Question

For a reaction, $\mathrm{A}+2\mathrm{B}⟶\mathrm{C}$, the amount of C formed by starting the reaction with 5 moles of A and 8 moles of B is:

• A. 4 mol
• B. 5 mol
• C. 8 mol
• D. 16 mol

Answer 1

The correct option is A

4 mol

An explanation for the correct option:

Option (A): 4 mol

• The reaction is given as; $\mathrm{A}+2\mathrm{B}⟶\mathrm{C}$
• so, from the reaction, 1 mole of A reacts with 2 moles of B to form 1 mole of C.
• Hence, 8 moles of B will react with 2*4 mole of A to form = 4 mole of C.
• Here, B is the limiting reagent here, as 1 mole of A will remain unreacted after consumption of 8 moles of B.

An explanation for the incorrect option:

Option (B): 5 mol

• We have already calculated the moles of product C as 4moles.
• Hence, option B; 5mol cant be the right option.

Option (C): 8 mol

• The calculated product C is found to be 4 moles.
• So, option C; 8mol cant be the right option.

Option (D): 16 mol

• The option is given as 16 moles, which doesn't coincide with the calculated product which is 4 moles.
• So, option D; 16moles cant be the right option.

Hence, For the reaction, $\mathrm{A}+2\mathrm{B}⟶\mathrm{C}$the amount of C formed by starting the reaction with 5 moles of A and 8 moles of B is 4 moles which is Option (A)