168.96 g of carbon dioxide (CO₂)
Explanation:
The chemical reaction representing the combustion of acetylene:
2 C₂H₂ (g) + 5 O₂ (g)→ 4 CO₂ (g) + 2 H₂O (g)
number of moles = mass / molecular weight
number of moles of acetylene (C₂H₂) = 50 / 26 = 1.92 moles
Taking in account the stoichiometry of the chemical reaction, we devise the following reasoning:
if 2 moles of acetylene (C₂H₂) produces 4 moles of carbon dioxide (CO₂)
then 1.92 moles of acetylene (C₂H₂) produces X moles of carbon dioxide (CO₂)
X = (1.92 × 4) / 2 = 3.84 moles of carbon dioxide (CO₂)
mass = number of moles × molecular weight
mass of carbon dioxide (CO₂) = 3.84 × 44 = 168.96 g
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combustion of hydrocarbons
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When the temperature increases,the particles will conduct successful collisions and the rate of reaction will also increase
Answer:
C3H6
Explanation:
We can obtain the molecular formula by using the empirical formula and the molar mass in combination.
This is shown below:
[CH2]n = 42g/mol
We then add the atomic masses of carbon and hydrogen and multiply by n to give the value of n .
n[12 + 2(1)] = 42
14n = 42
n = 42/14 = 3
The molecular formula is thus [CH2]3 = C3H6
It should be 1.13 x 10^25 atoms