Question

How many moles of O₂ will be formed from the decomposition of Pb(NO₃)₂?

• A. 1 mole
• B. 2 moles
• C. 0.5 mole
• D. 4 moles

Hint:

Always write and balance the full chemical equation. Then use the stoichiometric ratio directly from the coefficients to determine the number of moles of any product.

Answer 1

The Correct Option is A

Step 1: Write the balanced chemical equation for the decomposition of lead nitrate
\[ 2\, \text{Pb(NO}_3)_2 \rightarrow 2\, \text{PbO} + 4\, \text{NO}_2 + \text{O}_2 \] Step 2: Observe the mole ratio
From the equation: \[ 2 \text{ moles of Pb(NO}_3)_2 \text{ produce } 1 \text{ mole of O}_2 \] Step 3: Calculate the oxygen formed from 2 moles of Pb(NO\(_3\))\(_2\)
The question implicitly refers to the decomposition of 2 moles of Pb(NO\(_3\))\(_2\) (since the options suggest direct output), hence: \[ \text{O}_2 \text{ produced} = 1 \text{ mole} \] \[ \boxed{\text{1 mole of O}_2 \text{ is formed from the decomposition of 2 moles of Pb(NO}_3)_2} \]