Inorganic Chemistry Questions

Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). What is the identity of element X? Al Sr Cu Ni Si

What is the name of the compound with the formula KOH ? What is the name of the compound with the formula NaHCO3 ? What is the name of the compound with the formula AI(CN)3 ?

e. Choose an example of a synthesis reaction that is also an oxidation-reduction reaction, but that does not involve combustion. 2KNO3(s) → 2KNO2 (s) + O2(g) 2Fe(s) + 3Cl2 (g) → 2FeCl3 (s) 2AgNO3 (s) → 2Ag(s) + 2NO2(g) + O₂(g) CH4 (g) +202 (g) → CO2 (g) + 2H₂O(l) NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(1) C(s) + O₂(g) → CO2 (g)

When aqueous solutions of potassium carbonate and cobalt(II) iodide are combined, solid cobalt(II) carbonate and a solution of potassium iodide are formed. The net ionic equation for this reaction is:

Jason set up a textile mill in his hometown in 1865. He became a rich businessman by the time his son Earl took over the business in 1895. Soon after Earl started heading the business, the government passed laws to regulate business and protect consumers and workers. Due to this move by the government, the textile mill had to introduce a fixed salary structure for its employees and implement quality checks for the products manufactured. In the context of the history of American business, Jason had set up this textile mill in the ______

Choose the characteristic physical properties that distinguish the metallic elements from the nonmetallic elements. (Select all that apply.) rigid and fragile bad conductors of electricity bad conductors of heat excellent conductors of electricity generally shiny (lustrous) when a fresh surface is exposed excellent conductors of heat malleable and ductile generally transparent when polished

Balance each of the chemical reactions. 1) CuSO4 (27) + Zn (3) → ZnSO4 (aq) + Cu (s) 2) NaOH(aq) + HC1 (ag) → NaCl (ag) + H₂O (l) 3) Mg (s) + O2 (g) → MgO (s) 4) Co(NO3)2 (aq) + Na₂HPO4 (aq) → NaNO3 (qq) + CoHPO4 (s) 5) NaHCO3 (s) + HC₂H³O2 (aq) → NaC₂H³O2 (aq) + H₂O (1) + CO₂ (g)

Which of the following is incorrectly named? PO43, phosphate ion NO³-, nitrite ion Mg(OH)2, magnesium hydroxide Pb(NO3)2, lead(II) nitrate NH4CIO4, ammonium perchlorate

What is the name of the compound with the formula NaCIO2 ? What is the formula of calcium hypochlorite ?

A) Determine the type of each reaction (e. single replacement, etc. 1) H2(g)+C12(g) → 2HCl(g) 2) CaCO3(s) →CaO(s)+CO2)g) 3) Fe(s)+CuSO4(aq) →FeSO4(ag)+Cu(s) 4) AgNO3(aq)+NQl→ AgCl(s)++KINOS (3) 5) CH4(g)+202(g) →CO2(g)+2H2O(g)

How many protons and neutrons are contained in the nucleus of the isotopes below? Assuming the atoms are uncharged, how many electrons are present? 22Ti48 protons neutrons electrons 56fe26 protons neutrons electrons

Many plants are poisonous because their stems and leaves contain oxalic acid, H₂C₂O4, or sodium oxalate, Na2C2O4; when ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion, C₂O4², in a sample is to precipitate this species as calcium oxalate, which is insoluble in water. Choose the right net ionic equation for the reaction between sodium oxalate and calcium chloride, CaCl2, in aqueous solution. 2Ca²+ (aq) + C₂04² (aq) → Ca₂C₂O4(s) Ca²+(aq) + C₂O4²- (aq) → CaC₂O4(s) Ca²+ (aq) + 2C₂O4²- (aq) → Ca(C₂O4)2 (8) Ca²+ (aq) + C₂ 04² (aq) → CaC₂O4 (aq)

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

a. Give the correct definition of a combustion reaction. A combustion reaction is typically a reaction in which an element or compound reacts with so quickly and with such a large release of energy that a flame results. b. In addition to the chemical products, what other products do combustion reactions produce? electrons atoms heat energy protons c. Write the chemical equation for a combustion reaction of C₂H6. (Use the lowest possible coefficients. Omit states of matter.)

