equilibrium constant, K_p, is 4.00 × 10⁻⁴ for the equilibrium: 2HCN(g) ⇄ H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂N₂(g) ⇄ 2HCN(g)

Accepted Answer

The answer of At 500°C the equilibrium constant, K_p, is...

Question 5

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2)? (1) ½X₂(g) + ½Y₂(g) ⇄ XY(g) (2) 2XY(g) ⇄ X₂(g) + Y₂(g)

Accepted Answer

The answer of The equilibrium constant for reaction (1) below...

Question 6

In water, the following equilibrium exists: H⁺(aq) + OH⁻(aq) ⇄ H₂O(l) In pure water at 25°C, the concentration of H⁺ ions is 1.00 × 10⁻⁷ mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

Accepted Answer

The equilibrium constant for the reaction is calculated using the concentrations of the products and reactants at equilibrium. Given that the concentration of $H^+$ ions is $1.00 \times 10^{-7}$ mol/L in pure water at 25°C, and knowing that water self-ionizes to produce equal concentrations of $H^+$ and $OH^-$ ions, the concentration of $OH^-$ ions is also $1.00 \times 10^{-7}$ mol/L. The equilibrium constant ($K$) for the reaction is the product of the concentrations of the reactants raised to their stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients. Since water ($H_2O$) is a pure liquid, its concentration does not appear in the expression for $K$. Therefore, $K = [H^+][OH^-] = (1.00 \times 10^{-7})(1.00 \times 10^{-7}) = 1.00 \times 10^{-14}$.

Question 7

N₂(g) + O₂(g) ⇄ 2NO(g) K_c = 4.8 × 10⁻³¹ 2NOBr(g) ⇄ 2NO(g) + Br₂(g) K_c = 0.50 Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction 2NOBr(g) ⇄ N₂(g) + O₂(g) + Br₂(g)?

Accepted Answer

The answer of N₂(g) + O₂(g) ⇄ 2NO(g) K_c =...

Question 8

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) ⇄ 2NOBr(g)

Accepted Answer

The answer of Nitric oxide and bromine were allowed to...

Question 9

The equilibrium constant, K_p, for the reaction H₂(g) + I₂(g) ⇄ 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

Accepted Answer

To determine if the system is at equilibrium, calculate the reaction quotient, $Q_c$, and compare it to the equilibrium constant, $K_c$. For the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$, $Q_c = \frac{[HI]^2}{[H_2][I_2]}$. Given: $[HI] = 1.055 \, \text{atm}$, $[H_2] = 0.127 \, \text{atm}$, $[I_2] = 0.134 \, \text{atm}$, and $K_c = 55.2$. Calculating $Q_c$ gives $Q_c = \frac{(1.055)^2}{(0.127)(0.134)} = 61.4$, which is greater than $K_c$. This means the system is not at equilibrium, and the reverse reaction must proceed to decrease $Q_c$ to the value of $K_c$.

Question 10

The equilibrium constant, K_p, has a value of 6.5 × 10⁻⁴ at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) ⇄ 2NOCl(g) What is the value of K_c?

Accepted Answer

The equilibrium constant, K, is defined as: K = [products]^m/[reactants]^n where m and n are the stoichiometric coefficients of the products and reactants, respectively. In this case, the equilibrium constant (K_p) is given as: K_p = [NOCl]^2/([NO]^2[Cl₂]) To calculate the value of the equilibrium constant in terms of concentrations (K_c), we need to use the equation: K = KPRT^(Δn) where KP is the equilibrium constant in terms of partial pressures, R is the gas constant, T is the temperature in Kelvin, and Δn is the difference in moles of gas products and reactants (moles of products - moles of reactants). In this case, Δn = (2 moles of NOCl) - (2 moles of NO + 1 mole of Cl₂) = 0, since the number of moles of gas on either side of the equation is equal. Thus, the equation becomes: K = KPRT^(0) K = KP K_c = KP To convert from KP to KC, we need to use the equation: KP = KC(RT)^(Δn) Rearranging this equation gives: KC = KP/(RT)^(Δn) Plugging in the values for KP and Δn, we get: KC = K_p/(RT)^(Δn) Plugging in the given values and solving, we get: KC = 6.5 × 10^-14/[(0.0821 L·atm/K·mol)(308 K)]^0 KC = 1.6 × 10^-12 Therefore, the correct answer is C) 1.6 × 10^-12.

Question 11

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) ⇄ 2NO(g) + O₂(g) Where K_p = 4.48 × 10⁻¹³ at 25°C. What is the value for K_c?

