Acetylene C2H2 gas is often used in welding torches because of the very high heat produced when it reacts with oxygen O2 gas, producing carbon dioxide gas and water vapor. Calculate the moles of water produced by the reaction of 0.095mol of oxygen. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Question
Acetylene C2H2 gas is often used in welding torches because of the very high heat produced when it reacts with oxygen O2 gas, producing carbon dioxide gas and water vapor. Calculate the moles of water produced by the reaction of 0.095mol of oxygen. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Solution
The balanced chemical equation for the reaction is:
2C2H2 + 5O2 -> 4CO2 + 2H2O
From the balanced equation, we can see that 5 moles of oxygen (O2) react with 2 moles of acetylene (C2H2) to produce 2 moles of water (H2O). Therefore, the ratio of O2 to H2O is 5:2.
Given that 0.095 moles of oxygen are used, we can calculate the moles of water produced as follows:
(0.095 moles O2) * (2 moles H2O / 5 moles O2) = 0.038 moles H2O
So, 0.038 moles of water are produced. Rounding to 2 significant digits, we get 0.038 moles of water.
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