Inorganic Chemistry Questions

Which of the following statements is true? X. CH4 has a higher boiling point than CCl4 Y. trans-1,2-dichloroethene has a lower boiling point than cis-1,2-dichloroethene Z. H₂C-O has a higher boiling point than ethylene, C₂H6. only Z only Y X and Y All of them only X Y and Z X and Z None of them

At 27. °C, a gas occupies a volume of 2.75 L under 0.500 atm of pressure. At what temperature will this same amount of gas occupy 3.10 L with 0.700 atm of pressure? Assume ideal gas behavior. Provide your answer as an integer.

A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the barometric pressure is 686. torr. The mercury level in the open arm is 7.8 cm above that in the arm connected to the flask of neon. What is the neon pressure, in torr? Provide your answer in decimal notation rounded to the appropriate number of significant figures. Answer: Enter Value torr

Argon has normal boiling and freezing points of 87.3 K and 83.8 K, respectively. The triple point of argon occurs at 83.8 K at 0.68 atm. What physical change can be observed - if any - when the temperature of an argon sample is increased from 85 K to 90 K at a constant pressure of 0.46 atm? no physical change occurs - the sample is gas and stays gas solid to liquid liquid to gas no physical change occurs - the sample is liquid and stays liquid solid to gas

Determine the molar mass (in g/mol) of a gas that travels with an effusion time that is 2.38 times longer than that of F₂(g). Enter your answer in decimal notation to three significant figures. Answer: Enter Value g/mol

A closed vessel of fixed volume contains 22.9 g of CO₂(g) exerting a pressure of 1.50 atm. Some CH4(g) is introduced into the vessel, increasing the pressure to 3.25 atm. What mass of CH4(g) (in grams) was introduced in the vessel? Enter your answer in decimal notation, rounded to 3 significant figures.

Predict the starting materials of the following reactions, then write a balanced reaction showing the complete molecular equation: a.→ CaSO4(aq) +H₂0(1) b. → Na3PO4(aq) +H20(1) c. → MgCl₂(aq) + H₂(g)

Consider the following metals, A, B C and D at room temperature. 10.00 g of each metal absorbs 15kJ. Which metal will reach the highest temperature? Metal Specific Heat (Cs) in kJ/g°C A 1.0 B 5.0 C 10.0 D 25.0

How many moles of solid Ba(NO3)2 should be added to 300. mL of 0.20 M Fe(NO3)3 to increase the concentration of NO3- ion to 1.0 M? (Assume that the volume of the solution remains constant) a) 0.060 mol b) 0.12 mol c) 0.24 mol d) 0.41 mol

Problem: (Practice exam Q.20) Which of the following statements is true? a) H₂O has a greater dipole moment than H₂S b) H₂O is a polar, but H₂S is non-polar c) Both H₂O and H₂S have zero dipole moments d)Both H₂O and H₂S are linear

Why does water (H₂0 TB = 100°C) have a higher boiling point temperature in comparison to hydrogen sulfide (H₂S TB = -60°C)? H₂O is just a lot more stubborn than H₂S H₂O is a more polar molecule than H₂S Intermolecular forces are greater for H₂S in comparison to H₂O H₂O has a lower heat of vaporization than H₂S H₂O has a higher vapor pressure than H₂S

(6 pts) The molarity of a NaOH solution is 1.72x10-10 M. 4a. Calculate the [OH-], [H+], pOH, pH. Need to write the answers with one digit after the decimal for the pOH and pH. For the [OH-] and [H], the answers must be in scientific notation with one digit after the decimal. Must show all your work. Do not use scratch paper. Do the work directly on your paper. 4b)This solution is (acidic, basic, or neutral). (select the correct answer). Briefly explain.

Pb + Zn(OH)₂+ OH-Zn + HPbO₂ + H₂O In the above reaction, the oxidation state of zinc changes from to How many electrons are transferred in the reaction?

A sample of carbon dioxide gas at a pressure of 903 mm Hg and a temperature of 49 °C, occupies a volume of 9.34 liters. If the gas is heated at constant pressure to a temperature of 91 °C, the volume of the gas sample will be L.

Problem: When 100. mL of 0.100 M NaOH is mixed with 100. mL 1.00 M HCl the temperature of the solution increases from 25.0 °C to 28.0 °C. Calculate the AH for the reaction. Give: ducation -1.1 g/mL, Csolution - 4.1 J/g C

A sample of oxygen gas collected at a pressure of 0.751 atm and a temperature of 10.0 °C is found to occupy a volume of 27.6 liters. How many moles of O₂ gas are in the sample?

