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WorksheetsMole concept (Calc)
Total questions: 12
Worksheet time: 1hrs 22mins
How many moles are 98.3 grams of aluminum hydroxide, Al(OH)3? (Atomic mass of Al = 27, H= 1, O = 16)
1.26 moles
0.8 moles
7,673.4 moles
150 moles
How many molecules are contained in 25 g of NaBr? (Atomic mass of Na = 23, Br = 80)
102.96 molecules
0.24 molecules
1.45x1023 molecules
2.34 x 1020molecules
What is the empirical formula for thr compound, CxHyOz , if the ratio C: H: O equal to 2: 2.5 : 1
C2H2O1
C2H5O1
C4H5O2
C3H2O2
The empirical formula for hydrocarbon A is C2H7O. If the molar mass of the hydrocarbon is 141 g/mol, determine the molecular formula for this hydrocarbon.
C2H7O
C4H14O2
C6H21O3
C8H28O4
Calculate the percentage of composition by mass of oxygen in Al(HCO3)3.
22.86 %
68.57 %
78.26 %
40.50 %
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
NaPO2
Na2PO3
Na3PO4
NaPO4
Which of the following statement are true about the formula of dinitrogen monoxide, N2O?
The relative molecular mass is 28.
One molecule of N2O consists of one nitrogen atom and one oxygen atom.
One mole of N2O contains 6.02 x 1023 atoms of nitrogen.
One mole of N2O consists of two mole of nitrogen atom and one mole of oxygen atom.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
C3H8
CH4
C2H2
C4H10
1. Ibuprofen consists of carbon, hydrogen and oxygen. When 5.000 g sample of ibuprofen is burned in oxygen, 13.86 g of CO2 and 3.926 g of water are obtained. What is the empirical formula of ibuprofen?
C12H17O2
C13H18O2
C14H19O2
The combustion of 0.202 g of an organic compound produces 0.361 g of CO2 and 0.147 g of water. Determine the molecular formula of the compound if it consists of C, H and O and has the molar mass of 148 g/mol.
C3H6O2
C6H12O2
C6H12O4
C6H12O