Accepted Answer

The equilibrium constant expression for this reaction is:
K = [NO]^2[O2]/[NO2]^2
We can convert this to the given equilibrium constant expression using the relationship:
ΔG° = -RTln(K)
ΔG° = -RTln(4.48 × 10^-13) = 17030 J/mol
ΔG° = -RTln(Kc)
-17030 J/mol = -(8.314 J/mol*K)(298 K)ln(Kc)
ln(Kc) = 2.051
Kc = e^(2.051) = 7.78 × 10^0 = 1.83 × 10^-1^4

Question 12

Write the mass-action expression, Q_c, for the following chemical reaction. Sn²⁺(aq) + ½O₂(g) + 3H₂O(l) ⇄ SnO₂(s) + 2H₃O⁺(aq)

Accepted Answer

The answer of Write the mass-action expression, Q_c, for the...

Question 13

Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l) ⇄ H₃O⁺(aq) + HS⁻(aq) K₁= 1.0 × 10⁻⁷ HS⁻(aq) + H₂O(l) ⇄ H₃O⁺(aq) + S²⁻(aq) K₂= ? H₂S(g) + 2H₂O(l) ⇄ 2H₃O⁺(aq) + S²⁻(aq) K₃= 1.3 × 10⁻²⁰ What is the value of K₂?

Accepted Answer

The equilibrium constant K2 can be found by dividing K3 by K1, as K3 is the product of K1 and K2. Therefore, K2 = K3 / K1 = (1.3 × 10^−20) / (1.0 × 10^−7) = 1.3 × 10^−13.

Question 14

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O₂(g) ⇄ NO₂(g) (2) 2NO₂(g) ⇄ 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

Accepted Answer

Equilibrium (2) is the reverse of equilibrium (1) but doubled. Therefore, the equilibrium constant for (2), $K_{2}$, is the reciprocal of the square of the equilibrium constant for (1), $K_{1}$, i.e., $K_{2} = (1/K_{1})^2$.

Question 15

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) ⇄ 2NO(g) At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10⁻⁴. What is the value of K_p?

Accepted Answer

The equilibrium constant, Kc, is related to the equilibrium constant, Kp, by the equation Kp = Kc(RT)Δn, where Δn is the difference in the number of moles of gaseous products and gaseous reactants. In this case, Δn = 2 - 1 - 1 = 0, because there is one mole of nitrogen and one mole of oxygen on each side of the equation, and two moles of nitrogen monoxide. Since Δn = 0, Kp = Kc. Therefore, the value of Kp is 4.10 × 10^-14, which is the same as the value of Kc given in the problem. Hence, the answer is B.

Question 16

The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Accepted Answer

The answer of The equilibrium constant, K_p, for the reaction...

Question 17

H₂SO₃(aq) ⇄ HSO₃(aq) + H⁺(aq) K_c = 1.4 × 10⁻² H₂SO₃(aq) ⇄ SO₃²⁻(aq) + 2H⁺(aq) K_c = 9.1 × 10⁻¹⁰ Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction HSO₃⁻(aq) ⇄ SO₃²⁻(aq) + H⁺(aq)?

Accepted Answer

The equilibrium constant for the reaction HSO₃⁻(aq) ⇄ SO₃²⁻(aq) + H⁺(aq) can be obtained by dividing the equilibrium constant for the second reaction by the equilibrium constant for the first reaction.K_c = (9.1 × 10⁻¹⁰) / (1.4 × 10⁻²) = 6.5 × 10⁻⁸

Question 18

Consider the reactions of cadmium with the thiosulfate anion. Cd²⁺(aq) + S₂O₃²⁻(aq) ⇄ Cd(S₂O₃)(aq) K₁ = 8.3 × 10³ Cd(S₂O₃)(aq) + S₂O₃²⁻(aq) ⇄ Cd(S₂O₃)₂²⁻(aq) K₂= 2.5 × 10² What is the value for the equilibrium constant for the following reaction? Cd²⁺(aq) + 2S₂O₃²⁻(aq) ⇄ Cd(S₂O₃)₂²⁻(aq)

Accepted Answer

The equilibrium constant for the overall reaction is the product of the equilibrium constants for the individual steps: K = K1 * K2 = (8.3 × 10^3) * (2.5 × 10^2) = 2.075 × 10^6, which is approximately 2.1 × 10^6.

Question 19

Consider the equilibrium reaction: N₂O₄(g) ⇄ 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

Accepted Answer

K_p = RT × K_cThe equilibrium constant K_p is related to the equilibrium constant K_c by the equation K_p = RT × K_c, where R is the ideal gas constant and T is the temperature in Kelvin.

