chem final 2

Calculate the pH of a buffer solution that is 0.229 M HC2H3O2 and 0.29 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10-5. Hint: you can use the Henderson-Hasselbalch equation. -Type your numerical answer using three significant figures. HC2H3O2(s)+H2O(l)⟶H3O+(aq)+C2H3O2−(aq)

4.85

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C. 6.4 × 10-7 M 1.9× 10-12 M 5.4 × 10-2 M 9.5× 10-3 M 5.7 × 10-11 M

1.9× 10-12 M

What are the units of k in the following rate law?Rate = k[X] Ms M/s 1/s s/M M^-1s^-1

1/s

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water. The vapor pressure of pure water at 55°C is 118.1 torr. The van't Hoff factor for NaCl is 1.9. 108 torr 115 torr 92.8 torr 112 torr 87.1 torr 0.25 torr

112 torr

A body-centered cubic unit cell has a volume of 2.27 x 10-23 cm3. Find the radius of the atom in pm. Note: when you get your answer, type the number only and round your final answer to four significant figures.

122.6

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [P4O10]eq = 51.11 M, [P4]eq = 2.08 M, [O2]eq = 1.987 M.P4O10(s) ⇌ P4(s) + 5 O2(g)

30.973

The rate constant for the rate of decomposition of a novel organic compound in the gas phase is 1.68 L/mol-s at 558 K and 7.39 L/mol-s at 700 K. Assuming the kinetics of this reaction are consistent with the Arrhenius equation, calculate the activation energy (Ea), in kilojoules, for this decomposition. Remember that R = 8.314 J mol-1K-1 and report your answer using three significant figures.

33.9

Calculate the pH of a 0.724 M solution of the weak hydrocyanic acid. -Assume that the x value is very small. -Round your answer to three significant figures. Ka = 6.2 X 10-10 HCN(aq)+H2O(l)⇋H3O+(aq)+CN−(aq)

4.67

Express the equilibrium constant for the following reaction. 10 NH3(g) ⇔ 5 N2(g) + 15 H2(g) K = [N2][H2]^1/3 /[NH3]^1/2 K = [NH3]/ [N2]^2 [H2]^3 K = [N2]^5[H2]^15 /[NH3]^10 K = [NH3]^1/2 /[N2][H3]^1/3 K = [NH3]^10 /[N2]^5[H3]^15

K = [N2]^5[H2]^15 /[NH3]^10

Which of the following processes have a ΔS > 0? CH4(g) + H2O(g) → CO(g) + 3 H2(g) CH3OH(l) → CH3OH(s) N2(g) + 3 H2(g) → 2 NH3(g) Na2CO3(s) + H2O(g) + CO2(g) → 2 NaHCO3(s) All of the above processes have a DS > 0.

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

Which of the following bases is the strongest? The base is followed by its Kb. C5H5N, 1.7 × 10-9 NH3, 1.76 × 10-5 (CH3CH2)2NH, 8.6 × 10-4 CH3NH2, 4.4 × 10-4 C6H5NH2, 4.0 × 10-10

(CH3CH2)2NH, 8.6 × 10-4

Give the characteristic of a first order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant.

(The rate of the reaction is not proportional to the concentration of the reactant.)---WRONG CORRECT___

Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction.4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) S°(J/mol∙K)192.8205.2210.8188.8 +160.0 J/K +287.4 J/K -401.2 J/K +178.8 J/K -336.6 J/K

+178.8 J/K

Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g)ΔH°= +1.9 kJ; ΔS°= -109.6 J/K +57.7 kJ +17.3 kJ -41.5 kJ -30.8 kJ +34.6 kJ

+34.6 kJ

Consider the phase diagram shown. What is the normal sublimation point at 1 atm? 0°C 100°C -56.7 °C 31°C -78.5 °C

-78.5 °C

The rate constant for the first-order decomposition of N2O is 2.053 s-1. What is the half-life of the decomposition?

