Questions and Answers
What is the balanced chemical equation for the combustion of ethene?
How much water is produced from the combustion of 11g of ethene?
What mass of ethene (C2H4) is needed to produce 36g of water?
How many grams of oxygen (O2) are consumed when 11g of ethene is burned?
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Which of the following represents the correct relationship of molar masses in the combustion of ethene?
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Study Notes
Balancing Chemical Equations
- Ethene (C2H4) combustion reaction: C2H4 + 3O2 → 2CO2 + 2H2O
- Balanced equation ensures equal number of atoms for each element on both sides.
Calculation of Water Production from Ethene
- The molar mass of ethene (C2H4) is 28g.
- Oxygen (O2) has a molar mass of 32g; therefore, 3O2 has a mass of 96g.
- Carbon dioxide (CO2) has a molar mass of 44g, and water (H2O) has a molar mass of 18g.
- Total mass in the balanced equation: 28g (C2H4) + 96g (O2) → 88g (CO2) + 36g (H2O).
Water Production Calculation from Ethene
- To find the mass of water produced from 11g of C2H4, use the ratio from the balanced equation:
- Calculation: [36g (H2O) / 28g (C2H4)] × 11g (C2H4) = 29.79g of H2O.
- Therefore, the combustion of 11g of ethene yields approximately 29.79g of water.
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Description
This quiz focuses on balancing chemical equations and calculating the amount of water produced from the combustion of ethene. Participants will use the given equation and stoichiometry to find the mass of water resulting from a specified mass of ethene. Test your knowledge in basic chemistry calculations and concepts.
