Calculating Molar Masses of Compounds Just add together the molar masses of all the elements in the compound (by Conservation of Mass). Distribute through the parentheses when necessary. - Ex 1) CCl,F, Ex 2) M9CO; *** - Ex 3) (NH4);PO4 - Ex 4) Sn3(PO4)4 *** Molar mass = 3 atoms Sn ( 118.7) + 1(4) ( 31) + 4(4) (16) = 736.1 g/ mole %3D

Calculating Molar Masses of Compounds Just add together the molar masses of all the elements in the compound (by Conservation of Mass). Distribute through the parentheses when necessary. - Ex 1) CCl,F, Ex 2) M9CO; * - Ex 3) (NH4);PO4 - Ex 4) Sn3(PO4)4 * Molar mass = 3 atoms Sn ( 118.7) + 1(4) ( 31) + 4(4) (16) = 736.1 g/ mole %3D

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter8: Chemical Composition

Section: Chapter Questions

Problem 87AP: A binary compound of magnesium and nitrogen is analyzed, and 1.2791 g of the compound ¡s found to...

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A binary compound of magnesium and nitrogen is analyzed, and 1.2791 g of the compound ¡s found to contain 0.9240 g of magnesium. When a second sample of this compound is treated with water and heated, the nitrogen is driven off as ammonia, leaving a compound that contains 60.31% magnesium and 39.69% oxygen by mass. Calculate the empirical formulas of the two magnesium compounds.
The compound As2I4 is synthesized by reaction of arsenic metal with arsenic triiodide. If a solid cubic block of arsenic (d = 5.72 g/cm3) that is 3.00 cm on edge is allowed to react with 1.01 1024 molecules of arsenic triiodide, what mass of As2I4 can be prepared? If the percent yield of As2I4 was 75.6%, what mass of As2I4 was actually isolated?
By x-ray diffraction it is possible to determine the geometric pattern in which atoms are arranged in a crystal and the distances between atoms. In a crystal of silver, four atoms effectively occupy the volume of a cube 0.409 nm on an edge. Taking the density of silver to be 10.5 g/cm3, calculate the number of atoms in one mole of silver.
The reaction of iron(III) oxide with aluminum to give molten iron is known as the thermite reaction (page 172). Fe2O3(s) + 2 Al(s) 2 Fe(l) + Al2O3(s) What amount of Al, in moles, is needed for complete reaction with 3.0 mol of Fe2O3? What mass of Fe, in grams, can be produced?
Suppose that Si28(1428Si) is taken as the standard for expressing atomic masses and assigned an atomic mass of 10.00 amu. Estimate the molar mass of sodium nitride.
Lead(II) chromate (PbCrO₄) is used as the yellow pigmentin traffic lanes, but is banned from house paint because of therisk of lead poisoning. It is produced from chromite (FeCr₂O₄),an ore of chromium:4FeCr₂O₄(s) +8K2CO3(aq)+ 7O₂(g)→2Fe₂O₃(s)+ 8K₂CrO₄(aq)+ 8CO₂(g) Lead(II) ion then replaces the Kion. If a yellow paint is0.511% PbCrO₄by mass, how many grams of chromite areneeded per kilogram of paint?
Chemical analysis shows that the oxygen-carryingprotein hemoglobin is 0.34 percent Fe by mass. What isthe minimum possible molar mass of hemoglobin? Theactual molar mass of hemoglobin is about 65,000 g.How would you account for the discrepancy betweenyour minimum value and the experimental value?
A new organic material is to be examined by combustion analysis. Burning 0.09303 g of this sample in the presence of excess oxygen gives an increase in mass of 0.04256 g on Mg(ClO4)2 and a 0.1387g increase in mass on a NaOH on asbestos. If we know carbon, hydrogen and oxygen are the only elements present, what is the percent C, H, and O in the sample?
EDTA, which is short forethylenediaminetetraacetic acid, is a chemical used inthe textile industry to prevent metal impurities fromchanging the colours of dyed products. Th e empiricalformula for EDTA is C5H8NO4. Th e molar mass ofEDTA is 292.24 g/mol. What is its molecular formula?
Fluorine is so reactive that it forms compounds with mate-rials inert to other treatments.(a) When 0.327 g of platinum is heated in fluorine, 0.519 g of adark red, volatile solid forms. What is its empirical formula?(b) When 0.265 g of this red solid reacts with excess xenon gas,0.378 g of an orange-yellow solid forms. What is the empiricalformula of this compound, the first to contain a noble gas?(c) Fluorides of xenon can be formed by direct reaction of the el-ements at high pressure and temperature. Under conditions thatproduce only the tetra- and hexafluorides, 1.85x10^-4mol ofxenon reacted with 5.00x10^-4mol of fluorine, and 9.00x10^-6mol of xenon was found in excess. What are the mass percents ofeach xenon fluoride in the product mixture?
AB4(aq) + 4CD(aq) --> AD4(s) + 4CB(aq) How many grams of AD4(s) (MW= 231.11 g/mol) would be made from the reaction of 2.36E24 molecules of CD(aq)(MW=238.90 g/mol), assuming excess AB4(aq)(235.57g/mol)
At the end of this, how did we go from a 5 to 1 ratio moles to 2CO2 and 3H2O?