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chemistry
physical chemistry
Questions and Answers of
Physical Chemistry
There are 1.699 × 1022 atoms in 1.000 g of chlorine. Assume that chlorine atoms are spheres of radius 0.99 Å and that they are lined up side by side. How many miles in length is the line of
A sample of green crystals of nickel(II) sulfate heptahydrate was heated carefully to produce the bluish green nickel(II) sulfate hexahydrate. What are the formulas of the hydrates? If 8.753 g of the
Cobalt(II) sulfate heptahydrate has pink-colored crystals. When heated carefully, it produces cobalt(II) sulfate monohydrate, which has red crystals. What are the formulas of these hydrates? If 3.548
A sample of metallic element X, weighing 3.177 g, combines with 0.6015 L of O2 gas (at normal pressure and 20.0oC) to form the metal oxide with the formula XO. If the density of O2 gas under these
A sample of metallic element X, weighing 4.315 g, combines with 0.4810 L of Cl2 gas (at normal pressure and 20.0oC) to form the metal chloride with the formula XCl. If the density of Cl2 gas under
What is the difference between a molecular formula and a structural formula?
What is the fundamental difference between an organic substance and an inorganic substance? Write chemical formulas of three inorganic molecules that contain carbon.
Which of the following models represent a(n):a. Elementb. Compoundc. Mixtured. Ionic solide. Gas made up of an element and a compoundf. Mixture of elementsg. Solid elementh. Solidi. Liquid
The compounds CuCl and CuCl2 were formerly called cuprous chloride and cupric chloride, respectively. What are their names using the Stock system of nomenclature? What are the advantages of the Stock
Two compounds of iron and chlorine, A and B, contain 1.270 g and 1.904 g of chlorine, respectively, for each gram of iron. Show that these amounts are in the ratio 2: 3. Is this consistent with the
Part 1: Consider the four identical spheres below, each with a mass of 2.00 g.Calculate the average mass of a sphere in this sample. Part 2: Now consider a sample that consists of four spheres, each
Consider the following depictions of two atoms, which have been greatly enlarged so you can see the subatomic particles.a. How many protons are present in atom A? b. What is the significance of the
One of the early models of the atom proposed that atoms were wispy balls of positive charge with the electrons evenly distributed throughout. What would you expect to observe if you conducted
A friend is trying to balance the following equation: N2 + H2 → NH3 He presents you with his version of the “balanced” equation: N + H3 → NH3 You immediately recognize that he has committed a
Explain the operation of a cathode-ray tube. Describe the deflection of cathode rays by electrically charged plates placed within the cathode-ray tube. What does this imply about cathode rays?
You discover a new set of polyatomic anions that has the newly discovered element “X” combined with oxygen. Since you made the discovery, you get to choose the names for these new polyatomic
You have the mythical metal element “X” that can exist as X+, X2+, and X5+ ions.a. What would be the chemical formula for compounds formed from the combination of each of the X ions and SO42?b.
Match the molecular model with the correct chemical formula: CH3OH, NH3, KCl, H2O.
Consider a hypothetical case in which the charge on a proton is twice that of an electron. Using this hypothetical case, and the fact that atoms maintain a charge of 0, how many protons, neutrons,
Currently, the atomic mass unit (amu) is based on being exactly one-twelfth the mass of a carbon-12 atom and is equal to 1.66 × 10–27 kg. a. If the amu were based on sodium-23 with a mass equal to
For each of the following chemical reactions, write the correct element and/or compound symbols, formulas, and coefficients needed to produce complete, balanced equations. In all cases, the reactants
You perform a chemical reaction using the hypothetical elements A and B. These elements are represented by their molecular models shown below:The product of the reaction represented by molecular
What is the name of the element represented by each of the following atomic symbols? a. Ar b. Zn c. Ag d. Mg
For each atomic symbol, give the name of the element. a. Ca b. Cu c. Hg d. Sn
Give the atomic symbol for each of the following elements. a. Potassium b. Sulfur c. Iron d. Manganese
Explain Millikan’s oil-drop experiment.
Give the atomic symbol for each of the following elements. a. Carbon b. Sodium c. Nickel d. Lead
A student has determined the mass-to-charge ratio for an electron to be 5.64 × 10–12 kg/C. In another experiment, using Millikan’s oil-drop apparatus, he found the charge on the electron to be
The mass-to-charge ratio for the positive ion F+ is 1.97 × 10–7 kg/C. Using the value of 1.602 × 10–19 C for the charge on the ion, calculate the mass of the fluorine atom. (The mass of the
Naturally occurring chlorine is a mixture of the isotopes Cl-35 and Cl-37. How many protons and how many neutrons are there in each isotope? How many electrons are there in the neutral atoms?
Naturally occurring lithium is a mixture of 63Li and 73Li. Give the number of protons, neutrons, and electrons in the neutral atom of each isotope.
Ammonia is a gas with a characteristic pungent odor. It is sold as a water solution for use in household cleaning. The gas is a compound of nitrogen and hydrogen in the atomic ratio 1: 3. A sample of
Describe the nuclear model of the atom. How does this model explain the results of alpha-particle scattering from metal foils?
