Equilibrium Questions and Answers

What quantity in moles of will be formed when precipitate 100.0 mL of 2.00 M Nal is reacted with 80.0 mL of 0.900 M Pb(NO3)2 in the following chemical reaction? 2 Nal(aq) + Pb(NO3)2(aq) → Pbl₂(s) + 2 NaNO3(aq)

Select one answer. 7 points Will a solution of (CH₂)₂NHBr be basic, acidic, or neutral? Use Ionization Constants of Common Weak Acids and Ionization Constants of Common Weak Bases as needed. A. O acidic B. basic C. O neutral

Will a solution of Na₂SO, be basic, acidic, or neutral? Select one answer. A. O acidic B. basic C. O neutral 7 points Use Ionization Constants of Common Weak Acids and Ionization Constants of Common Weak Bases as needed.

When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 15.6 g of carbon were burned in the presence of 54.7 g of oxygen, 13.1 g of oxygen remained unreacted. What mass of carbon dioxide was produced? Express your answer to one decimal place and include the appropriate units.

(a salt formed with the Ni and the hydroxide anion will Double replacement: NiCl₂ (aq) + NaOH(aq)→ usually precipitate, while all salts formed with the chloride ion remain aqueous)

In a solution of 0.100 M hypoiodious acid, what species is in the highest concentration? A. hydronium ion B. hypoiodite ion C. hydroxide ion D. hypoiodious acid

A solution is prepared at 25 °C that is initially 0.23 M in benzoic acid (HC, H,CO₂), a weak acid with K, -6.3x10^-5, and 0.27 M in sodium benzoate (NaC, H, CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places.

A solution is prepared at 25 °C that is initially 0.11 M in chloroacetic acid (HCH2CICO₂), a weak acid with K=1.3x10^-3, and 0.0046 M in potassium chloroacetate (KCH2CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places.

Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 5.0 L flask with 4.6 atm of methane gas and 4.9 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 5.5 atm, Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits.

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 50.0 L tank with 2.8 mol of sulfur dioxide gas and 5.0 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 1.4 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits.

Sulfurous acid (H₂SO₂) is a polyprotic acid. Write balanced chemical equations for the sequence of reactions that sulfurous acid can undergo when it's dissolved in water. H₂SO, (aq) + H₂O(1)→ HSO, (aq) + H₂O* (aq) HSO (aq) + H₂O (aq) → H₂SO, (aq) + H₂O(1) HSO (aq) + H₂O(1) So, (aq) + H₂O (aq) so (aq) + H₂O (aq) → HSO, (aq) + H₂O(1)

While ethanol (CH, CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 5.0 L flask with 3.6 atm of ethylene gas and 4.4 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.3 atm of ethylene gas and 2.1 atm of water vapor. The engineer then adds another 1.8 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm ,

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 125. L tank with 12. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 4.2 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. ?

The density of silver is 10.5 g/cm³. The material measure has a length of 75 cm and a height of 28 cm. It has a mass of exactly 95.36 g. What is the volume of the material?

Suppose a 500. mL flask is filled with 1.0 mol of 12 and 1.5 mol of HI. The following reaction becomes possible: H₂(g) +I₂(g) -> 2HI(g) The equilibrium constant K for this reaction is 7.40 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places.

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 5.0 L flask with 4.1 atm of ammonia gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 3.7 atm, Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

A 4.3 g rock sample is added to a graduated cylinder filled with water, causing the level to increase from 10.3 mL to 12.4 mL. What is the density of the rock sample? Select the correct answer below: 1.7 g/mL 1.4 g/mL 2.0 g/mL 2.7 g/mL

The solubility of PbSO, in water at 25 °C is 7.9 x 104 M. What is Ksp for PbSO,?

