How many moles of CO₂ are consumed when 22.0g of NH₃ react completely in the following equation? CO₂ + 2NH₃ $\rarr$CO(NH₂)₂ + H₂O

Question

Quizplus · Accepted Answer

First, we need to correct the chemical formulas from the given equation. The correct equation seems to be: $$ CO + 2NH_3 \rightarrow CO(NH_2)_2 + H_2O $$. To find the moles of $ CO $ consumed, we start with the molar mass of $ NH_3 $ (17.03 g/mol). Given 22.0 g of $ NH_3 $, we have $ \frac{22.0 \, \text{g}}{17.03 \, \text{g/mol}} = 1.291 \, \text{mol} $ of $ NH_3 $. Since the reaction consumes 2 moles of $ NH_3 $ for every mole of $ CO $, the moles of $ CO $ consumed are $ \frac{1.291 \, \text{mol}}{2} = 0.646 \, \text{mol} $.

How Many Moles of CO2 Are Consumed When 22 →\rarr→ CO(NH2)2 + H2O A)0

How Many Moles of CO₂ Are Consumed When 22 $\rarr$ CO(NH₂)₂ + H₂O
A)0