Preparation and Properties of Compounds Questions and Answers

Given the standard enthalpy changes for the following two reactions: (1) 2Fe(s) + O₂(g) →2FeO(s) ΔH = -544.0 kJ (2) Fe(s) + Cl₂(g) →FeCl₂(s) ΔH = -341.8 kJ what is the standard enthalpy change for the reaction: (3) 2FeCl₂(s) + O₂(g)- 2FeO(s) + 2Cl₂(g) ΔH² = ?

The compound barium iodide is a strong electrolyte. Write the reaction when solid barium iodide is put into water:

Many chromate (CrO42) salts are insoluble, and most have brilliant colors that have led to their being used as pigments. Choose the correct net ionic equation for the reaction of Ba²+ with a chromate ion. Ba²+ (aq) + CrO42 (aq) → Ba₂ CrO4(s) Ba²+ (aq) + CrO4² (aq) → BaCrO4 (aq) Ba²+ (aq) + CrO4² (aq) → BaCrO4 (s) Ba²+ (aq) + CrO4² (aq) → Ba(CrO4)2 (8)

Draw the electron distribution diagram for water. Begin with 1 central water molecule. Show the chemistry of each element within the central water molecule (all electron orbits, lone pair electrons, type of chemical bond, polarity/charge, and correct shape). What type of bond creates a water molecule? What type of bond holds 1 water molecule to another water molecule? Next, draw the correct number of other water molecules bonding to the central water molecule. How many other water molecules bond to a central molecule of water?

Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) a aqueous barium hydroxide and nitric acid

What number of Ti atoms and what amount (moles) of Ti atoms are in 100.0 g of titanium?

In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: 3N₂H₂ + 2Cr+ 6H₂O →ONH3 + 2Cr(OH)3 formula of the oxidizing agent: name of the element reduced: formula of the reducing agent:

When aqueous solutions of ammonium carbonate and silver(I) nitrate are combined, solid silver(I) carbonate and a solution of ammonium nitrate are formed. The net ionic equation for this reaction is:

A unknown atom has atomic number of 7 and mass number 15. It has s. 7 protons and 7 neutrons. b. 7 protons and 8 neutrons. c. 7 protons and 15 neutrons. d. 15 protons and 7 neutrons. e. 8 protons and 7 neutrons

The following skeletal oxidation-reduction reaction occurs under basic conditions. Write the balanced OXIDATION half reaction. Br + ClO3 → Br₂ + Cr

1. How many GRAMS of cobalt(II) cyanide are present in 3.07 moles of this compound ? 2. How many MOLES of cobalt(II) cyanide are present in 2.96 grams of this compound ?

According to the following reaction, how many grams of phosphoric acid are necessary to form 0.170 moles potassium phosphate? potassium hydroxide (aq) + phosphoric acid (aq) →potassium phosphate (aq) + water (l)

Choose the correct net ionic equation for the reaction between nickel(II) chloride and sodium oxalate. Ni2+ (aq) + C₂04²(aq) → NiC₂O4(s) NiCl₂(aq) + Na₂C₂O4(aq) → NiC₂O4(s) + 2 NaCl(aq) Ni2+ (aq) + 2 Cl(aq) + 2 Na*(aq) + C₂04² (aq) → Ni²+ (aq) + C₂042 (aq) + 2Na*(aq) + 2CH(aq) Ni2+ (aq) + 2 CH(aq) + 2 Na*(aq) + C₂04²(aq) → NIC2O4(s) + 2Na*(aq) + 2CH(aq)

The compound lead(II) cyanide is a strong electrolyte. Write the reaction when solid lead(II) cyanide is put into water:

The compound copper(II) nitrate is a strong electrolyte. Write the reaction when solid copper(II) nitrate is put into water:

The following reactions 2K(s) + Br₂(1)→ 2KBr(s) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) HCl(aq) + KOH(aq) → H₂O(l) + KCl(aq) are examples of precipitation (two) and acid-base reactions, respectively. redox, precipitation, and acid-base, respectively. Oprecipitation reactions. Oredox reactions. None of these choices are correct.

For the following reaction, 25.2 grams of hydrochloric acid are allowed to react with 51.8 grams of barium hydroxide. hydrochloric acid(aq) + barium hydroxide(aq) barium chloride(aq) + water(l) A.What is the maximum amount of barium chloride that can be formed? B.What is the FORMULA for the limiting reagent? C.What amount of the excess reagent remains after the reaction is complete?

You are given 0.902 g of an unknown diprotic acid, H₂A. It reacts with NaOH according to this balanced equation. H₂A(aq) + 2 NaOH(aq) → Na₂A(aq) + 2 H₂O(1) If a volume of 18.0 mL of 0.659 M NaOH is required to react with all of the acid, what is the molar mass of the acid A)38.3 g/mol B)152 g/mol C)304 g/mol D)76.3 g/mol E)15.2 g/mol

Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog: 4Fe(s) + 302(g) →2Fe₂O3(s) If there is 14.56 g Fe and excess O₂ present, the reaction yields 18.0 g Fe2O3. Calculate the percent yield for the reaction.

