Question

question 11 (1 point) if 24 g of c is consumed in 2 c + o2 → 2 co, the mass of carbon monoxide produced is
112 g
28 g
32 g
56 g
question 12 (1 point)

Explanation:

Step1: Determine molar - mass of C and CO

The molar - mass of C is $M_{C}=12\ g/mol$, and the molar - mass of CO is $M_{CO}=12 + 16=28\ g/mol$.

Step2: Calculate moles of C consumed

The number of moles of C, $n_{C}=\frac{m_{C}}{M_{C}}$, where $m_{C} = 24\ g$. So $n_{C}=\frac{24\ g}{12\ g/mol}=2\ mol$.

Step3: Use stoichiometry

From the balanced chemical equation $2C+O_{2}
ightarrow2CO$, the mole ratio of C to CO is 1:1. So the number of moles of CO produced, $n_{CO}=n_{C}=2\ mol$.

Step4: Calculate mass of CO produced

The mass of CO, $m_{CO}=n_{CO}\times M_{CO}$. Substituting $n_{CO}=2\ mol$ and $M_{CO}=28\ g/mol$, we get $m_{CO}=2\ mol\times28\ g/mol = 56\ g$.

Answer:

56 g