Inorganic Chemistry Questions

Consider the reaction: Br2(g) + Cl₂(g) → 2BrCl(g) Given an initial mass of 19.86 g Br2, an excess of Cl₂, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of BrCl produced by the reaction.

What is the oxidation state of each element in Mn(CrO4)₂?

Calculate the mass of gold (III) chloride (Au2Cl6) that contains a million (1.0 × 10^6) chlorine atoms. Be sure your answer has a unit symbol if necessary, and round it to 2 significant digits.

Consider the following unbalanced equation: C2H6(g)+Oz(g)→ CO2(g)+H2O(g) Which amount requires more oxygen gas, 2.43 mol C₂H6 or 28.8 g C₂H6? HOW DO WE GET THERE? For 2.43 mol C₂H6: What is the mole ratio between C₂H6 and O₂ in the balanced equation? 2C2H6(g) + 702(g) → 4CO2(g) + 6H₂O(g) X = Y = X mol O₂ Y mol C₂H6 mol O₂ mol C₂H6

Calculate the number of oxygen atoms in a 60.0 g sample of diphosphorus pentoxide (P₂O5). Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits.

Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting hematite with carbon monoxide, CO, in a blast furnace. Carbon monoxide is formed in the furnace by partial combustion of carbon. The reaction is Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) How many grams of iron can be produced from 1.62×103 g Fe2O3 reacting with an excess of CO? HOW DO WE GET THERE? How many moles are present in 1.62×10³ g of Fe₂O3(s)? mol Fe2O3(s)

Calculate the number of oxygen atoms in a 130.0 g sample of dinitrogen tetroxide (N₂O4). Be sure your answer has a unit symbol if necessary, and round it to 4 significant digits.

This is the chemical formula for nickel tetracarbonyl (a powerfully poisonous liquid used in nickel refining): Ni(CO)4 A chemical engineer has determined by measurements that there are 4.277 moles of carbon in a sample of nickel tetracarbonyl. How many moles of oxygen are in the sample? Round your answer to 4 significant digits.

Calculate the number of hydrogen atoms in a 80.0 g sample of ammonia (NH3).

Calculate the number of oxygen atoms in a 80.0 g sample of forsterite (Mg2SiO4). Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits.

You have a solution that is 18.5% (v/v) methyl alcohol. If the bottle contains 1.09 L of solution, what is the volume (V) in milliliters of methyl alcohol? Express your answer with the appropriate units.

Measurements show that unknown compound X has the following composition: element mass % nitrogen 26.0% oxygen 74.1% Write the empirical chemical formula of X.

Consider the following unbalanced equation: C2H6(g) + O2(g) → CO₂(g) + H₂O(g) Which amount requires more oxygen gas, 2.43 mol C₂H6 or 28.8 g C2H6? HOW DO WE GET THERE? For 28.8 g C2H6: How many moles are present in 28.8 g C₂H6? mol C₂H6

Molarity is one of the most commonly used concentration units for solutions and is abbreviated as "M". Molarity is calculated by determining the number of moles of the solute, or the substance being dissolved, in 1 liter of solution. In other words, molarity is the number of moles/liter. This is summarized as follows: Molarity (M)= moles of solute/1 L of solution What is the molarity of a solution prepared from 34.5 grams of NaCl in 250.0 milliliters of solution? 0.138 M NaCl 6.78 M NaCl 2.36 M NaCl 0.424 M NaCl I DON'T KNOW YET

Consider the following unbalanced equation: NH3(g) → N₂(g) + H₂(g) How many moles of N₂ will be produced by the decomposition of 4.06 moles of ammonia? How many moles of N₂ are produced from 4.06 mol NH3? mol N₂

A flask contains 0.015 mol of HCl in 10.0 mL of water. a. What is the molarity of the HCl solution? b. In a titration with NaOH, how many moles of NaOH will be required to reach the end point?

A 6.00 % (m/v) NaCl solution contains 18.2 g of NaCl. What is the total volume (V) of the solution in milliliters? Express your answer with the appropriate units.

