Question

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced?

Answer 1

Answer:

The mass of iodine produced will be 79.46 kg .

Explanation:

Let us calculate the mole ratio of potassium and iodine formed when first sample was decomposed.

Atomic mass of potassium =39 g/mol

Atomic mass of iodine = 127 g/mol

Moles of K produced = $\frac{mass}{atomicmass}=\frac{13}{39}= 0.33$

Moles of I produced =  $\frac{mass}{atomicmass}=\frac{42.3}{127}= 0.33$

The mole ration of K :I = 1:1

The moles of K produced by second sample = $\frac{mass}{molarmass}=\frac{24.4X10^{3}}{39}= 0.626X10^{3} mol$

The same moles of I must have been produced.

The mass of Iodine produced = moles X atomic mass = 0.626  X 127=79.46 kg