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If one mole of c2h2 is used in the chemical reaction represented by the equation Incorrect (2.5 moles of o2 are needed). 2c2h2 + 5o2 → 4co2 + 2h2o we can determine the correct statement by examining the coefficients in the balanced equation
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From the equation, we can see that for every 2 moles of c2h2, 5 moles of o2 are required. One mole of oxygen was used in this reaction The number of atoms of each element on both sides of (2c2h2) + (5o2) = (4co2) + (2h2o) is equal which means that the equation is already balanced and no additional work is needed.
The given reaction is an example of a combustion reaction
In a combustion reaction, a substance (usually a hydrocarbon) reacts with oxygen to produce carbon dioxide (co2) and water (h2o). In the given reaction, acetylene (c2h2) is reacting with oxygen (o2) to produce water (h2o) and carbon dioxide (co2) This is a classic example of a combustion reaction. The balanced equation for the complete oxidation of acetylene (c2h2) burning in air is
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Thus, the correct answer is c
The given chemical equation is 2c 2h 2 + 5o2 → 4c o2 + 2h 2o This reaction is classified as a combustion reaction Let's break this down further:
Since there is an equal number of each element in the reactants and products of 2c2h2 + 5o2 = 4co2 + 2h2o, the equation is balanced. From the equation, 2 moles of c2h2 produce 4 moles of co2 This calculation confirms that 2 moles of co2 are produced from 1 mole of c2h2, aligning with the stoichiometric relationships in the equation 2
