Lesson 5.1.2
5.1.2 Empirical and molecular formulae Quiz: Pearson Edexcel Chemistry, Unit 5
20 questions
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Lesson 5.1.2, Empirical and molecular formulae: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 5: Formulae, Equations and Amounts of Substance, written with Revision Ninja.
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The 20 questions
-
Which formula shows the simplest whole-number ratio of atoms in a compound?
- Molecular formula
- Empirical formula
- Structural formula
- Displayed formula
-
Which formula shows the actual number of atoms of each element in a molecule?
- Molecular formula
- Structural formula
- General formula
- Empirical formula
-
What is the empirical formula of glucose, C6H12O6?
- C3H6O3
- C6H12O6
- C2H4O2
- CH2O
-
What is the empirical formula of ethene, C2H4?
- CH2
- C2H4
- CH4
- C3H6
-
A compound with empirical formula CH2O has molar mass 180 g mol-1. What is its molecular formula?
- C3H6O3
- C5H10O5
- C2H4O2
- C6H12O6
-
A compound contains 40.0% C, 6.7% H and 53.3% O by mass. What is its empirical formula? (C = 12, H = 1, O = 16)
- CH2O
- CH4O
- C2H4O2
- CHO
-
A hydrocarbon is 85.7% C and 14.3% H by mass. What is its empirical formula? (C = 12, H = 1)
- CH2
- C2H
- CH
- CH3
-
A compound is 82.8% C and 17.2% H by mass. What is its empirical formula? (C = 12, H = 1)
- C2H5
- CH2
- CH4
- C3H8
-
A hydrocarbon has empirical formula CH2 and molar mass 56 g mol-1. What is its molecular formula?
- C4H8
- C5H10
- C3H6
- C2H4
-
1.20 g of magnesium burns completely to give 2.00 g of an oxide. What is the empirical formula? (Mg = 24, O = 16)
- MgO2
- MgO
- Mg3O2
- Mg2O
-
A compound contains 2.4 g C, 0.4 g H and 3.2 g O. What is its empirical formula? (C = 12, H = 1, O = 16)
- C2H4O
- CH4O
- CHO2
- CH2O
-
Which equation relates pressure, volume, amount and temperature for a gas?
- pn = VRT
- p/V = nRT
- pV = nRT
- pV = R/nT
-
How many moles of gas occupy 0.0245 m^3 at 298 K and 101325 Pa? (R = 8.31)
- 0.100 mol
- 1.00 mol
- 10.0 mol
- 0.0245 mol
-
What is 250 cm^3 expressed in m^3?
- 2.5 x 10^-6 m^3
- 0.25 m^3
- 2.5 x 10^-4 m^3
- 2.5 x 10^-3 m^3
-
0.60 g of a gas occupies 245 cm^3 at 101325 Pa and 298 K. What is its molar mass? (R = 8.31)
- 120 g mol-1
- 6 g mol-1
- 30 g mol-1
- 60 g mol-1
-
What temperature unit must be used in the ideal gas equation pV = nRT?
- Joules
- Degrees Celsius
- Degrees Fahrenheit
- Kelvin
-
A compound has empirical formula CH2O and molar mass 90 g mol-1. What is its molecular formula? (Empirical mass 30)
- C6H12O6
- CH2O
- C3H6O3
- C2H4O2
-
Which property must be known alongside combustion data to find a molecular formula?
- Avogadro constant
- Boiling point
- Molar mass
- Density
-
What is the percentage by mass of carbon in ethene, C2H4? (C = 12, H = 1)
- 66.7%
- 50.0%
- 14.3%
- 85.7%
-
What is the first step when calculating an empirical formula from mass percentages?
- Add percentages together
- Divide by Mr
- Divide by Ar
- Multiply by Ar
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