Considering the limiting reactant concept,how many moles of C are produced from the reaction of 1.00 mol A and 1.00 mol B? A(g)+ 2 B(g)→ 3 C(g)

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To determine the limiting reactant, we need to compare the amount of product that can be produced from each reactant. From the balanced chemical equation, we can see that for every 1 mole of A reacting, we can produce 3 moles of C, and for every 2 moles of B reacting, we can produce 3 moles of C. 
- If we start with 1.00 mol of A and 1.00 mol of B, we can see that we have enough B to react with all of the A (since for every 2 moles of B, we only need 1 mole of A). So, B is not the limiting reactant.
- To determine how much C is produced, we can use the ratio from the balanced equation: 1 mole of A produces 3 moles of C. Therefore, our maximum amount of C produced is 3.00 mol.
- However, since A is the limiting reactant (we only have 1.00 mol of A), we need to use that number to calculate how much C is actually produced. Using the same ratio, 1 mole of A produces 3 moles of C. Therefore, only 1.00 mol of C can be produced from the given amount of A.
- Therefore, the amount of C produced is limited by the amount of A, and the answer is B) 1.50 mol, which is half of the maximum amount of C that could be produced.

Considering the Limiting Reactant Concept,how Many Moles of C Are