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid-base, or oxidation-reduction. (Select all that apply.) K₂SO4 (aq) + Pb(NO3)2 (aq) → PbSO4(s) + KNO3(aq) precipitation acid-base oxidation-reduction HCl(aq) + Sr(s) → H₂(g) + SrCl₂ (aq) precipitation acid-base oxidation-reduction HCl(aq) + CsOH(aq) → H₂O(l) + CsCl(aq) c. O precipitation acid-base oxidation-reduction

In the examples cited by Robert Cialdini and Steve Martin, when servers provided mints to their customers as they gave them the bill, the difference in tips from giving one mint versus two mints, jumped from 3 percent to percent of the bill. a. 5 b. 14 c. 6 d. 10

Hexamethylenediamine (C6H16N₂) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (C6H10O4) by the following overall equation: C6H10 O4 (1) 2NH3 (g) + 4H2 (9)→ C6H16N2 (1) + 4H₂O(1) What is the percent yield for the reaction if 1.41 x 10³ g of Percent yield = hexamethylenediamine is made from 1.99 x 10³ g of adipic acid?

A chemist prepares a solution of calcium sulfate (CaSO4) by measuring out 0.33 g of calcium sulfate nto a 250. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's calcium sulfate solution. Be sure your answer has the correct number of significant digits.

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)

A compound containing only sulfur and phosphorus is 50.9% S by mass; the molar mass is 252 g/mol. What are the empirical and molecular formulas of the compound? Empirical formula: Molecular formula:

An unknown piece of metal weighing 68.0g at 90 °C is dropped into a calorimeter that contains 200 grams of 25 °C water. The final temperature of the is 38.3 °C. What is the 8.3°C. What is the specific heat capacity of the unknown metal?

The statement a person receives information that conflicts with their existing beliefs or attitudes, and then alters the information to coincide with those beliefs is indicative of which process? a. Selective exposure b. Selective retention. c. Selective distortion Od. Selective analysis

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?

Iron oxide ores, commonly a mixture of FeO and Fe2O3, are given the general formula Fe3O4. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes: Fe3O4(s) + H₂(g) → Fe(s) + H₂O(g) Fe3O4(s) + CO(g) → Fe(s) + CO2(g)

Choose the balanced equations that show how three of the common strong acids ionize to produce a hydrogen ion. (Select all that apply.) H₂SO4 (aq) → H+ (aq) + HSO4¯ (aq) HCl(aq) → H+ (aq) + Cl(aq) H₂SiO3(aq) → H+ (aq) + HSiO3(aq) HNO3(aq) → H+ (aq) + NO3(aq) HCIO(aq) → H+ (aq) + CIO¯(aq) Q HClO,(aq) → H*(aq) +ClO, (aq)

Complete the balanced equation for the reaction that produces the given salt. (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. __ + __ -> __ Rb2SO4 (aq) + __H2O (l) a. __ + __ -> __CsNO3 (aq) + __H2O (l) a. __ + __ -> __ RbCl (aq) + __H2O (l)

In 1987 the first substance to act as a superconductor at a temperature above that of liquid nitrogen (77 K) was discovered. The approximate formula of this substance is YBa2Cu3O7. Calculate the percent composition by mass of this material.

The following molecular equation represents the reaction that occurs when aqueous solutions of silver(I) nitrate and manganese(II) iodide are combined. 2AgNO3 (aq) + MnI₂ (aq) —2AgI (s) + Mn(NO3)2 (aq) Write the balanced net ionic equation for the reaction.