Why does KBr have a lower melting point temperature than NaCl? a. Because the electron transfer, a requirement for ionic bonding, is less complete for KBr salts b. Because KBr salts ions with greater charge than those found in NaCl. c. Because period 4 elements have lower melting point temperatures as a general rule d. Because KBr salts are composed of larger ions than NaCl salts. e. Because NaCl salts utilize expanded ionic bonding; something not possible for KBr salts

Alchemist adds 340.0 mL of a 2.5 mol/L potassium iodide (KI) solution to a reaction flask. Calculate the mass in kilograms of potassium iodide the chemist has added to the flask.

Assume that Potassium Iodide and Lead(II) Nitrate are the starting substances (reactants) in a reaction: a. Write a balanced chemical reaction between Potassium Iodide and Lead(II) Nitrate. Be sure to include physical states. b. State the names of the products that are produced from this reaction. c. Write complete ionic and net ionic reactions for the balanced equation in part (a). d. What type of reaction(s) is/are being represented by the chemical reaction you wrote in part (a)? e. If 9.2 g of potassium iodide and 1.8 g of lead(II) iodide are combined then theoretically, what mass of solid product could be formed from these amounts of reactants? What is the limiting reactant? f. What is the % yield if 3.550 g of the solid product was actually obtained? g. Based on your answers to parts (a) - (f), determine whether a solid precipitate forms in the reaction. h. How many potassium atoms are in 0.227 g of potassium iodide? i. How many moles of lead(II) nitrate will react with 0.887 mg of potassium iodide? j. How many molecules are in one mole of lead(II) nitrate?

Given the following equilibrium equation: heat+ N₂(g) + 3 F2(g) <--> 2 NF3 How would Increasing the size of the reaction container change the equilibrium? It would shift the equilibrium to the right to make more products. It would shift the equilibrium to the right and consume more NF3. It would shift the equilibrium to the left and consume more F2. It would shift the equilibrium to the left and make more N₂.

PI3Cl2 is a nonpolar molecule. Based on this information, determine the I-P-I bond angle, the CI-P-Cl bond angle, and the I-P-Cl bond angle. Enter the number of degrees of the I-P-I, CI-P-Cl, and I-P-Cl

How many grams of PbBr₂ will precipitate when excess CrBr₂ solution is added to 51.0 mL of 0.657 M Pb(NO3)2 solution? Pb(NO3)2(aq) + CrBr₂(aq) → PbBr₂(s) + Cr(NO3)2(aq)

Given the following reaction: CH3COOH + H₂O <==> CH3COO™ + H3O+ How would Removing CH3COO and adding CH3COOH shift the reaction? This would shift the equilibrium to the right and make the solution more alkaline. This would not shift the equilibrium and pH would remain the same. This would shift the equilibrium to the left and make the solution more alkaline. This would shift the equilibrium to the right and make the solution more acidic. This would shift the equilibrium to the left and make the solution neutral.

SO3 is place into a 1.00 liter container. At equilibrium, the concentration of SO3 is 1.00 M, while the concentration of SO2 is 0.50 M and that of O₂ is 1.50 M. Calculate the value of the equilibrium constant for the following reaction: 2 SO2 + O₂ <=> 2 SO3 (all are gases) Keq = 1.3 Keq = 6.00 Keq = 0.38 Keq = 2.7

For the following reaction, 6.93 grams of sulfur dioxide are mixed with excess water. The reaction yields 6.33 grams of sulfurous acid (H₂SO3). sulfur dioxide (g) + water (1) -> sulfurous acid (H₂SO3) (g) What is the theoretical yield of sulfurous acid (H₂SO3) ? What is the percent yield for this reaction ?

A 50.0 mL sample of 0.010 M HCI solution was diluted to 500.0 mL. What is the pOH of the new acid solution? But first answer these questions: 1st) What is the pH of the original 0.010 M HCl solution: [H+]=0.010M 2nd) What is the molar concentration of the new dilute solution: 3rd) What is the pH of the new dilute acid solution: 4th) What is pOH of the new dilute acid solution. (A) 1st) pH of original = 2.0 2nd) Concentration of dilution solution = 0.001 M 3rd) pH of dilution solution = 11.0 4th) pOH of dilution solution = 3.0 (B) 1st) pH of original = 1.0 2nd) Concentration of dilution solution = 0.1 M 3rd) pH of dilution solution = 1.0 4th) pOH of dilution solution = 13.0 (C) 1st) pH of original = 1.0 2nd) Concentration of dilution solution = 0.001 M 3rd) pH of dilution solution = 3.0 4th) pOH of dilution solution 11.0 B

What volume of a 0.160 M hydroiodic acid solution is required to neutralize 26.9 mL of a 0.101 M sodium hydroxide solution?

When 1 mole of Al(OH)3 chemically reacts with 1 mole of H3PO4, what salt is formed? a. Al(OH)3 is the salt formed. b. Al3PO4 is the salt formed. c. AIPO4 is the salt formed. d. H3PO4 is the salt formed.

