Question

How many moles of H2O are produced from 6.23g of C2H6 in the following reaction? 2C2H6+7O2 -> 4CO2+6H2O

Answer 1

C2H6 (g) + O2 (g). --> CO2(g)+H2O (g)

2C2H6 (g) + 7O2 (g). --> 4CO2(g)+6H2O (g)

(8.45 x 10^23)/(6.022x10^23) = 1.403 moles H2O

1.403 moles H2O x (4molCO2/6molH2O)= .935 moles CO2

.935 moles CO2 x (6.022 x10^23)= 5.63 x 10^23 molecules CO2

Answer 2

Answer:

0.623 moles of H₂O.

Explanation:

• balanced equation: 2C₂H₆ + 7O₂ -> 4CO₂+ 6H₂O

Given:

• 6.23g of C₂H₆

• C₂H₆ molar mass is 30

solve for moles of C₂H₆

• moles = mass/mr

• moles = 6.23/30

• moles = 0.2077

solve for moles of H₂O using molar ratio

• 2C₂H₆ : 6H₂O

• 2 : 6

• 0.2077 : 0.623

Therefore, found that 0.623 moles of H₂O is produced.