Question

PLEASE ANSWER QUICKLY!!!!! 50 POINTS

2KI(aq) + Cl₂(g) → 2KCI(aq) + 1₂ (g)
44.8 L I2 forms at STP. How many moles of KI were required for the
reaction?
?] mol KI

Answer 1

Step-by-step explanation:

We use the balanced chemical equation to determine the mole ratio between KI and I2.

From the balanced equation,

2 moles of KI produce 1 mole of I2

So, 1 mole of I2 is produced from 2 moles of KI.

To find the moles of KI required, we can use the following formula:

moles of KI = moles of I2 / 2

At STP, 1 mole of any gas occupies 22.4 L volume.

So, the number of moles of I2 can be calculated as:

n = V / Vm = 44.8 L / 22.4 L/mol = 2.00 mol

Substituting the value of n in the above formula, we get:

moles of KI = 2.00 mol / 2 = 1.00 mol of KI

Therefore, 1.00 mol of KI was required for the reaction.