Chapter 3 regular
what is the percentage by mass of nitrogen in calcium nitrate (Ca(NO3)2)
164.1 amu
Sodium hydroxide reacts with carbon dioxide to form sodium carbonate and water- how many grams Na2CO3 can be prepared from 2.40g of NaOH
3.18g-m
calculate the number of moves in glucose (C6H12)6) an a 5.380 g sample.
0.02989 mol C6H12O6
Determine how many grams of water are produced in the oxidation of 1.00 grams of glucose, C6H12O6
0.600g H2O
How many oxygen atoms are in this sample if 180g moles ammonium chloride 1.75 x 10^22 molecules C6H12O6
1.05 x 10^23 atoms O
How many O atoms are in this sample
1.20 x 10^23 atoms 'O'
How many glucose molecules are in 180g of C6H12O6
1.75 x 10^22 molecules C6H12O6
How many chlorine atoms are in 12.2 g of CCl4
1.91 x 10^23
calculate the percentage of potassium, by mass, in K2PtCl6
16.1%
Calculate the formula weight of calcium nitrateCa(NO3)2
164.1 amu
calculate the molar mass of Ca(NO3)2
164.1g/mol
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g) How many grans of NaN3 are required to form 11.0g of nitrogen gas?
17.0g
What is the molar mass of glucose C6H12O6
180.0 amu
How many sulfur atoms are in 1.10 mol of aluminum sulfide
19.9 x 10^23
a sample of an ionic compound containing iron and chlorine is analyzed and found to have a molar mass of 126.8g/mol. What is the charge of the iron in this compound
2+
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g) How many moles of N2 are produced by the decomposition of 1.60 mol of NaN3
2.40 mol
Calculate the number of H atoms in 0.350 mol of C6H12O8
2.53x 10^24 H atoms
how many sulfur atoms are in 0.45 mol BaSO4
2.7 x 10^23 atoms
How many oxygen atoms are in 1.50 mol of sodium carbonate
2.709 x 10^24 'O' atoms
An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g). Calculate the number of grams of CO that can react with 0.400kg of Fe2O3
210g
calculate the formula weight of tantalum oxynitride (TaON)
211.0 amu
what is the mass, in grams of 0.30 mol of sulfuric acid
25.2g NaHCO3
An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g). Calculate the number of grams of Fe formed when 0.400kg of Fe2)3 reacts
280g
Mesitylene, a hydrocarbon found in crude oil, has an empirical formula of C3H4 and an experimental determined molecular weight of 121 amu. What is its molecular formula?
3.03
When 1.57 mol O2 reacts with H2 to form H2O, how many moles of H2 are consumed in the process?
3.14 mol
Calculate the formula weight of calcium phosphate
310.3amu
calculate the formula weight of methanol (CH3OH)
32.0 amu
An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g). Calculate the number of grams of CO2 formed when 0.400 kg of Fe2O3 reacts
331g
Calculate the formula weight of sucrose C12H22,O111
342 amu
how many atoms are there in 3g of copper (Cu)
3x10^22 atoms
how many nitric acid molecules are in 4.20 g of HNO3
4.01 x 10^22 molecules HNO3
what is the percent composition of carbon in glucose?
40%
Decomposition of KCIO3 is sometimes used to prepare small amounts of O2 in the laboratory; 2KCIO39(s) -----> 2KCI(s) + 3O2(g). How many grams of O2 can be prepared from 4.50g of KCIO3
41.26%
Calculate the percentage of carbon in C12H22O11
42.1%
Calculate the percentage of oxygen C12H22O11
51.5%
What is the mass, in grams, of 6.33 mol of NaHCO3
532 g
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g) How many grams of NaN3 are required to produce 10.0 ft ^3 of nitrogen gas if the gas has a density of 1.25g/L
548g
How many moles of water are in 1.00 L of water, whose density is 1.00g/mL
55.55
What is the madd, in grams, of 0.50 mol of Carbon
6.0 g
What is Avogadro's number?
6.02 x 10^23
A 508g sample of sodium bicarbonate (NaHCO3) contains how many moles of sodium bicarbonate
6.05 mol NaHCO
Calculate the percentage of hydrogen in C12H22O11
6.4%
calculate the mass, in grams, of 0.433 mol of calcium nitrate
71.1 g Ca(NO3)2
calculate the formula weight of aluminum hydroxide Al(OH)3
78.0 amu
Calculate the mass, in grams, of 0.433 mol of calcium nitrate
8.29 g
What is the mass, in grams of 0.155 moles ammonium chloride
8.29 g
how many oxygen atoms are in 0.25 mol of Ca(NO3)2
9.0 x 10^23 atoms
Ethylene glycol, used in automobile antifreeze, is 38.7% C, 8.7% H, and 51.6% O by mass. Its molar mass is 62.1 g/mol. what is the molecular formula of ethane glycol
C2H6O2
A 5.325g sample of methyl benzoate, a compound used in the manufacture of perfumes, contains 3.758g of carbon, 0.316g of hydrogen, and 1.251g of oxygen. What is the empirical formula of this substance
C4H4O
Cyclohexane, a commonly used organic solvent, is 85.6%C and 14.4% H by mass with a molar mass of 84.2 g/mol. What its molecular formula?
C6H12
Ascorbic acid (vitamin C) contains 40.92% C, 4.58% H. and 54.50% O by mass. What is the empirical formula of ascorbic acid
C:H:O = (3x1:3 x 1.33 x 1) = (3: 4: 3) the empirical formula is C3H4O3
Ethylene glycol, used in automobile antifreeze, is 38.7% C, 8.7% H, and 51.6% O by mass. Its molar mass is 62.1 g/mol. What is the empirical formula of ethylene glycol.
CH3O
A 2.144g sample of phosgene, a compound used as a chemical warfare agent during World War I, contains 0.260g of carbon, 0.347g of oxygen, and 1.537g of chlorine. What is the empirical formula of this substance
COCl2
rank the following samples in order of increasing number of atoms: 9.0×1023 molecules of H2O2, 3 mol N2O3, 16 g O2.
Largest-smallest; 3molN2O3, 9.0x10^23 molecules of H2O2, 16gO2
An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g). balance this equation
answer
assuming 100.00 g of para-aminobenzoic acid and converting to moles
moles of each substance