Express the composition of each of the following compounds as the mass percents of its elements. a. acetone, C3H6O Mass% C = Mass% H= Mass% O = b. glycerol, C3 Hg O3 Mass% C= Mass% H = Mass% 0 =

A solution was prepared by mixing 60.00 mL of 0.100 M HNO3 and 180.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere while leaving a residue of pure mercury. Heating 0.3249 g of one of the compounds leaves a residue of 0.3009 g. Heating 0.2086 g of the other compound results in a mass loss of 0.008 g. a Determine the empirical formula of the first compound. Formula: b Determine the empirical formula of the second compound. Formula:

A 11.0 g sample of an aqueous solution of hydrochloric acid contains an unknown amount of the acid. If 11.3 mL of 2.08 M potassium hydroxide are required to neutralize the hydrochloric acid, what is the percent by mass of hydrochloric acid in the mixture?

Freon-12 (CCl₂F₂) is used as a refrigerant in air conditioners and as a propellant in aerosol cans. alculate the number of molecules of Freon-12 in 5.90 mg of Freon- What is the mass of chlorine in 5.90 mg of Freon-12?

A compound is found to contain 34.60 % chlorine, 46.85 % oxygen, and 18.55 % fluorine by mass. The empirical formula for this compound is The molar mass for this compound is 102.5 g/mol. The molecular formula for this compound is

Nickel (Ni) is a metal that is added to steel to improve its resistance to corrosion. Calculate both the number of moles in a sample of nickel containing 8.39 × 10^20 atoms and the mass of the sample.

An element consists of 0.19% of an isotope with mass 135.907 u, 0.25% of an isotope with mass 137.9060 u, 88.45% of an isotope with mass 139.9054 u, and 11.11% of an isotope with mass 141.9092 u. Calculate the average atomic mass, and identify the element.

The next step is to see if an insoluble product can form from the ions available. We do this by xchanging or "crossing" the ions in the reactants. This gives Ag2CO3 and KNO3. Are either of these insoluble? Ag¹(aq) + NO3 ¯(aq) + K*(aq) + CO3 ²¯(aq) → (Select all that apply.) KNO3 Ag2CO3

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

Which of the statements below is NOT part of the scientific method? observation and measurement testing of a hypothesis by experimentation refinement of a hypothesis as needed formation of a hypothesis All of the above steps are part of the scientific method.

What volume of 0.100 M Na3PO4 is required to precipitate all the lead(II) ions from 200.0 mL of 0.400 M Pb(NO3)2?

Si Br(l) + 2Ba(s) → 2BaBr₂ (s) + Si(s) Reducing Agent Substance Oxidized Substance Reduced Be(OH)2 (aq) → BeO₂ (aq) + 2H₂O(1) Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced

What volume of each of the following acids will react completely with 50.00 mL of 0.100 M NaOH? a. 0.150 M HCl Volume = b. 0.250 M HNO3 Volume = mL Volume = mL c. 0.100 M HC₂H3 O₂ (1 acidic hydrogen) mL

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

A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC₂H3O2), is titrated with 0.5502 M NaOH, and 20.00 mL is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is 1.006 g/cm³, what is the mass percent of acetic acid in the vinegar?

Categorize the following statement as observation, law, or theory: The mass of a gas that will dissolve in a liquid is directly proportional to the pressure of the gas. observation law theory

The equation for the production of methane is C + 2H₂(g) → CH4(g). How many grams of hydrogen are needed to produce 44.8 liters of methane at 273 K and 760 mm Hg? a. 2.0 g b. 4.0 g c. 6.0 g d. 8.0 g e. 89.6

Salespeople often deal with hundreds of different people and firms over time is indicative of which reason to choose a career in sales. a. Freedom b. Job challenge c. Rewards d. Opportunities of advancement

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:

Write the net ionic equation for the precipitation of magnesium sulfide from aqueous solution.

Write the net ionic equation for the following molecular equation. Ag₂SO4(aq) + (NH4)2CO3(aq) → Ag₂CO3(s) + (NH4)2SO4(aq)