0.338

What is the solubility, in g/L, of PbF2 in water? The Ksp for PbF2 is 2.7 x 10-8? PbF2(s)⇋Pb2+(aq)+2F−(aq)

0.46 WRONG?

Calculate the pH of the following acid in water knowing that its concentration is 0.39 M and its Ka = 0.75. -You might need to use the quadratic equation. -Round your numerical answer to two decimals. HA(aq)+H2O(l)⇌H3O(aq)+ + A(aq)−

0.55

Determine the pH of a 0.116 M HNO3 solution. -Consider HNO3 to be a strong acid. -Round your answer to two significant figures.

0.94

The normal boiling point of a newly discovered solvent at 760 mmHg is 34.5o C. Estimate, in mmHg, its vapor pressure at 73.2o C. This new solvent has a heat of vaporization of 10.0 kJ/mol. Remember that R = 8.31 J/(K-mol). Note: when you get your answer, type the number only and round your final answer to four significant figures.

1,177

Write a balanced reaction for which the following rate relationships are TRUE.Rate = -1/2 delta[N2O5]/delta t = 1/4 delta[NO2]/delta t = delta[O2]/delta t 2 N2O5 → NO2 + 4 O2 2 N2O5 → 4 NO2 + O2 1/4NO2 + O2 →1/2 N2O5 1/2N2O5 → 1/4NO2 + O2 4 NO2 + O2 → 2 N2O5

2 N2O5 → 4 NO2 + O2

Consider the phase diagram shown. What is the triple point?

5.1 atm, -56.7 °C

Using the decomposition of the Metal Oxide below, calculate the standard free energy, ΔG∘, in KJ at room temperature ( 298 K) using standard enthalpies of formation and standard entropies. The needed information is provided in Table 1. M2O(s)⟶2M(s)+12O2(g) Table 1. Standard enthalpy of formation and standard entropies. CompoundΔHf∘ (kJ/mol)ΔS∘ (J/K-mol) M2O(s) 16.45 23.2 M(s) 279.9 6.41 O2(g) 0 0

546.44

Give the coordination number for a body-centered cubic cell. 10 8 0 6 12

8

What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10^-14? 0.465 8.446 7.000 7.233 6.767

6.767

Which one of the following statements is TRUE? A buffer is an aqueous solution composed of two strong bases. A buffer does not change pH when strong base is added. A buffer can absorb an unlimited amount of base. A buffer resists pH change by neutralizing added acids and bases. All of the above are true.

A buffer resists pH change by neutralizing added acids and bases.

Reaction rate can change with temperature. the addition of a catalyst. reactant concentrations. A and C. A, B, and C.

A, B, and C.

Define deposition. A gas becomes a solid. A solid becomes a gas. A solid becomes a liquid. A liquid becomes a gas. A gas becomes a liquid.

A gas becomes a solid.

Define boiling. A solid becomes a liquid. A gas becomes a solid. A gas becomes a liquid. A solid becomes a gas. A liquid becomes a gas.

A liquid becomes a gas.

Define a salt bridge. A pathway between the cathode and anode in which ions are oxidized. A pathway between the cathode and anode in which ions are reduced. A pathway by which counter ions can flow between the half-cells without the solutions in the half-cell totally mixing. A pathway, composed of salt water, that ions pass through. A pathway in which no ions flow.

A pathway by which counter ions can flow between the half-cells without the solutions in the half-cell totally mixing.

Choose the statement below that is TRUE. A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. None of the above are true.

A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.

Which of the following bases is the weakest? The base is followed by its Kb value. (CH3CH2)3N, 5.2 × 10-4 C5H5N, 1.7 × 10-9 HOCH2CH2NH2, 3.2 × 10-5 NH3, 1.76 × 10-5 Since these are all weak bases, they have the same strength.

C5H5N, 1.7 × 10-9

Define buffer capacity. Buffer capacity is the amount of base that can be added until all of the base is used up. Buffer capacity is the amount of acid that can be added until all of the base is used up. Buffer capacity is the amount of base that can be added until all of the acid is used up. Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness. Buffer capacity is the amount of acid that can be added until all of the acid is used up.

Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness.

What element is being oxidized in the following redox reaction?MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g) Mn H O C

C

What element is being reduced in the following redox reaction?Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq) Cl Cr H O

Cl

What element is being oxidized in the following redox reaction?Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq) Cl Cr O H

Cr

Which of the following statements is TRUE? In general, the solubility of a solid in water decreases with increasing temperature. The solubility of an ionic solid in water decreases with increasing temperature. In general, the solubility of a gas in water decreases with increasing temperature. The solubility of a gas in water usually increases with decreasing pressure. None of the above statements are true.

In general, the solubility of a gas in water decreases with increasing temperature.

Which of the following statements is TRUE? Entropy is temperature independent. Exothermic processes decrease the entropy of the surroundings. ΔSuniverse is always greater than zero for a nonspontaneous process. Entropy is an extensive property. None of the above are true.

Entropy is an extensive property.

The ________ Law of Thermodynamics states the energy is conserved in chemical processes. Zero First Second Third Fourth

First

Identify the statement that is FALSE. Entropy generally increases with increasing molecular complexity. The entropy of a gas is greater than the entropy of a liquid. Entropy increases with dissolution. Free atoms have greater entropy than molecules. For noble gasses, entropy increases with size.

Free atoms have greater entropy than molecules.

Express the equilibrium constant for the following reaction.3 CH3Cl(g) + 3/2 Cl2(g) ⇔ 3 CH2Cl2(g) + 3/2 H2(g) K = K = K = K = K =

K = [CH2Cl]63[H2]^3/2 /[CH3Cl]^3[Cl2]^3/2 (q17)

Balance the following reaction under basic conditions. What are the coefficients in front of H2O and Cl- in the balanced reaction?Cl2(aq) + Br2(l) → BrO3-(aq) + Cl-(aq) H2O = 6, Cl- = 10 H2O = 2, Cl- = 5 H2O = 7, Cl- = 3 H2O = 2, Cl- = 2 H2O = 4, Cl- = 6

H2O = 6, Cl- = 10

Place the following in order of increasing standard molar entropy. H2O(l)H2O(g)H2O(s) H2O(s) < H2O(l) < H2O(g) H2O(l) < H2O(s) < H2O(g) H2O(g) < H2O(l) < H2O(s) H2O(g) < H2O(s) < H2O(l) H2O(s) < H2O(g) < H2O(l)

H2O(s) < H2O(l) < H2O(g)

Identify the diprotic acid. HBr HNO3 H2SO4 HClO4 CH3COOH

H2SO4

Which of the following is an Arrhenius acid? H2SO4 CH3CH3 NH2CH3 NaOH More than one of these is an Arrhenius acid.

H2SO4

Which of these is an example of a polyprotic oxyacid? H3PO4 CH3COOH HCN HClO3 None of the above

H3PO4

The stomach excretes ________ to kill microorganisms and to activate enzymes that break down food. HCl HNO3 CH3COOH LiHCO3 HBr

HCl

Identify the weakest acid. HI HF HBr HCl Not enough information is available.

HF

Which of the following statements is FALSE? When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent. K >> 1 implies that the reaction is very fast at producing products. When K >> 1, the forward reaction is favored and essentially goes to completion. When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.

K >> 1 implies that the reaction is very fast at producing products.

A ligand is a molecule or ion that acts as a Lewis acid conjugate base Brønsted-Lowry acid Lewis base Arrhenius base

Lewis base

What are the units of k in the following rate law?Rate = k[X][Y]^2 M^2s^-1 M^-3s^-1 M^-1s^-2 M^2s M^-2s^-1

M^-2s^-1

What element is being reduced in the following redox reaction?MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g) H O C Mn

Mn

Identify the base that is in baking soda. K2CO3 NH3 RbOH NaOH NaHCO3

NaHCO3

Give the direction of the reaction, if K ≈ 1. The forward reaction is favored. The reverse reaction is favored. Neither direction is favored. If the temperature is raised, then the forward reaction is favored. If the temperature is raised, then the reverse reaction is favored.