A solution containing 1.63 g of barium chloride is added to a solution containing 2.40 g of sodium chromate (chromate ion, CrO2). Determine which reactant is in excess. Find the number of grams of barium chromate that can precipitate.

strong electrolyte weak electrolyte nonelectrolyte A 20 mL solution containing 2 mmol of HBr(g) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb produced a bright glow. HBr (g) is a A 20 mL solution containing 2 mmol of C12H22O11 (aq) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb remained off. C12H22O11 (aq) is a A 20 mL solution containing 2 mmol of Ca3(PO4)2 (s) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb faintly flickered. Ca3(PO4)2 (s) is a A 20 mL solution containing 2 mmol of CH3NH₂(1) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb produced a dim glow. CH3NH₂(l) is a

For the following reaction, 9.37 grams of glucose (C6H12O6) are allowed to react with 13.6 grams of oxygen gas. glucose (C6H12O6)(s) + oxygen(g) → carbon dioxide(g) + water(l) What is the maximum amount of carbon dioxide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?

Consider the following fictional element and polyatomic ions: Tb = tiberium (a "complex" transition metal, i.e. forms type II ionic compounds) TbO2- = tiberite TbO3- = tiberate What would be the name of the following compounds: Tbo tiberium (II) HTbO3 HTbO2 HTbO

What did Ernest Rutherford discover and what were there charges? He discovered the nucleus contained electrons. He discovered the nucleus contained protons. The electrons possessed a negative charge. The protons possessed a positive charge.

For the following reaction, 5.23 grams of nitrogen gas are allowed to react with 9.15 grams of oxygen gas. nitrogen (g) + oxygen(g) ---> nitrogen monoxide(g) What is the maximum mass of nitrogen monoxide that can be formed? What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete?

"In our bodies, sugar is broken down with oxygen to produce water and carbon dioxide." According to the following reaction: C6H12O6 (s) + 6O₂ (g) → 6CO2 (g) + 6H₂O (l) What would you multiply "moles of glucose (C6H1206)" by to convert to the units "moles of water"?

For the following reaction, 25.7 grams of sulfur dioxide are allowed to react with 5.54 grams of oxygen gas. sulfur dioxide (g) + oxygen (g) → sulfur trioxide (g) What is the maximum amount of sulfur trioxide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?

Interpret the following equation for a chemical reaction using the coefficients given: C₂H4(g) + Br2(g) CH₂BrCH₂Br(g) On the particulate level: of C₂H4(g) reacts with of Br2(g) to form of CH₂BrCH₂Br(g). On the molar level: of C₂H4(g) reacts with of Br2(g) to form of CH₂BrCH₂Br(g).

Determine the ionic compound that forms between the given elements. a. Calcium and chlorine b. Potassium and iodine c. Aluminum and sulfur d. Cesium and nitrogen e. Magnesium and nitrogen f. Aluminum and phosphorus g. Zinc and chlorine h. Silver and bromine

Which of the following are properties of alkali metals? mostly solids, dull, brittle reactive, conductors mostly solids, luster, high density, conductors mostly gases, brittle, dull, low density, insulators solids, luster, malleable, conductors, reactive

Name the following compounds: (a) NaH (b) KMnO4 (c) Ag₂CO3 (d) LizN

Given that the following reaction is a precipitation reaction, find the precipitate and the filtrate respectively? 2AgNO3(aq) + CaCl₂(aq) → 2AgCl (s)+ Ca(NO3)2 (aq) A. CaCl2, Ca(NO3)2- B. AgCl, Ca(NO3)2- C. CaCl2, Ca(NO3)2- D. AgNO3, CaCl2.

(2 points) Phosphonic acid (H3PO3), also known as phosphorous acid, is a diprotic acid. Infrared spectroscopy and nuclear magnetic resonance results indicate that its structure is consistent with the formula OPH(OH)2. With this information, write the correct Lewis structure.