Hydrogen sulfide is a gas with the odor of rotten eggs. The gas can sometimes be detected in automobile exhaust. It is a compound of hydrogen and sulfur in the atomic ratio 2 : 1. A sample of
Calculate the atomic mass of an element with two naturally occurring isotopes, from the following data:What is the identity of element X?
An element has two naturally occurring isotopes with the following masses and abundances: Isotopic Mass (amu) Fractional Abundance 49.9472…………………. 2.500 ×
An element has three naturally occurring isotopes with the following masses and abundances: Isotopic Mass (amu) Fractional Abundance 38.964………………………………
An element has three naturally occurring isotopes with the following masses and abundances: Isotopic Mass (amu) Fractional
While traveling to a distant universe, you discover the hypothetical element X.You obtain a representative sample of the element and discover that it is made up of two
While roaming a parallel universe, you discover the hypothetical element Z. You obtain a representative sample of the element and discover that it is made up of two isotopes,
Identify the group and period for each of the following. Refer to the periodic table. Label each as a metal, nonmetal, or metalloid. a. C b. Po c. Cr d. Mg e. B
Refer to the periodic table and obtain the group and period for each of the following elements. Also determine whether the element is a metal, nonmetal, or metalloid. a. S b. Fe c. Ba d. Cu e. Ne
What are the different kinds of particles in the atom’s nucleus? Compare their properties with each other and with those of an electron.
Give one example (atomic symbol and name) for each of the following. a. A main-group (representative) element in the second period b. An alkali metal c. A transition element in the fourth period d. A
Give one example (atomic symbol and name) for each of the following. a. A transition element in the fifth period b. A halogen c. A main-group (representative) element in the second period d. An
The normal form of the element sulfur is a brittle, yellow solid. This is a molecular substance, S8. If this solid is vaporized, it first forms S8 molecules; but at high temperature, S2 molecules are
White phosphorus is available in sticks, which have a waxy appearance. This is a molecular substance, P4. When this solid is vaporized, it first forms P4 molecules; but at high temperature, P2
A 1.50-g sample of nitrous oxide (an anesthetic, sometimes called laughing gas) contains 2.05 × 1022 N2O molecules. How many nitrogen atoms are in this sample? How many nitrogen atoms are in 1.00 g
Nitric acid is composed of HNO3 molecules. A sample weighing 4.50 g contains 4.30 × 1022 HNO3 molecules. How many nitrogen atoms are in this sample? How many oxygen atoms are in 2.81 g of nitric
A sample of ammonia, NH3, contains 3.3 × 1021 hydrogen atoms. How many NH3 molecules are in this sample?
A sample of ethanol (ethyl alcohol), C2H5OH, contains 4.2 × 1023 hydrogen atoms. How many C2H5OH molecules are in this sample?
Give the molecular formula for each of the following structural formulas.a.b. c. d.
Describe how protons and neutrons were discovered to be constituents of nuclei.
What molecular formula corresponds to each of the following structural formulas?a.b. c. d.
Write the molecular formula for each of the following compounds represented by molecular models.
Write the molecular formula for each of the following compounds represented by molecular models.
Iron(II) nitrate has the formula Fe(NO3)2. What is the ratio of iron atoms to oxygen atoms in this compound?
Ammonium phosphate, (NH4)3PO4, has how many hydrogen atoms for each oxygen atom?
Write the formula for the compound of each of the following pairs of ions.a. Fe3+ and CNb. K+ and SO42c. Li+ and N3d. Ca2+ and P3
For each of the following pairs of ions, write the formula of the corresponding compound. a. Co2+ and N3 b. NH4+ and PO43 c. Na+ and CO32 d. Fe3+ and OH
Name the following compounds. a. Na2SO4 b. CaS c. CuCl d. Cr2O3
Name the following compounds.a. Na2Ob. MN2O3c. NH4HCO3d. Cu(NO3)2
Write the formulas of: a. Lead(II) permanganate b. Barium hydrogen carbonate c. Cesium sulfide d. Iron(II) acetate
Write the formulas of: a. Sodium thiosulfate b. Copper(I) hydroxide c. Calcium hydrogen carbonate d. Nickel(II) phosphide
For each of the following binary compounds, decide whether the compound is expected to be ionic or molecular. a. SeF4 b. LiBr c. SiF4 d. Cs2O
For each of the following binary compounds, decide whether the compound is expected to be ionic or molecular. a. AlN b. As4O6 c. ClF3 d. Fe2O3
Give systematic names to the following binary compounds. a. N2O b. P4O10 c. AsCl3 d. Cl2O7
Give systematic names to the following binary compounds. a. N2F2 b. CCl4 c. N2O5 d. As4O6
Write the formulas of the following compounds. a. Nitrogen tribromide b. Xenon tetroxide c. Oxygen difluoride d. Dichlorine pentoxide
Write the formulas of the following compounds. a. Chlorine trifluoride b. Nitrogen dioxide c. Dinitrogen tetrafluoride d. Phosphorus pentafluoride
Give the name and formula of the acid corresponding to each of the following oxoanions. a. Bromate ion, BrO3 b. Hyponitrite ion, N2O22 c. Disulfite ion, S2O52 d. Arsenate ion, AsO43
Describe how Dalton obtained relative atomic masses.