Question 20

The equilibrium constant, K_c, for the decomposition of COBr₂ COBr₂(g) ⇄ CO(g) + Br₂(g) Is 0.190. What is K_c for the following reaction? 2CO(g) + 2Br₂(g) ⇄ 2COBr₂(g)

Accepted Answer

The equilibrium constant for the reverse reaction is the reciprocal of the given equilibrium constant, and for the reaction with coefficients doubled, it is the square of the reciprocal. Given K = 0.190 for COBr2 ⇄ CO + Br2, the K for the reverse reaction is 1/0.190. For 2CO + 2Br2 ⇄ 2COBr2, it's (1/0.190)^2 = 27.7.

Quiz 17: Equilibrium: the Extent of Chemical Reactions

Consider the equilibrium reaction: H₂(g) + Br₂(g) ⇄ 2HBr(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) ⇄ 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) ⇄ ½Br₂(g) + ½Cl₂(g)

At 500°C the equilibrium constant, K_p, is 4.00 × 10⁻⁴ for the equilibrium: 2HCN(g) ⇄ H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂N₂(g) ⇄ 2HCN(g)

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) ½X₂(g) + ½Y₂(g) ⇄ XY(g) (2) 2XY(g) ⇄ X₂(g) + Y₂(g)

In water, the following equilibrium exists: H⁺(aq) + OH⁻(aq) ⇄ H₂O(l) In pure water at 25°C, the concentration of H⁺ ions is 1.00 × 10⁻⁷ mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

N₂(g) + O₂(g) ⇄ 2NO(g) K_c = 4.8 × 10⁻³¹ 2NOBr(g) ⇄ 2NO(g) + Br₂(g) K_c = 0.50 Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction 2NOBr(g) ⇄ N₂(g) + O₂(g) + Br₂(g) ?

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) ⇄ 2NOBr(g)

The equilibrium constant, K_p, for the reaction H₂(g) + I₂(g) ⇄ 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

The equilibrium constant, K_p, has a value of 6.5 × 10⁻⁴ at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) ⇄ 2NOCl(g) What is the value of K_c?

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) ⇄ 2NO(g) + O₂(g) Where K_p = 4.48 × 10⁻¹³ at 25°C. What is the value for K_c?

Write the mass-action expression, Q_c, for the following chemical reaction. Sn²⁺(aq) + ½O₂(g) + 3H₂O(l) ⇄ SnO₂(s) + 2H₃O⁺(aq)

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O₂(g) ⇄ NO₂(g) (2) 2NO₂(g) ⇄ 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) ⇄ 2NO(g) At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10⁻⁴. What is the value of K_p?

The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

H₂SO₃(aq) ⇄ HSO₃(aq) + H⁺(aq) K_c = 1.4 × 10⁻² H₂SO₃(aq) ⇄ SO₃²⁻(aq) + 2H⁺(aq) K_c = 9.1 × 10⁻¹⁰ Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction HSO₃⁻(aq) ⇄ SO₃²⁻(aq) + H⁺(aq) ?

Consider the equilibrium reaction: N₂O₄(g) ⇄ 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

The equilibrium constant, K_c, for the decomposition of COBr₂ COBr₂(g) ⇄ CO(g) + Br₂(g) Is 0.190. What is K_c for the following reaction? 2CO(g) + 2Br₂(g) ⇄ 2COBr₂(g)

Quiz 17: Equilibrium: the Extent of Chemical Reactions

Consider the equilibrium reaction: H2(g) + Br2(g) ⇄ 2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) ⇄ 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) ⇄ ½Br2(g) + ½Cl2(g)

At 500°C the equilibrium constant, Kp, is 4.00 × 10−4 for the equilibrium: 2HCN(g) ⇄ H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2N2(g) ⇄ 2HCN(g)

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) ½X2(g) + ½Y2(g) ⇄ XY(g) (2) 2XY(g) ⇄ X2(g) + Y2(g)

In water, the following equilibrium exists: H+(aq) + OH−(aq) ⇄ H2O(l) In pure water at 25°C, the concentration of H+ ions is 1.00 × 10−7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

N2(g) + O2(g) ⇄ 2NO(g) Kc = 4.8 × 10−31 2NOBr(g) ⇄ 2NO(g) + Br2(g) Kc = 0.50 Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction 2NOBr(g) ⇄ N2(g) + O2(g) + Br2(g) ?

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. 2NO(g) + Br2(g) ⇄ 2NOBr(g)

The equilibrium constant, Kp, for the reaction H2(g) + I2(g) ⇄ 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

The equilibrium constant, Kp, has a value of 6.5 × 10−4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) ⇄ 2NOCl(g) What is the value of Kc?

