4A+B2→2A2B
The molar mass of A is 12g/mol. The molar mass of B is 4g/mol. The molar mass of A2B
is 28g/mol. When the goal of the reaction is to produce 112g of the product, how many grams of reactant A should be present initially?
(1 point)
Responses
16
16
96
96
24
24
48
To determine the grams of reactant A needed to produce 112g of the product A2B, we need to first calculate the molar ratio of A to A2B in the reaction.
From the balanced chemical equation, we see that 4 moles of A are required to produce 2 moles of A2B. This means the molar ratio of A to A2B is 4:2 or 2:1.
Given that the molar mass of A is 12g/mol, we can use the molar ratio to calculate the grams of A needed to produce 112g of A2B:
12g A (1 mol A / 12g A) (2 mol A / 2 mol A2B) = 12g A
Therefore, we need 12 grams of reactant A initially to produce 112g of the product A2B.
Therefore, the correct answer is not provided in the options.