6 (a) Methane is a hydrocarbon fuel - Edexcel - GCSE Chemistry - Question 6 - 2020 - Paper 1
Question 6
6 (a) Methane is a hydrocarbon fuel.
(i) Complete the word equation for the complete combustion of methane in oxygen.
methane + oxygen → water
(ii) The incomplete... show full transcript
Worked Solution & Example Answer:6 (a) Methane is a hydrocarbon fuel - Edexcel - GCSE Chemistry - Question 6 - 2020 - Paper 1
Step 1
Complete the word equation for the complete combustion of methane in oxygen.
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Answer
The complete word equation for the combustion of methane in oxygen is:
methane + oxygen → water + carbon dioxide.
Step 2
Give the reason why carbon and carbon monoxide are produced in the incomplete combustion of methane.
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Answer
Carbon and carbon monoxide are produced during incomplete combustion due to insufficient oxygen supply, leading to the formation of solid carbon (soot) and the poisonous gas carbon monoxide instead of fully oxidizing to carbon dioxide.
Step 3
Name the fraction in Figure 10 that is used to surface roads.
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Answer
The fraction used to surface roads is bitumen.
Step 4
Name the fraction in Figure 10 that contains hydrocarbons with the lowest boiling point.
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Answer
The fraction that contains hydrocarbons with the lowest boiling point is gases.
Step 5
Which of the following shows the fractions where the relative demand is greater than the relative amount in the crude oil?
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Answer
The correct answer is A: kerosene, diesel oil, bitumen.
Step 6
Determine the value of x in the molecule of CxHy.
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Answer
To maintain the balance of carbon and hydrogen, when C8H18 is cracked to form one molecule of C7H16, the equation is:
C8H18 → C7H16 + CxHy.
From this equation, we find that x = 2, so the molecule is C2H4.
Step 7
Calculate the maximum mass of octane that could be produced when 340g of dodecane is cracked.
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Answer
The molar mass of dodecane is 170 g/mol. The ratio of dodecane to octane is 1:1. Therefore, 340 g of dodecane (which is 2 moles) can produce 2 moles of octane. The mass of octane produced is:
mass = moles × molar mass = 2 mol × 114 g/mol = 228 g.
Thus, the maximum mass of octane that could be produced is 228 grams.
