Determine the molecular formula of a compound with an empirical formula CH₂ and a molar mass of 84 g.
C₆H₁₂
What mass of sodium chloride (NaCl) is formed when 4.6 g of sodium reacts with chlorine gas? (Na = 23, Cl = 35.5)
11.5 g
How many liters of hydrogen gas (H₂) are produced when 4 moles of Al react with excess HCl? (Al + 3HCl → AlCl₃ + 3/2 H₂, Molar volume = 24 dm³)
72 dm³
A compound has 54.5% carbon, 9.1% hydrogen, and 36.4% oxygen. Determine its empirical formula. (C = 12, H = 1, O = 16)
C₂H₄O
How many grams of O₂ are required to completely react with 4 moles of CH₄ in the reaction CH₄ + 2O₂ → CO₂ + 2H₂O? (O = 16)
128 g (4 × 2 × 32)
A sample of hydrated copper(II) sulfate, CuSO₄·xH₂O, has a molar mass of 250 g/mol. Find the value of x if CuSO₄ = 160 g/mol.
x = 5 (CuSO₄·5H₂O)
In a reaction, 60 g of carbon reacts with 160 g of oxygen to produce carbon dioxide. Identify the limiting reactant and calculate the mass of CO₂ formed. (C = 12, O = 16, C + O₂ → CO₂)
Carbon is the limiting reactant; CO₂ produced = 220 g
Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. How many grams of Fe are formed when 160 g of Fe₂O₃ reacts? (Fe = 56, O = 16, Fe₂O₃ + 3CO → 2Fe + 3CO₂)
112 g
How many grams of aluminum oxide (Al₂O₃) are produced when 54 g of aluminum reacts with oxygen? (Al = 27, O = 16, 4Al + 3O₂ → 2Al₂O₃)
102 g
Calculate the number of molecules in 88 g of CO₂. (Mr of CO₂ = 44, Avogadro’s constant = 6.02 × 10²³)
1.204 × 10²⁴ molecules
A compound contains 27.3% carbon, 72.7% oxygen. Find its empirical formula. (C = 12, O = 16)
CO₂
Ammonia (NH₃) reacts with oxygen to produce nitrogen monoxide (NO) and water. Balance the equation and determine how many moles of NO are produced from 10 moles of NH₃. Equation: 4NH₃ + 5O₂ → 4NO + 6H₂O
10 moles of NH₃ produce 10 moles of NO
A reaction has a theoretical yield of 50 g, but only 35 g of product was obtained. What is the percentage yield?
70%
A hydrocarbon contains 85.7% carbon and 14.3% hydrogen. Determine its empirical formula. (C = 12, H = 1)
CH₂
Calculate the percentage composition of carbon in C₆H₁₂O₆. (C = 12, H = 1, O = 16)
40%
How many moles of H₂SO₄ are present in 196 g of sulfuric acid? (H = 1, S = 32, O = 16)
2 moles
How many moles of water are produced from 5 moles of oxygen in the reaction 2H₂ + O₂ → 2H₂O?
10 moles
How many liters of NH₃ gas are produced from 5 moles of N₂ in the reaction N₂ + 3H₂ → 2NH₃? (Molar volume = 24 dm³)
240 dm³
What volume of CO₂ gas is produced at RTP when 10 g of calcium carbonate decomposes? (CaCO₃ → CaO + CO₂, Molar volume = 24 dm³, CaCO₃ = 100 g/mol)
2.4 dm³
What mass of magnesium oxide is formed when 5 g of magnesium burns in oxygen? (Mg = 24, O = 16, 2Mg + O₂ → 2MgO)
8.33 g
Your experience on this site will be improved by allowing cookies.