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Using Moles To Balance Equations (ht Only) (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Using Moles To Balance Equations (ht Only)' from the broader topic Quantitative Chemistry. The test is geared towards the AQA exam board style syllabus.
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For N2 + 3H2 ? 2NH3, if 10.0 dm3 H2 reacts with excess N2 at RTP, what volume NH3 (dm3) is formed?
In combustion 2Fe2O3 + 3C ? 4Fe + 3CO2. If 40.0 kg Fe2O3 is reduced completely with excess C, what volume of CO2 (dm3) is produced at RTP (1 mol gas = 24.0 dm3, Mr Fe2O3 = 160)?
2Al + 3Cl2 ? 2AlCl3. What is the atom economy for producing AlCl3 (mass of desired product ÷ mass of reactants ×100)? (Use Ar Al 27.0, Cl 35.5)
What is the limiting reagent and how many moles of CO2 are made when 1.50 mol NH3 reacts with 0.60 mol O2 in the reaction 4NH3 + 5O2 ? 4NO + 6H2O?
A sample of product shows actual mass 24.6 g when theoretical mass was 30.0 g. What is percentage yield?
2Mg + SiO2 ? 2MgO + Si. What minimum mass of Mg (g) is needed to completely reduce 1.20 kg SiO2? (Ar: Mg 24, Si 28, O 16)
2H2 + O2 ? 2H2O. If you start with 3.00 mol H2 and 1.00 mol O2, which statement is correct about the limiting reagent and moles of H2O formed?
CaCO3 ? CaO + CO2. If 48.0 dm3 CO2 (RTP, 1 mol gas = 24.0 dm3) is collected, what mass of CaCO3 was decomposed? (Mr CaCO3 = 100.0)
At RTP 33.6 dm3 of N2 gas is collected. What is its mass? (Molar volume = 24.0 dm3, Mr N2 = 28.0)
Mg + 2HCl ? MgCl2 + H2. If 0.0200 mol Mg reacts fully, what volume (dm3) of H2 is formed at RTP (1 mol gas = 24.0 dm3)?
2Na + Cl2 ? 2NaCl. If 46.0 g sodium reacts with excess chlorine, what mass of NaCl is formed? (Ar: Na 23.0, Cl 35.5)