Question

How many moles of h2o are produced when 64.0 g c2h2 burns in oxygen?

Answer 1

When you burn 64.0 g of C₂H₂ in oxygen, you produce 2.46 moles of H₂O based on the stoichiometry of the balanced chemical equation for the combustion of acetylene.

Step-by-step explanation:

To determine how many moles of H₂O are produced when 64.0 g of C₂H₂ burns in oxygen, we need the balanced chemical equation for the combustion of acetylene (C₂H₂):
2 C₂H₂ (g) + 5 O₂ (g) → 4 CO₂ (g) + 2 H₂O (l)

Now, we can use the molar mass of C₂H₂ (26.04 g/mol) to convert the mass of C₂H₂ to moles:

64.0 g C₂H₂ × (1 mol C₂H₂ / 26.04 g) = 2.46 moles C₂H₂

According to the stoichiometry of the balanced equation, every 2 moles of C₂H₂ produce 2 moles of H₂O. Therefore, if you start with 2.46 moles of C₂H₂, you will produce an equal amount of moles of H₂O:

2.46 moles C₂H₂ (2 moles H₂O / 2 moles C₂H₂) = 2.46 moles H₂O.

This is the number of moles of H₂O produced when 64.0 g of C₂H₂ burn in oxygen.

Answer 2

the balanced eqaution for the combustion of C2H2 is as follows
2C₂H₂ + 5O₂ --> 4CO₂ + 2H₂O

stoichiometry of C₂H₂ to H₂O is 2:2 .
Number of moles of C₂H₂ = mass present / molar mass of C₂H₂
Since molar mass of C₂H₂ is 26 g/mol.
Number of C₂H₂ moles reacted = 64.0 g / 26 g/mol = 2.46 mol.
according to molar ratio of 2:2.
the number of H₂O moles formed = number of C₂H₂ moles reacted.
Therefore number of H₂O moles produced = 2.46 mol