A compound is found to contain 63.65 % nitrogen and 36.35 % oxygen by mass. QUESTION 1: The empirical formula for this compound is______? QUESTION 2: The molar mass for this compound is 44.02 g/mol. The molecular formula for this compound is______?

The following chemical equation, 2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g), is an example of a(n)__________reaction. A)oxidation-reduction and precipitation B)oxidation-reduction and acid-base C)oxidation-reduction D)precipitation E)acid-base reaction.

An ion from a given element has 15 protons and 18 electrons. What is the charge on the ion? What is the name of the element? What is the symbol for the ion?

a. Fr-218 decays by alpha decay. What are the atomic symbol and mass number of the product? Product: b. At-209 decays by alpha decay. What are the atomic symbol and mass number of the product? Product: c. Be-7 decays by gamma emission. What are the atomic symbol and mass number of the product? Product: d. Cu-67 decays by beta decay. What are the atomic symbol and mass number of the product? Product:

Imagine you are in a laboratory. You are exploring the following reaction: A+B -->C When the product C is created, bubbles form. When 10mL of A is added to 10mL of B, the reaction takes twenty seconds. Your teacher gives you three unknown substances (X, Y, and Z), one of which is a catalyst for the reaction. Design an experiment to test substances X, Y, and Z to determine which one is a catalyst for the reaction.

4.8 g of sulfur and 5.4 g of aluminum react based on the chemical equation below and 4.5 g of aluminum sulfide (Al₂S₃) are recovered from the reaction, a small amount cannot be recovered. 3S + 2A1 → Al₂S₃ Determine the percent yield of Al2S3- (Molar mass of S = 32.06g/mol, molar mass of Al = 26.98 g/mol)

Example Solute Solvent Solution 1. Fruit-flavored drink (25 g flavoring powder ---------- ------------ -------- in 1000 g water). 2. Simple syrup(450g sugar -------- ------------ -------- in 550g water) 3. Medical saline (4 g salt in ---------- ------------ ------- 100 g water)

The formula for the conjugate acid of C6H6O6^2- is ________ The formula for the conjugate acid of HPO4^2- is __________

If a salesperson placed an ad in the paper or put a sign on a property he had listed without giving the name of the brokerage he would have placed (a) A legal and proper sign (b) A sign by estoppel. (c) A blind ad (d) A deaf sign

Which of the following statements about the benefits of phosphates as active components of biochemistry are true? Select one or more: a. Phosphate are kinetically stable b. Their negative charges protect from nucleophilic attacks c. Phosphates are thermodynamically unstable d. Removal of a phosphate has a highly positive free energy change associated with it e. Phosphates are non-polar

Write the balanced chemical equation for each of the reactions. Include phases. When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. However, when additional aqueous hydroxide is added, the precipitate redissolves, forming a soluble [Pb(OH)4]²-(aq.) complex ion.

Looking at the same nonmetal group on the periodic table, how does the reactivity of an element in period 2 compare to the reactivity of an element in period 4? The period 2 element would be more reactive because the attractive force of protons is stronger when there are fewer neutrons interfering. The period 2 element would be more reactive because the attractive force of protons is stronger when electrons are attracted to a closer electron shell. The period 4 element would be more reactive because the attractive force of protons is stronger when there are more neutrons helping The period 4 element would be more reactive because the attractive force of protons is stronger when electrons are attracted to a farther electron shell.

At 25 °C, an aqueous solution has an equilibrium concentration of 0.00237 M for a generic cation, A²⁺ (aq), and 0.00474 M for a generic anion, B‾(aq). What is the equilibrium constant, Ksp, of the generic salt AB₂ (s)?

Which of the following factors explains why H2O is a polar molecule? the presence of two non-bonding pairs of electrons the presence of two hydrogen atoms the presence of two bonding pairs of electrons an asymmetrical distribution of charge

Which of the following describes the element Rb. Choose all that apply. is very reactive as a metal. forms basic solution in water. consists of diatomic molecules in elemental form. is one of the group of the least reactive elements. reacts vigorously with alkali metals to form salts. is found in nature only combined with the other elements.

The atomic radii in picometers of F, Br, and I are shown in the table below. 9 F 64 pm 17 CI ? pm 35 Br 114 pm 53 I 138 pm Using this information, predict which of the following best represents the most reasonable atomic radius of Cl.

3. Draw the chemical structure of a single lipid composed of myristic, palmitic and linoleic acids and glycerol. Label the different parts of the molecule.

Whether or not the process is observed in nature, which of the following could account for the transformation of magnesium-20 to sodium-20? (Select all that apply.) alpha decay positron emission beta decay electron capture

A 10.0 g sample of powder was found to contain 1.36 g lithium, 2.36 g carbon and 6.28 g oxygen. The molecular weight of the compound is 101.898 g/mol. Determine the empirical and molecular formula.

