Concept explainers
(a)
Interpretation:
Amount in moles, number of molecules and formula units present in
(a)
Explanation of Solution
Number of moles of alumina:
Formula of alumina is given as
Thus the number of moles of alumina in
Number of molecules in alumina:
One mole of any substance contains
Thus the number of molecules of alumina in
Number of formula units:
As this is given species is a compound, the number of formula units will be equal to the number of molecules. Therefore, the number of formula units in
(b)
Interpretation:
Amount in moles, number of molecules and formula units present in
(b)
Explanation of Solution
Number of moles of hydrogen fluoride:
Formula of hydrogen fluoride is given as
Thus the number of moles of hydrogen fluoride in
Number of molecules in hydrogen fluoride:
One mole of any substance contains
Thus the number of molecules of hydrogen fluoride in
Number of formula units:
As this is given species is a compound, the number of formula units will be equal to the number of molecules. Therefore, the number of formula units in
(c)
Interpretation:
Amount in moles, number of molecules and formula units present in
(c)
Explanation of Solution
Number of moles of hydrogen peroxide:
Formula of hydrogen peroxide is given as
Thus the number of moles of hydrogen peroxide in
Number of molecules in hydrogen peroxide:
One mole of any substance contains
Thus the number of molecules of hydrogen peroxide in
Number of formula units:
As this is given species is a compound, the number of formula units will be equal to the number of molecules. Therefore, the number of formula units in
(d)
Interpretation:
Amount in moles, number of molecules and formula units present in
(d)
Explanation of Solution
Number of moles of glucose:
Formula of glucose is given as
Thus the number of moles of glucose in
Number of molecules in glucose:
One mole of any substance contains
Thus the number of molecules of glucose in
Number of formula units:
As this is given species is a compound, the number of formula units will be equal to the number of molecules. Therefore, the number of formula units in
(e)
Interpretation:
Amount in moles, number of molecules and atoms present in
(e)
Explanation of Solution
Number of moles of nitrogen:
The mass of nitrogen atom is
Thus the number of moles of nitrogen atoms in
Two atoms of nitrogen combines to give a molecule of nitrogen. Therefore, the number of moles of nitrogen molecule is calculated as shown below;
Thus the number of moles of nitrogen molecules in
Number of atoms or molecules in nitrogen:
One mole of any substance contains
Thus the number of atoms of nitrogen in
Two atoms of nitrogen combines to give a molecule of nitrogen. Therefore, the number of nitrogen molecule is calculated as shown below;
Thus the number of nitrogen molecules in
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Chapter F Solutions
CHEMICAL PRINCIPLES PKG W/SAPLING
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- You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.arrow_forward4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.arrow_forwardNitrogen fixation in the root nodules of peas and other legumes occurs with a reaction involving a molybdenum-containing enzyme named nitrogenase. This enzyme contains two Mo atoms per molecule and is 0.0872% Mo by mass. Calculate the molar mass of the enzyme.arrow_forward
- Chalky, white crystals in mineral collections are often labeled borax, which has the molecular formula Na2B4O7 10H2O, when actually they are partially dehydrated samples with the molecular formula Na2B4O7 5H2O, which is more stable under the storage conditions. Real crystals of borax are colorless and transparent. (a) Calculate the percent mass that the mineral has lost when it partially dehydrates. (b) Is the percent boron by mass the same in both compounds?arrow_forwardWhat is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury (II) chloride in the body and that a fatal dose is 0.20 g of HgCl2.) How many pounds of fish is this?arrow_forward
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