An acid HX has a [H] = 5.7 x 104 M. The pKa of the acid must be, given that 10.0 g of the acid is dissolved to make 250.0 mL of solution. Assume the mol. wt of HX is 81.07 g/mol. (a) 5.7 x 10^-4 (b) 3.25 x 10^-8 (c) 6.18 (d) 6.59 x 10^-7 (e) None

Convert each H30+ concentration to a pH value. a. 6.5 × 10-5 M b. 8.03 x 10-8 M

Will a precipitate form when 20.0 mL of 1.8 x 10^-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 x 10-4 M Na2SO4? The Ksp of PbSO4 is 6.3 × 10^-7. No, because Ksp equals the ion product No, because the ion product, Q< Ksp Yes, because the ion product, Q> Ksp Yes, because the ion product, Q< Ksp No, because the ion product, Q> Ksp

An equilibrium is established for the endothermic reaction 2 CO(g) + MoO₂ (s) -> 2CO₂(g) + MoO2(s). How would each of the following changes affect the partial pressure of carbon dioxide at equilibrium? Adding Mo. A) The partial pressure increases. B) The partial pressure decreases. C) The partial pressure does not change.

The Kc = 1.7 x 10-3 at 2300 K for the reaction N2(g) + O2(g) = 2NO(g). a) What is the value of K. for the reaction at 2300 K? 1/2 N2(g) + 1/2 O2(g) → NO(g) b) What is the value of Ke for the reaction at 2300 K? 4NO(g) = 2N2(g) + 2O2(g)

Consider the reaction: 2 NO2 (g) -> N₂O4 (g) At equilibrium, the partial pressures of N₂O4 and NO₂ are 0.35 atm and 4.3 atm, respectively. What is Kp?

A solution is prepared at 25 °C that is initially 0.43 M in dimethylamine ((CH3)2NH), a weak base with Kb = 5.4 × 10^-4, and 0.012M in dimethylammonium bromide ((CH3)2NH₂ Br). Calculate the pH of the solution. Round your answer to 2 decimal places. -4

On analysis, an equilibrium mixture for the reaction 2H₂S(g) = 2H2(g) + S2(g) was found to contain 0.70 mol H₂S, 1.0 mol H₂, and 0.35 mol S2 in a 2.0 L vessel. Calculate the equilibrium constant, Ke, for this reaction.

Consider the reaction: 2 HI (g) = H₂ (g) + 12 (g) Kc = 7.21 If at equilibrium the reaction vessel contains 1.20 M of H₂ and 1.70 M 12, then what is the equilibrium concentration of HI?

CO₂ can react with OH", forming HCO3. In this reaction, A. the CO₂ acts as a Brønsted acid, accepting a proton from the OH ion. B. the CO₂ acts as a Lewis acid, accepting a proton from the OH ion. C. the OH ion acts as a Brønsted base, donating a proton to the CO2 molecule. D. the OH ion acts as a Lewis acid, accepting an electron pair from the CO2 molecule to form a coordinate covalent bond. E. the OH ion acts as a Lewis base, donating an electron pair to the CO2 molecule to form a coordinate covalent bond. A B C D E

Consider the reaction below: 2 CO(g) + O₂(g) = 2 CO₂(g) If Kc is 2.24 x 1022 at 1273.0°C, calculate Kp at the same temperature. (R = 0.08206 L'atm/mol K.)

Kingsley then adds 42.99 mL of NaOH to 250.00 mL of the HCOOH solution. The neutralization reaction resulted in 0.099 moles of HCOOH and 0.025 moles of HCOO left in solution. Determine the pH of the resulting solution. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.

The K, for an amine is 4.955 x 10-5. What percentage of the amine is protonated if the pH of a solution of the amine is 9.564? Assume that all OH came from the reaction of B with H₂O.

Write the equilibrium constant for the following reversible reactions.(4 points per equation 12 points total) a. CO₂ (g) + C(s) → 2 CO (g) b. 2 SO 3 (g) → 2 SO₂ (g) + O₂(g) c. Mn2+ (aq) + Cl₂(g) + 2 H₂O (1) MnO₂ (s) + 4 H+ (aq) + 2 Cl- (aq)

Classify each of these solids as ionic, molecular, metallic, or covalent (also known as covalent-network solids ormacromolecular solids). Ionic Molecular Metallic Covalent Answer Bank CaCl2 Mg CCL4 C(diamond)

An analytical chemist is titrating 210.3 ml. of a 0.2400 M solution of benzoic acid (HC6H5CO₂) with a 0.9700 M solution of KOH. The PK, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 41.95 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added.