What would be the pH of a solution if 0.0010 moles of KOH was mixed with 0.0015 moles of HNO3? Assume volume is 1 L Assume volume is 1.0 L. HNO3 is more than KOH a how much extra HNO3 do we have? knowing this will allow you to get [H+] which will allow you to calculate the pH. a. Solution pH = 2.8 b. Solution pH = 3.3 c. Solution pH = 3.0 d. Solution pH = 11.0

Write a balanced chemical equation for the neutralization reaction of hydrochloric acid with sodium hydroxide. a. 2HCI + NaOH → NaCl + 2H₂O b. HCI + 2NaOH →2NaCl + H₂O c. 2HCl + 2NaOH → 2NaCl + 2H₂O d. HCI + NaOH → NaCl + H₂O

What is true of an acidic solution? An acidic solution contains more hydronium ions than hydroxide ions. An acidic solution contains the same number of hydronium ions as hydroxide ions. An acidic solution contains more hydroxide ions than hydronium ions. An acidic solution contains more OH ions than H3O+ ions.

When 1 mole of Mg(OH)2 chemically reacts with 1 mole of H₂S, what salt is formed? a. H₂S is the salt formed. b. MgS2 is the salt formed c. Yes, MgS is the salt magnesium sulfide formed when the cation of the base combines with the anion of the acid. d. Mg(OH)2 is the salt formed.

An acid is a compound that dissociates in water to produce ___ ion, which are ____ Hydronium ions, which are cations. Hydronium ions, which are anions. Hydroxide ions, which are cations. Hydroxide ions, which are anions.

What is true of an alkaline solution? An alkaline solution has more hydrondium ions than hydroxide ions. An alkaline solution contains more H3O+ ions than OH ions. An alkaline solution has the same number of hydroxide ions as hydrondium ions. An alkaline solution has more hydroxide ions than hydronium ions.

When 1 mole of Ca(OH)2 chemically reacts with 1 mole of H₂SO4, what salt is formed? a. Ca₂SO4 is the salt formed. b. Ca(OH)2 is the salt formed c. CaOH is the salt formed. d. CaSO4 is the salt formed.

What is the electron geometry of CIF5 ? What is the molecular geometry of CIF5? Ignoring lone-pair effects, what is the smallest bond angle in CIF5 ?

A chemist must prepare 800.0 mL of hydrobromic acid solution with a pH of 0.60 at 25 °C. He will do this in three steps: • Fill a 800.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (6.0 M) stock hydrobromic acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrobromic acid that the chemist must measure out in the second step.

A chemist must prepare 450.0 mL of hydrobromic acid solution with a pH of 1.60 at 25 °C. He will do this in three steps: • Fill a 450.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (6.0M) stock hydrobromic acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrobromic acid that the chemist must measure out in the second step.

The molecule [CuF6]K4 has a unique structure (due to jahn-teller distortion) where it has an elongated z-axis in the octahedral structure which changes its point group from Oh to D4h. Answer the following questions related to elongated structure of [CuF6]K4. a. The oxidation state of Cu: ___and F: ___ b. Calculate the total number of electrons for [CuF6]4-: ____

Which statement is correct for pure water? a. if truly pure, water contains only H₂O molecules, and no ions b. pure water contains no hydronium ions c. pure water contains no hydroxide ions d. pure water contains hydronium and hydroxide ions in equal concentrations

If you dissolve 10.0 g of compound X in 100.0 mL of distilled water, the liquid turns red. The temperature of the liquid stays at 24 °C for 10 minutes. Why would you not want to sell a cold pack made with compound X?

Hydrogen atoms emit light with a wavelength of 410.2 nm when the electron transitions from the n = 6 level to a final quantum state. Associate each of the quantities in this question with a variable and/or constant in an equation from your equation sheet. What is the sign associated with the change in energy of this transition? What is the value of ΔE? What is the quantum number of this final state (nf)?

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) Cu(s) + FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 100. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 135. mg. Calculate the original concentration of copper(II) sulfate in the sample.

What are the expected bond angles in ICl4+? 90 degrees 109.5 degrees 120 degrees 180 degrees

An analytical chemist weighs out 0.024 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 1.5 mL of NaOH solution. Calculate the molar mass of the unknown acid.

Predict the reactants of this chemical reaction. ___ → CaF₂(aq) + H₂O(l)

The fact that butane gas (found in lighters) as well as gasoline vapor when combined with oxygen burn, relates a two substances. a. intensive physical property b. extensive physical property c. a chemical as well as physical property d. physical property e. chemical property

The percent by mass of fluorine in PNF2 is

1. How many ATOMS of sulfur are present in 2.55 moles of sulfur dioxide ? 2. How many MOLES of oxygen are present in 3.89x1022 molecules of sulfur dioxide ?

Based on formal charges, draw the most preferred Lewis structure for the chlorate ion, ClO3-