Neither direction is favored.

What element is being oxidized in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2⁻(aq) + O2(g) O C Cl N H

O

Determine the rate law and the value of k for the following reaction using the data provided.NO2(g) + O3(g) → NO3(g) + O2(g) [NO2]i (M) [O3]i (M) Initial Rate 0.10 0.33 1.42 0.10 0.66 2.84 0.25 0.66 7.10 Rate = 43 M^-1s^-1[NO2][O3] Rate = 1360 M^-2.5s^-1[NO2]^2.5[O3] Rate = 430 M^-2s^-1[NO2]^2[O3] Rate = 130 M^-2s^-1[NO2][O3]^2 Rate = 227 M^-2.5s^-1[NO2][O3]^2.5

Rate = 43 M^-1s^-1[NO2][O3]

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. 2NO(g) + Cl2(g) → 2NOCl(g) Rate=−1/2 Δ[NOCl]/ Δt Rate=−1/2 Δ[NO]/ Δt Rate=−2Δ[NOCl]/ Δt Rate=+1/2 Δ[NOCl]/ Δt It is not possible to determine without more information.

Rate=+1/2 Δ[NOCl]/ Δt

Which of the following forms an ionic solid? Rb I Ag S O3 C7H15NH2

Rb I

________ is applied to roads in wintertime so that the ice will melt at a lower temperature. Antifreeze Sugar Oil Salt Water

Salt

Consider a reaction that has a negative ΔH and a negative ΔS. Which of the following statements is TRUE? This reaction will be spontaneous only at high temperatures. This reaction will be spontaneous at all temperatures. This reaction will be nonspontaneous at all temperatures. This reaction will be nonspontaneous only at high temperatures. It is not possible to determine without more information.

This reaction will be nonspontaneous only at high temperatures.

Which of the following is TRUE? The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. An indicator is not pH sensitive. A titration curve is a plot of pH vs. the [base]/[acid] ratio. At the equivalence point, the pH is always 7. None of the above are true.

The equivalence point is where the amount of acid equals the amount of base during any acid-base titration.

Give the reason that antifreeze is added to a car radiator. The freezing point is elevated and the boiling point is lowered. The freezing point is lowered and the boiling point is elevated. The freezing point and the boiling point are lowered. The freezing point and the boiling point are elevated. None of the above.

The freezing point is lowered and the boiling point is elevated.

Give the characteristic of a second order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant.

The rate of the reaction is proportional to the square of the concentration of the reactant.

Give the direction of the reaction, if K << 1. The forward reaction is favored. The reverse reaction is favored. Neither direction is favored. If the temperature is raised, then the forward reaction is favored. If the temperature is raised, then the reverse reaction is favored.

The reverse reaction is favored.

Which of the following statements is generally TRUE? The solubility of a solid is highly dependent on both pressure and temperature. The solubility of a solid is highly dependent on temperature. The solubility of a solid is not dependent on either temperature or pressure. The solubility of a solid is highly dependent on pressure. None of the above.

The solubility of a solid is highly dependent on temperature.

A solution is formed at room temperature by vigorously dissolving enough of the solid solute so that some solid remains at the bottom of the solution. Which statement below is TRUE? The solution is considered supersaturated. The solution is considered unsaturated. The solution would be considered unsaturated if it were cooled a bit to increase the solubility of the solid. The solution is considered saturated. None of the above are true.

The solution is considered saturated.

Define triple point. The temperature that is unique for a substance. The temperature, pressure, and density for a gas. The temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium. The temperature at which the boiling point equals the melting point. The temperature at which the solid and liquid co-exist.

The temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium.

Consider a reaction that has a positive ΔH and a negative ΔS. Which of the following statements is TRUE? This reaction will be spontaneous only at high temperatures. This reaction will be spontaneous at all temperatures. This reaction will be nonspontaneous at all temperatures. This reaction will be nonspontaneous only at high temperatures. It is not possible to determine without more information.