The rusting of iron is represented by the equation: 4Fe +302 --> 2Fe₂O3 If you have a 1.45-mol sample of iron, how many moles of Fe₂O3 will there be after the iron has rusted completely? 0.483 mol 2.175 mol 0.967 mol 0.725 mol 1.45 mol

Refer to the following equation: 4 NH3 (g) + 7 O₂ (g) --> 4 NO₂ (g) + 6 H₂O(g) How many moles of ammonia will be required to produce 11.9 mol of water? 11.9 mol 5.95 mol 7.93 mol 4.76 mol none of these options

Balance the equation below using the smallest possible whole-number stoichiometric coefficients. For the balanced equation, what is the coefficient in front of the reactant O2? C3H6O + O2 -> CO2 + H2O

The sun supplies about 1.1 kilowatt(s) of energy for each square meter of surface area (1.1 kW/m², where a watt = 1 J/s). Plants produce the equivalent of about 0.22 g of sucrose ( C12 H22 O11) per hour per square meter. 12CO2 (g) + 11H₂O (1)→C12H22O11 + 1202 (g) ΔH = 5645kJ Express your answer using two significant figures.

Consider the following chemical reaction: 4 NH3 + 7O2 -> 2 N₂O4 + 6H₂O Identify the limiting reagent when 6.25 mol of NH3 reacts with 10.3 mol of O2. Assume the reaction goes to completion. Select one: O2 NO2 H₂O NH3 Both NH3 and O2 are used up at the same time

In two or more complete sentences, describe how one of the occupations that you studied would use descriptive statistics when performing their job. Justify your answers in two or more complete sentences.

The ionization energy of sodium is 496 kJ/mol. What is the minimum frequency of light required to ionize one electron from one atom of sodium? 2.56 x 10^14 S^-1 6.31 x 10^15 S^-1 3.88 x 10^14 S^-1 8.63 x 10^13 S^-1 1.24 x 10^15 S^-1

What is the electrostatic potential energy (in joules) between an electron and a proton that are separated by 45 pm?

Does a reaction occur when aqueous solutions of calcium chloride and ammonium sulfate are combined? yes/no If a reaction does occur, write the net ionic equation.

In the manufacture ofr NaOH by electrolysis of an aqueous solution of sodium chloride, the cathode and anode are separated by using a diaphragm or slate partitions because it increases the yield of Cl2 it prevents the reaction taking place between NaOH and Cl₂ it prevents the mixing of NaOH and NaCl it prevents the reaction taking place between Na and Cl2

Using the combined gas law, we solve for P2 by multiplying both sides by _______dividing both sides by _________ The expression obtained is P1V1/T1 x _____ = P2V2 x _____ Finally, P₂ = P₁ x _____

A metallurgist has one alloy containing 44 % aluminum and another containing 70 % aluminum. How many pounds of each alloy must he use to make 48 pounds of a third alloy containing 64 % aluminum? (Round to two decimal places if necessary.)

Which of the following property of magnesium does not resemble with lithium? Bicarbonates of both exist in solution state but not in solidform Carbonates of both produce CO₂ on heating Both can produce nitride on reaction with N₂ Both can be identified by flame colour test

Does a reaction occur when aqueous solutions of barium nitrate and magnesium sulfate are combined? yes / no If a reaction does occur, write the net ionic equation.

The density of titanium is 4.50 g/cm³. A pure titanium cube contains 8.96x 10^23 atoms. What is the edge length of this cube in cm? Provide answer to the correct number of significant figures.

For the molecular compound sulfur dioxide, what would you multiply "grams of SO₂ " by to get the units "molecules of SO₂ " ?

Decide whether each pair of elements in the table below will form an ionic compound. If they will, write the empirical formula and name of the compound formed in the spaces provided.

In the photoelectric effect experiment, light shines on a metal and no electrons are emitted from its surface. Which of the following changes might result in electrons emitted from the metal surface? Check all that apply. Use light of the same frequency but with higher intensity (brighter). Use light of a lower wavelength. Use a different metal surface with a metal having lower binding energy. Use light of a lower frequency.

A certain gas is present in a 13.0 L cylinder at 4.0 atm pressure. If the pressure is increased to 8.0 atm, the volume of the gas decreases to 6.5 L. Find the two constants k₁, the initial value of k, and ke, the final value of k, to verify whether the gas obeys Boyle's law. Express your answers to two significant figures separated by a comma.