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3. Based on the following balanced equation:
2 C H20 + 13 02 8 CO2 + 10 H2O
a. How many moles of O2 are required to react completely with 4.00 moles of C4H10?
3.00 6.00 8.00 10.00 13.00 16.00 20,00 23,00 26.00
b. How many moles of CO2 are produced after complete reaction of 4.00 moles of C H10?
3.00 6.00 8.00 10.00 13,00 16.00 20.00 23.00 26.00
c. How many moles of H2O are produced after complete reaction of 4.00 moles of C&H10?
3.00 6.00 8.00 10.00 13.00 1.6.00 20.00 23,00 26.00

Respuesta :

Answer:

A. 26 moles O2

B. 16 moles CO2

C. 20 moles H20

Explanation:

a. 4 moles C4H10 x [tex]\frac{13 moles O2}{2 moles C4H10}[/tex] = 26 moles O2

B. 4 moles C4H10 x [tex]\frac{8 moles CO2}{2 moles C4H10}[/tex] = 16 moles CO2

C. 4 moles C4H10 x [tex]\frac{10 moles H2O}{2 moles C4H10}[/tex] = 20 moles H20

Use the coefficients of the balanced equation to make the convertions

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