Question

question 3
ethanol burns according to the following reaction:
c₂h₅oh + 3 o₂ → 2 co₂ + 3 h₂o
how many grams of co₂ (mw = 44.01) are produced when 5.5 g of c₂h₅oh (mw = 46.08) is completely burned?
report your answer to one place after the decimal point.

Explanation:

Step1: Calculate moles of \(C_2H_5OH\)

Use the formula \(n=\frac{m}{MW}\), where \(m = 5.5\space g\) and \(MW = 46.08\space g/mol\).
\(n_{C_2H_5OH}=\frac{5.5}{46.08}\space mol\approx0.1194\space mol\)

Step2: Use mole - ratio from balanced equation

From \(C_2H_5OH + 3O_2
ightarrow2CO_2 + 3H_2O\), the mole - ratio of \(C_2H_5OH\) to \(CO_2\) is \(1:2\). So \(n_{CO_2}=2\times n_{C_2H_5OH}\)
\(n_{CO_2}=2\times0.1194\space mol = 0.2388\space mol\)

Step3: Calculate mass of \(CO_2\)

Use \(m = n\times MW\), with \(n = 0.2388\space mol\) and \(MW = 44.01\space g/mol\)
\(m_{CO_2}=0.2388\times44.01\space g\approx10.5\space g\)

Answer:

\(10.5\)