This reaction will be nonspontaneous at all temperatures.

Consider a reaction that has a negative ΔH and a positive ΔS. Which of the following statements is TRUE? This reaction will be spontaneous only at high temperatures. This reaction will be spontaneous at all temperatures. This reaction will be nonspontaneous at all temperatures. This reaction will be nonspontaneous only at high temperatures. It is not possible to determine without more information.

This reaction will be spontaneous at all temperatures.

Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE? This reaction will be nonspontaneous at all temperatures. This reaction will be spontaneous only at high temperatures. This reaction will be nonspontaneous only at high temperatures. This reaction will be spontaneous at all temperatures. It is not possible to determine without more information.

This reaction will be spontaneous only at high temperatures.

Base on relative strengths of acids and bases, select the stronger acid from the following equilibrium SO42−(aq)+HCN(aq)⇋HSO4−(aq)+CN−(aq) The hydrogen sulfate ion. HCN CN The sulfate ion.

WRONG---HCN CORRECT---

The stronger the acid, then which of the following is TRUE? The weaker the conjugate base. The stronger the conjugate base. The stronger the conjugate acid. The weaker the conjugate acid. None of the above

WRONG---The weaker the conjugate acid. CORRECT---

Which of the following processes have a ΔS < 0? The melting of a cube of ice Condensation of water vapor into rain drops Dissolving of salt into water Dry ice sublimating into carbon dioxide gas Water boiling on the stovetop

WRONG---Water boiling on the stovetop ----CORRECT

Identify the type of solid for argon. metallic atomic solid ionic solid nonbonding atomic solid molecular solid networking atomic solid

nonbonding atomic solid

Write a balanced reaction for which the following rate relationships are TRUE.Rate = 1/2 delta[N2]/delta t = delta[O2]/delta t = -1/2 delta[N2]/delta t 1/2N2 + O2 → 1/2 N2O 2 N2O → 2 N2 + O2 1/2 N2O →1/2 N2 + O2 2 N2 + O2 → 2 N2O N2O → N2 + 2 O2

[2 N2 + O2 → 2 N2O]--WRONG CORRECT____

Give the expression for the solubility product constant for BaF2. BaF2(s)⇋Ba(aq)+2F−(aq) [Ba^2+][F⁻]^2/[BaF2] [Ba^2+][ F⁻] [Ba^2+][F⁻]^2 [Ba^2+]/{Ba^2=][2F-]^2 [Ba^2+]^2[ F⁻]

[Ba^2+][F⁻]^2

Give the expression for the solubility product constant for PbCl2. PbCl2(s)⇋Pb(aq)+2Cl−(aq) [Pb^2+]^2[Cl⁻]/[PbCl2] [PbCl2]/ [Pb^2+][Cl⁻]^2 [Pb^2+][Cl⁻]^2 [Pb^2+][2Cl⁻]^2/[PbCl2] [Pb^2+]^2[ Cl⁻]

[Pb^2+][Cl⁻]^2

What data should be plotted to show that experimental concentration data fits a zeroth-order reaction?

[reactant] vs time

All of the following are examples of a spontaneous process EXCEPT a boulder slides down the side of a mountain. a pencil falls off a table and drops on the floor. ice melting when the temperature rises above 0°C. a driver warming up her car engine a pure copper coin left outside in the rain starts to rust.

a driver warming up her car engine

A solution containing more than the equilibrium amount is called an unsaturated solution. a saturated solution. a supersaturated solution. a concentrated solution. a dilute solution

a supersaturated solution.

Identify the colligative property. osmotic pressure vapor pressure lowering boiling point elevation freezing point depression all of the above

all of the above

A solution containing less than the equilibrium amount is called a saturated solution. a dilute solution. a supersaturated solution. an unsaturated solution. a concentrated solution.

an unsaturated solution.

Stalactites and stalagmites form as ________ precipitates out of the water evaporating in underground caves. sodium bicarbonate sodium chloride calcium carbonate hydrochloric acid sodium hydroxide

calcium carbonate

The forces between polar molecules is known as dipole-dipole forces. hydrogen bonding. ion-dipole forces. ionic forces. dispersion forces.

dipole-dipole forces.

