Scelta multipla
If 60 grams of ethane (C_2H_6, molar mass 30 grams/mol) react completely with excess oxygen according to the equation 2 C_2H_6 + 7 O_2 → 4 CO_2 + 6 H_2O, how many moles of CO_2 are produced?
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3. Chemical Reactions
Stoichiometry
Scelta multipla
In the reaction of potassium permanganate (KMnO4) with oxalic acid (C2H2O4) to produce carbon dioxide (CO2), how many moles of KMnO4 are consumed to form 0.886 moles of CO2? (Assume the balanced equation: 2 KMnO4 + 5 C2H2O4 + 3 H2SO4 → 2 MnSO4 + K2SO4 + 10 CO2 + 8 H2O)
A
0.177 moles
B
0.443 moles
C
0.886 moles
D
0.354 moles
Guida verificata passo dopo passo1
Identify the balanced chemical equation given: 2 KMnO4 + 5 C2H2O4 + 3 H2SO4 → 2 MnSO4 + K2SO4 + 10 CO2 + 8 H2O.
From the balanced equation, note the mole ratio between KMnO4 and CO2. For every 2 moles of KMnO4 consumed, 10 moles of CO2 are produced.
Set up a proportion to find the moles of KMnO4 needed to produce 0.886 moles of CO2 using the mole ratio: \( \frac{2 \text{ moles KMnO}_4}{10 \text{ moles CO}_2} = \frac{x \text{ moles KMnO}_4}{0.886 \text{ moles CO}_2} \).
Solve the proportion for \( x \), which represents the moles of KMnO4 consumed: \( x = \frac{2}{10} \times 0.886 \).
Interpret the result to determine how many moles of KMnO4 are consumed to form 0.886 moles of CO2.
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