Answer:
Option C, (Actual yield ÷ percent yield) × 100
Explanation:
Theoretical yield is defined as the total amount of product formed for given reactants in a chemical reaction. It is an ideal case which assumes no exceptions or wastage.
The mathematical relation between the actual yield, percent yield and theoretical yield is as follows -
Where
P.Y. represents the percent yield a
M A.Y. represents the mass obtained from actual yield
M T.Y. represents the mass obtained from theoretical yield
Hence, if we rearrange the formula, we get -
Hence, option C is correct
The mass of CO2 produced by 26g of acetylene is 88g.
Given ,
In an oxyacetylene torch, acetylene gas (ethyne; HCCH) burns to produce carbon dioxide and water vapour.
The acetylene combustion reaction is given by,
H2O + HCCH + 5/2 O=O 2CO2
Heat of reaction for acetylene combustion = 1259kj/mol
CO2 has a molecular mass of 44g/mol.
2 moles of CO2 have a molecular mass of 88g.
On combustion, 1 mole of acetylene yields 2 moles of CO2.
Thus, 26g of acetylene produces 88g of CO2 when burned.
As a result, the mass of carbon dioxide produced by 26g of acetylene is 88g.
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it depends how heavy and how far it travels