A Lewis base donates a proton. accepts electrons. donates more than one proton. donates electrons. accepts a proton

donates electrons.

Identify the battery that is used as a common flashlight battery. NiCad battery fuel cell dry-cell battery lithium ion battery lead-acid storage battery

dry-cell battery

Equilibrium in which rate of the forward reaction equals the rate of the reverse reaction is impossible. dynamic. volume independent. concentration independent. temperature independent.

dynamic

Which one of the following has a low density? liquid solid gas none of the above all of the above

gas

For a given compound, list the decreasing order of entropy for a liquid, solid, and gas. gas > solid > liquid solid > liquid > gas gas > liquid > solid liquid > solid > gas solid > gas > liquid

gas > liquid > solid

The heat required to melt 1 mol of a solid is known as the critical point. freezing point. melting point. heat of fusion. heat of vaporization.

heat of fusion.

What is the strongest type of intermolecular force present in NH2CH3? hydrogen bonding dispersion ion-dipole dipole-dipole none of the above

hydrogen bonding

Identify the characteristics of a gas. indefinite shape, but definite volume indefinite shape and volume definite shape and volume none of the above all of the above

indefinite shape and volume

Chemical equilibrium is the result of all of the reactants being converted into products. stoppage of further reaction. a loss of pressure in the system. formation of products equal in mass to the mass of the reactants. opposing reactions attaining equal rates.

opposing reactions attaining equal rates.

Which type of bonding does Sr form upon solidification? molecular ionic covalent network metallic

metallic

Identify the type of solid for gold. metallic atomic solid ionic solid nonbonding atomic solid molecular solid networking atomic solid

metallic atomic solid

Give the term for the amount of solute in moles per kilogram of solvent. molarity mass percent mole percent molality mole fraction

molality

Give the term for the amount of solute in moles per liter of solution. mole percent molarity mole fraction molality mass percent

molarity

Identify the type of solid for diamond. metallic atomic solid ionic solid nonbonding atomic solid molecular solid networking atomic solid

networking atomic solid

Identify the process that is spontaneous photosynthesis electrocatalysis burning wood rusting of iron water flowing uphill

rusting of iron

Which one of the following has a definite shape and volume?

solid

In a liquid, the energy required to increase the surface area by a unit amount is called capillary action. viscosity. dipole-dipole force. surface tension. hydrogen bonding.

surface tension.

Identify the location of oxidation in an electrochemical cell. the electrode the cathode the socket the salt bridge the anode

the anode

Identify the location of reduction in an electrochemical cell. the salt bridge the cathode the electrode the socket the anode

the cathode

Give the direction of the reaction, if K >> 1. The forward reaction is favored. The reverse reaction is favored. Neither direction is favored. If the temperature is raised, then the forward reaction is favored. If the temperature is raised, then the reverse reaction is favored

the forward reaction is favored.

Define freezing. the phase transition from solid to gas the phase transition from gas to solid the phase transition from gas to liquid the phase transition from liquid to gas the phase transition from liquid to solid

the phase transition from liquid to solid

Define sublimation. the phase transition from solid to gas the phase transition from gas to solid the phase transition from gas to liquid the phase transition from liquid to gas the phase transition from liquid to solid

the phase transition from solid to gas

Define fusion. the phase transition from solid to liquid the phase transition from gas to solid the phase transition from gas to liquid the phase transition from liquid to gas the phase transition from liquid to solid

the phase transition from solid to liquid

In a semiconductor, the bonding molecular orbitals that contain electrons are referred to as the ________, while the antibonding orbitals that are completely empty are referred to as the ________. single bond, antibond conduction band, valence band valence band, conduction band n-type, p-type p-type, n-type

valence band, conduction band

The resistance of a liquid to flow is known as viscosity. capillary action. intermolecular forces. meniscus. surface tension.

viscosity.