Give the name and formula of the acid corresponding to each of the following oxoanions. a. Selenite ion, SeO32 b. Sulfite ion, SO32 c. hypoiodite ion, IO d. nitrite ion, NO2
For the balanced chemical equation Pb(NO3)2 + K2CO3 → PbCO3 + 2KNO3, how many oxygen atoms are on the left side?
In the equation 2PbS + O2 → 2PbO + 2SO2, how many oxygen atoms are there on the right side? Is the equation balanced as written?
Balance the following equations. a. Sn + NaOH → Na2SnO2 + H2 b. Al + Fe3O4 → Al2O3 + Fe c. CH3OH + O2 → CO2 + H2O d. P4O10 + H2O → H3PO4 e. PCl5 + H2O → H3PO4 + HCl
Balance the following equations. a. Cl2O7 + H2O → HClO4 b. MnO2 + HCl → MnCl2 + Cl2 + H2O c. Na2S2O3 + I2 → NaI + Na2S4O6 d. Al4C3 + H2O →Al(OH)3 + CH4 e. NO2 + H2O → HNO3 + NO
Solid calcium phosphate and aqueous sulfuric acid solution react to give calcium sulfate, which comes out of the solution as a solid. The other product is phosphoric acid, which remains in solution.
Determine whether the following compounds are soluble or insoluble in water. a. NaBr b. Ba(OH)2 c. Calcium carbonate
A sample of sodium chloride, NaCl, weighing 0.0678 g is placed in a 25.0-mL volumetric flask. Enough water is added to dissolve the NaCl, and then the flask is filled to the mark with water and
How many milliliters of 0.163 M NaCl are required to give 0.0958 g of sodium chloride?
How many moles of sodium chloride should be put in a 50.0-Ml volumetric flask to give a 0.15 M NaCl solution when the flask is filled to the mark with water? How many grams of NaCl is this?
You have a solution that is 1.5 M H2SO4 (sulfuric acid). How many milliliters of this acid do you need to prepare 100.0 mL of 0.18 M H2SO4?
You are given a sample of limestone, which is mostly CaCO3, to determine the mass percentage of Ca in the rock. You dissolve the limestone in hydrochloric acid, which gives a solution of calcium
Nickel sulfate, NiSO4, reacts with sodium phosphate, Na3PO4, to give a pale yellow-green precipitate of nickel phosphate, Ni3(PO4)2, and a solution of sodium sulfate, Na2SO4. 3NiSO4(aq) + 2Na3PO4(aq)
A 5.00-g sample of vinegar is titrated with 0.108 M NaOH. If the vinegar requires 39.1 mL of the NaOH solution for complete reaction, what is the mass percentage of acetic acid, HC2H3O2, in the
Write complete ionic and net ionic equations for each of the following molecular equations. a. 2HNO3(aq) + Mg(OH)2(s) → 2H2O(l) + Mg(NO3)2(aq) Nitric acid, HNO3, is a strong electrolyte. b.
You mix aqueous solutions of sodium iodide and lead(II) acetate. If a reaction occurs, write the balanced molecular equation and the net ionic equation. If no reaction occurs, indicate this by
Label each of the following as a strong or weak acid or base: a. H3PO4 b. HClO c. HClO4 d. Sr(OH)2
Write the molecular equation and the net ionic equation for the neutralization of hydrocyanic acid, HCN, by lithium hydroxide, LiOH, both in aqueous solution.
Write molecular and net ionic equations for the successive neutralizations of each of the acidic hydrogens of sulfuric acid with potassium hydroxide. (That is, write equations for the reaction of
Write the molecular equation and the net ionic equation for the reaction of calcium carbonate with nitric acid.
Obtain the oxidation numbers of the atoms in each of the following: (a) Potassium dichromate, K2Cr2O7. (b) Permanganate ion, MnO4.
Use the half-reaction method to balance the equation Ca(s) + Cl2(g) → CaCl2(s).
LiI(s) and CH3OH(l) are introduced into separate beakers containing water. Using the drawings shown here, label each beaker with the appropriate compound and indicate whether you would expect each
Your lab partner tells you that she mixed two solutions that contain ions. You analyze the solution and find that it contains the ions and precipitate shown in the beaker. a. Write the molecular
At times, we want to generalize the formula of certain important chemical substances; acids and bases fall into this category. Given the following reactions, try to identify the acids, bases, and
Consider the following beakers. Each contains a solution of the hypothetical atom X. a. Arrange the beakers in order of increasing concentration of X. b. Without adding or removing X, what specific
Consider three flasks, each containing 0.10 mol of acid. You need to learn something about the acids in each of the flasks, so you perform titration using an NaOH solution. Here are the results of
Explain why some electrolyte solutions are strongly conducting, whereas others are weakly conducting.
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