Question

In the reaction: C6H12O6(s) +602(g) → 6CO2(g) + 6H2O(1) If 1.0 g CH12O6 reacts with excess O₂, what mass (by grams) of H₂O is formed?
A 0.3 g
B 1.2 g
0.6 g
D 9.9 g
E none of these

Answer 1

The balanced reaction shows that 1 mole of C6H126 produces 6 moles of H2O.
First, calculate the molar mass of C6H12O6:
(612.01)+(121.01)+(6*16.00) = 180.18 g/mol
Next, calculate the number of moles in 1.0g of C6H12O6:
1.0g / 180.18 g/mol = 0.00555 mol
Since the molar ratio is 1:6 for C6H12O6 to H2O, multiply the moles of C6H12O6 by 6 to find the moles of H2O produced:
0.00555 mol * grams:
.0333 mol * 18. 0.62O is formed in the reaction.
The correct answer is C) 0.6 g.