Preparation and Properties of Compounds Questions and Answers

A chemist prepares a solution of zinc nitrate (Zn(NO3)₂) by measuring out 113. μmol of zinc nitrate into a 300. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in μmol/L of the chemist's zinc nitrate solution. Round your answer to 3 significant digits.

A chemist prepares a solution of potassium iodide (KI) by measuring out 6.1 × 10² μmol of potassium iodide into a 500. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's potassium iodide solution. Round your answer to 2 significant digits.

A chemist prepares a solution of calcium bromide (CaBr₂) by measuring out 57. μmol of calcium bromide into a 150. mL volumetric flask and filling the flask to the mark with water." Calculate the concentration in mol/L of the chemist's calcium bromide solution. Round your answer to 2 significant digits.

What is the mass of boron (in g) in a 27.5g sample of boric acid, B(OH)3? Note: For the formula weight, use the values from our periodic table. Round your answer to 4 significant figures, do not include units.

How many electrons are transferred in the following oxidation-reduction reaction? Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) a. 1 b. 3 C. 4 d. 2 e. 5

Ammonia is produced by the millions of tons annually for use as a fertilizer. It is commonly made from N₂ and H₂ by the Haber process. Because the reaction reaches equilibrium before going completely to product, the stoichiometric amount of ammonia is not obtained. At a particular temperature and pressure, 10.0 g of H₂ reacts with 20.0 g of N₂ to form ammonia. When equilibrium is reached, 15.0 g of NH3 has formed. (a) Calculate the percent yield. (b) How many moles of N₂ and H₂ are present at equilibrium?

Consider the following chemical reaction: 3 H₂ + N₂ --> 2 NH3 If 3.50 g of H₂ reacts with 21.0 g of N₂ to produce 18.8 g of NH3, what is the percent yield of NH3? Molar mass: for the hydrogen atom, H, must use 1.008 g/mol and for the nitrogen atom, N, use 14.01 g/mol Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal place.

Complete and balance the molecular equation for the reaction of aqueous chromium(II) bromide, CrBr₂, and aqueous sodium carbonate, Na₂CO3. Include physical states. molecular equation: Enter the balanced net ionic equation for the reaction. Include physical states. net ionic equation:

A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of product. Calculate the empirical formula of the iron sulfide.

Even though thermodynamically favourable, the conversion of diamond into graphite does not occur normally since. the activation energy of the process is high. the activation energy of the process is low. the change of entropy is zero. the change of enthalpy is zero.

Gaseous butane (CH₂(CH₂)2CH₂) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 0.58 g of butane is mixed with 3.91 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: BrO3-, CH3CO₂-, Fe3+, NH4+

A 25.00 mL sample of 6.00 M HCl solution is diluted to a new volume of 85.00 mL. What is the concentration of the dilute solution? 0.568 M 2.82 M 2.04 M 1.76 M I DON'T KNOW YET

A solution involves an attraction between the solute, the substance being dissolved, and the solvent, the substance that does the dissolving. This attraction is based on the polarity of the solute and the solvent. a. If both the solute and the solvent are polar, the solute will dissolve in the solvent. The same can also be said the solute and the solvent are nonpolar. This results in the formation of a solution. b. However, if the solute and the solvent have differing polarities (i.c., one is polar and the other is nonpolar), they will not dissolve in one another, and a solution will not form. Which substance will dissolve in water? CCI4 C4H10 CH3OH BF3 I DON'T KNOW YET

An inorganic compound (A) is white and exist as dimer. (A)Get sublimes on Heating (A)Gives fumes (B) with wet air (A) Gives white ppt with NH₂OH. However (A) Is soluble in excess of NaOH to give soluble compound (C) The inorganic compound 'A's Al₂O3 AlBr3 AICI 3 BeCl₂ An inorganic compound (A) is white and exist as dimer. (A)Get sublimes on Heating (A)Gives fumes (B) with wet air (A) Gives white ppt with NH₂OH. However (A) Is soluble in excess of NaOH to give soluble compound (C) The soluble compound (C) NaBO₂ NaAlO₂ Al₂O3 Al(OH)3

(CH₂(CH₂)4CH3) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 37.9 g of hexane is mixed with 99. g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.

In a solution of pure water, the dissociation of water can be expressed by the following: H₂O(l) + H₂O(l) H₂O'(aq) + OH(aq) The equilibrium constant for the ionization of water, K, is called the ion-product of water. In pure water at 25 °C, K has a value of 1.0 10¹. The dissociation of water gives one H₂O' ion and one OH ion and thus their concentrations are equal. The concentration of each is 1.0 x 10 M. K - [HO][OH^] K(1.0 10 )(1.0 × 10) - 1.0 × 10 ¹¹ X X [H₂O'][OH]- 1.0 × 10 ¹ X A solution has a [OH ]-3.4 10 M at 25 °C. What is the [HO] of the solution? O O 2.9 × 109 M X 3.4 × 10⁹ M 2.9 × 10-¹5 M 2.9 × 10 10 M I DON'T KNOW YET

Hydrogen sulfide gas (H₂S) and aqueous iron(II) chloride are formed by the reaction of aqueous hydrochloric acid (HCI) and solid iron(II) sulfide

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.

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.

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

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

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

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

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

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 _____

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.

Watch the video to determine which of the following relationships are correct according to Boyle's law. Check all that apply. V ∝ P P ∝ 1/V V ∝ 1/P PV ∝ V PV ∝ P P ∝ V

Write the empirical formula of at least four binary ionic compounds that could formed from the following ions: Ca²+, Cr4+, I-, O²-

Consider a 9.02 g sample of C3H6. How many atoms of C would be in this sample?

A photon having a wavelength in eV. (1 eV = 1.602 x 10^-19 J) of 437 nm strikes a metal surface having a threshold frequency of 3.23 x 10^14 Hz

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids. MgCO3(s)

Consider a 8.12 g sample of C4H10. How many molecules are in this sample?

When aqueous solutions of lead(II) nitrate and potassium carbonate are combined, solid lead(II) carbonate and a solution of potassium nitrate are formed.

Cyclohexene reacts with oxygen to produce carbon dioxide and water by the following balanced chemical reaction. 2 C6H10(l) + 17 O2 (g) → 12 CO2 (g) + 10 H₂O (l) a. If 59.0. grams of O2 is reacted with 24.5 grams of C6H10, which is the limiting reagent? Limiting reagent b. How many grams of H20 will be produced? Grams If 10.2 grams of H₂O are produced, what is the % yield for the reaction? % yield (10 points)