Fe3O4(s) reacts with H₂(g) to form Fe(s) and H₂O(g) according to the following equation. Fe3O4(s) + 4H₂(g) + 36.1 kcal- →3Fe(s) + 4H₂O(g) Is this reaction endothermic or exothermic? Is energy evolved or absorbed when the reaction takes place? How many kcal of energy is this when 1.54 mol of Fe3O4(s) reacts?

Nickel carbonyl decomposes to form nickel and carbon monoxide, like this: Ni (CO)4⇒ (9) Ni(s) +4 CO(g) At a certain temperature, a chemist finds that a 6.8 L reaction vessel containing a mixture of nickel carbonyl, nickel, and carbon monoxide at equilibrium has the following composition: compound amount Ni (CO), 0.134 g Ni 33.0 g CO 1.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Consider the following chemical equilibrium: 2 PbO (s) + O₂ (g)⇒ 2 PbO₂ (s) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature 7. You can assume Tis comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS calculator

What volume of 0.150 M Na3PO4 is required to precipitate all the lead(II) ions from 100.0 mL of 0.400 M Pb(NO3)2? Volume = mL

A solution of 0.235 M KOH is used to titrate 20.0 mL of a 0.187 M H3PO4 solution. What volume, in milliliters, of the KOH solution is required? H3PO4 (aq) + 3KOH(aq) → 3H₂O(1) + K3PO4 (aq) Express your answer with the appropriate units. Volume =

Suppose a 250 mL flask is filled with mol of Bf2, 1.8 mol of BrOCI and 1.1 mol of BrCI. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrC1 (g) The equilibrium constant K for this reaction is 0.327 at the temperature of the flask. Calculate the equilibrium molarity of BrOCI, Round your answer to two decimal places.

Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 25.0 L tank with 7.8 mol of methane gas and 9.8 mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 4.7 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits.

Suppose a 250. mL flask is filled with 1.9 mol of Br₂, 1.8 mol of BrOCI and 1.1 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) BrOCI(g) + BrC1 (g) The equilibrium constant K for this reaction is 0.327 at the temperature of the flask. Calculate the equilibrium molarity of BrOCI. Round your answer to two decimal places.

70 mL of 0.1 M HCI (aq.) is titrated against 0.2 M _K₂Cr₂O7 (aq.) solution to form CrCl3, Cl₂ and KCI. Select the correct options : Required volume of K₂Cr₂O7 to titrate HCI completely will be 35/6 mL. Moles of Cl₂ formed during reaction is 1.5 × 10–³ Equivalent mass of CrCl3 is (M = Equivalent mass of Cl₂ is.

Which one describes the ionization of a strong acid in water? HCl(aq)- →H+(aq) + Cl-(aq) KOH(aq) + HCl(aq) → KCl(aq) + H₂O(l) BaCO3(aq) → Ba²+ (aq) + CO3²- (aq) NaNO3(aq) → Na*(aq) + NO3(aq)

The reaction CH,OH (9) ⇒CO(g) + 2 H₂ (9) occurs in a closed reaction vessel at constant volume and temperature. Initially, the vessel contains only CH,OH at a pressure of 1.55 atm. After the reaction reaches equilibrium, the total pressure is 2.95 atm. What is the value of the equilibrium constant, Kp. for the reaction?

A chunk of NaCl is added to a solution until it is saturated. The concentration of Nat ions is found to be 0.050mol/L and the concentration of Cl ions is found to be 0.030mol/L. What is the equilibrium constant. Answer to 5 decimal places. Do not include units

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °C is kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H₂O, AHfus = 6.01 kJ/mol, and Hvap = 40.67 kJ/mol.

Write the complete molecular, ionic, and net ionic equations for the reaction between Pb(NO3)2 and MgCl₂. Balance all equations and include phases for all substances.

Determine equilibrium constant for the following reaction under standard state. A (g) + B (g) --- C (g) + 1.90 kj the standard entropy change for the reaction is - 10 J/k. A.0.717 B, 7.17 C. 1.55 D,0.647 E, 0.140

Determine standard free energy change for the reaction: NO₂ (aq) + H₂(1) ------ HNO₂ (aq) + OH (aq) The ionization constant for HNO₂ is 3.65 x 10-5 at 25 °C. 25316 J/mol 25316 J/mol 54551 J/mol 48658 J/mol 249.84 J/mol