Which of the following enables manufacturers to provide products made in less time and with less money. less pollution, less energy, and less use of natural resources? innovative designs and processes reverse engineering eco-friendly devices and processes life cycle assessments

What is the last step in the formation of a solution with an ionic compound as a solute? Breaking of ionic bonds. Weakening of the IMF among solvent particles. Dissociation of ions. The ions are surrounded by water molecules.

Space Cadet Katrina wants to keep some leaking poison gases from escaping from the science lab on her space station. She knows that if she can reduce the pressure of the air in the lab, it will help keep bad air from flowing out into the rest of the station. She cannot manipulate the pressure directly, but she can control the air conditioning remotely. The pressure in the lab is currently 20 lbs/in² and the temperature is 27°C. She won't feel safe until she reduces the pressure to 8 lbs/in². To what temperature must she cool the lab? Assume constant volume. ANS: (t1 = 300 K = 27°C) (12= 120 K = -153°C)

Propane, C₂H, is the fuel used with barbeque grills. When propane reacts with oxygen gas, the following is the unbalanced chemical equation: _C₂H₂(g) +O₂ (g)_CO₂ (g) +H₂O (g) If properly balanced, which of the following word equations correctly describes this chemical reaction? A One molecule of propane gas and five molecules of molecular oxygen undergo a combustion reaction forming three molecules of carbon dioxide and four molecules of water. B One molecule of propane and four molecules of molecular oxygen combust, forming one molecule of carbon dioxide and four molecules of water. C One molecule of propane gas reacts with two molecules of oxygen gas in a double replacement reaction to form one molecule of carbon monoxide and two molecules of water. D Two molecules of propane gas react with 3 molecules of molecular oxygen to form one molecule of carbon dioxide and four molecules of water.

Complete the questions below based upon the following chemical reaction that has taken place during a chemistry lab. Iron (II) nitrate reacts with sodium phosphate. 1. What type of reaction was performed in the lab? What evidence would you expect to see to support your conclusion for the reaction type?

Column A 1.LIBN 2.KCI 3.MnO 4.MgCl2 5.CO2 6.H2S 7.C2B2 8.CO 9.C3N4 10.KMnO4 11.H2SO4 12.KCN 13.NaCl 14.HB 15.KNO2 Column B a. Hydrogen Sulfate (Sulfuric Acid) Sulfato de Hydrogeno (Acido Sulfurico) b. Potassium Cynide Cianuto de Potasio c. Manganese Oxide Oxido de Manganeso d. Sodium Chloride (Salt) Clroruro de Sodio (Salt) e. Carbon Monoxide Monoxido de Carbono f. Lithium Nitride Nitruro de Litio g. Dicarbon Diboron Diboruro de Dicarbono h. DiHydrogen MonoSulfide MonoSulfuro de Dihidrogeno i. Magnesium Chloride Cloruro de Magnesio j.Potassium Chloride Cloruro de potasio k. Potassium Permanganate Permanganato de Potasio l. Hydrogen Monoboron Monoboruro de Hidrogeno m. Potassium nitrite Nitrato de Potasio n. Carbon Dioxide Dioxido de Carbono o. Tricarbon tetranitride

A student calculates their theoretical yield of a certain chemical reaction to be 197 grams. They then perform the experiment and obtain an actual yield of 146 grams. Calculate the student's percent yield.

Do this on a separate sheet of paper and upload. Please show all work. The concentration of an unknown sample of sulfuric acid was determined by the method used in this experiment. In the first titration, the sodium hydroxide was standardized by titrating 0.1852g of oxalic acid dihydrate (molar mass = 126.07g/mol) with 32.30 mL of sodium hydroxide solution. In the second titration, 10.00mL of the unknown sulfuric acid solution was titrated with 12.85mL of the sodium hydroxide solution. What was the concentration of the sulfuric acid?

Ammonia reacts with copper (II) oxide according to the reaction equation shown below. NH3 + CuO → Cu + N₂ + H₂O Calculate the number of moles of ammonia consumed during the reaction if 75.1 grams of nitrogen are produced.

Nickel (III) oxide decomposes forming nickel and oxygen gas. Write the reaction equation, balance, and calculate the number of moles of nickel (III) oxide consumed during the reaction if 0.947 moles of nickel are produced.

Determine the electron geometry (eg) and molecular geometry (mg) of XY4 where X is in group 4A and Y is in group 7A. A) eg - tetrahedral, mg = trigonal pyramidal B) eg-octahedral, mg - tetrahedral C) eg - trigonal bipyramidal, mg - tetrahedral D) egtetrahedral, mg - bent E) egtetrahedral, mg = tetrahedral

155 grams of solid iron (II) sulfide reacts with aqueous hydrochloric acid (HCI). Determine what products are formed, balance the chemical equation and calculate the theoretical yield, in grams, of the product containing chlorine.