Nitrogen dioxide decomposes according to the reaction 2NO2(g) ⇄ 2NO(g) + O2(g) Where Kp = 4.48 × 10−13 at 25°C. What is the value for Kc?

Write the mass-action expression, Qc, for the following chemical reaction. Sn2+(aq) + ½O2(g) + 3H2O(l) ⇄ SnO2(s) + 2H3O+(aq)

Hydrogen sulfide will react with water as shown in the following reactions. H2S(g) + H2O(l) ⇄ H3O+(aq) + HS−(aq) K1 = 1.0 × 10−7 HS−(aq) + H2O(l) ⇄ H3O+(aq) + S2−(aq) K2 = ? H2S(g) + 2H2O(l) ⇄ 2H3O+(aq) + S2−(aq) K3 = 1.3 × 10−20 What is the value of K2?

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) ⇄ NO2(g) (2) 2NO2(g) ⇄ 2NO(g) + O2(g) Which one of the following is the correct relationship between the equilibrium constants K1 and K2?

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) ⇄ 2NO(g) At 2000°C, the equilibrium constant, Kc, has a value of 4.10 × 10−4. What is the value of Kp?

The equilibrium constant, Kp, for the reaction CO(g) + H2O(g) ⇄ CO2(g) + H2(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

H2SO3(aq) ⇄ HSO3(aq) + H+(aq) Kc = 1.4 × 10−2 H2SO3(aq) ⇄ SO32−(aq) + 2H+(aq) Kc = 9.1 × 10−10 Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction HSO3−(aq) ⇄ SO32−(aq) + H+(aq) ?

Consider the equilibrium reaction: N2O4(g) ⇄ 2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?

The equilibrium constant, Kc, for the decomposition of COBr2 COBr2(g) ⇄ CO(g) + Br2(g) Is 0.190. What is Kc for the following reaction? 2CO(g) + 2Br2(g) ⇄ 2COBr2(g)

Consider the equilibrium reaction: H₂(g) + Br₂(g) ⇄ 2HBr(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) ⇄ 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) ⇄ ½Br₂(g) + ½Cl₂(g)

At 500°C the equilibrium constant, K_p, is 4.00 × 10⁻⁴ for the equilibrium: 2HCN(g) ⇄ H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂N₂(g) ⇄ 2HCN(g)

The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2) ? (1) ½X₂(g) + ½Y₂(g) ⇄ XY(g) (2) 2XY(g) ⇄ X₂(g) + Y₂(g)

In water, the following equilibrium exists: H⁺(aq) + OH⁻(aq) ⇄ H₂O(l) In pure water at 25°C, the concentration of H⁺ ions is 1.00 × 10⁻⁷ mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

N₂(g) + O₂(g) ⇄ 2NO(g) K_c = 4.8 × 10⁻³¹ 2NOBr(g) ⇄ 2NO(g) + Br₂(g) K_c = 0.50 Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction 2NOBr(g) ⇄ N₂(g) + O₂(g) + Br₂(g) ?

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction. 2NO(g) + Br₂(g) ⇄ 2NOBr(g)

The equilibrium constant, K_p, for the reaction H₂(g) + I₂(g) ⇄ 2HI(g) Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

The equilibrium constant, K_p, has a value of 6.5 × 10⁻⁴ at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) ⇄ 2NOCl(g) What is the value of K_c?

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) ⇄ 2NO(g) + O₂(g) Where K_p = 4.48 × 10⁻¹³ at 25°C. What is the value for K_c?

Write the mass-action expression, Q_c, for the following chemical reaction. Sn²⁺(aq) + ½O₂(g) + 3H₂O(l) ⇄ SnO₂(s) + 2H₃O⁺(aq)

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O₂(g) ⇄ NO₂(g) (2) 2NO₂(g) ⇄ 2NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) ⇄ 2NO(g) At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10⁻⁴. What is the value of K_p?

The equilibrium constant, K_p, for the reaction CO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

H₂SO₃(aq) ⇄ HSO₃(aq) + H⁺(aq) K_c = 1.4 × 10⁻² H₂SO₃(aq) ⇄ SO₃²⁻(aq) + 2H⁺(aq) K_c = 9.1 × 10⁻¹⁰ Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction HSO₃⁻(aq) ⇄ SO₃²⁻(aq) + H⁺(aq) ?

Consider the equilibrium reaction: N₂O₄(g) ⇄ 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_p for the reaction?

The equilibrium constant, K_c, for the decomposition of COBr₂ COBr₂(g) ⇄ CO(g) + Br₂(g) Is 0.190. What is K_c for the following reaction? 2CO(g) + 2Br₂(g) ⇄ 2COBr₂(g)