Question

Carbon and oxygen react to form carbon monoxide:

2C+O22CO2 \mathrm { C } + \mathrm { O } _ { 2 } \longrightarrow 2 \mathrm { CO }

. What masses of carbon and oxygen are needed to make 56.0 g CO? Which law does this illustrate?

Solutions

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Given equation :

2C + O2  2CO\begin{equation} \text{2C + O$_2$ $\rightarrow$ 2CO}\tag{1} \end{equation}

Based on above-balanced equation, we can write the below relation :

2 mole carbon : 1 mole oxygen : 2 mole CO\begin{equation} \text{2 mole carbon : 1 mole oxygen : 2 mole CO}\tag{2} \end{equation}

Molecular mass of carbon, oxygen and CO are 12, 32 and 28 respectively.

Also, we know that Mass = moles ×\times molecular weight, hence we can rewrite equation (1) as :

24 g carbon : 32 g oxygen : 56 g CO\begin{equation} \text{24 g carbon : 32 g oxygen : 56 g CO}\tag{3} \end{equation}

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