Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
What volume of steam is produced when 10g of propyne is burn in excess oxygen at S.T.P
Accepted Answer
When 10 g of propyne is burned in excess oxygen at STP, the volume of steam produced can be calculated using the following steps:
1. Balanced Chemical Equation:
Combustion of propyne with oxygen produces carbon dioxide and water vapor according to the following balanced chemical equation:
C3H4(g) + 4O2(g) → 3CO2(g) + 2H2O(g)
2. Moles of Propyne:
Convert the mass of propyne to moles using its molar mass (42.08 g/mol):
moles of C3H4 = 10 g / 42.08 g/mol = 0.2377 mol
3. Moles of Steam Produced:
From the balanced chemical equation, 1 mole of propyne produces 2 moles of steam:
moles of H2O = 2 * moles of C3H4 = 2 * 0.2377 mol = 0.4754 mol
4. Volume of Steam at STP:
At STP (Standard Temperature and Pressure, 0 °C and 1 atm), 1 mole of any ideal gas occupies 22.4 L:
Volume of H2O = 0.4754 mol * 22.4 L/mol = 10.62 L
Therefore, when 10 g of propyne is burned in excess oxygen at STP, 10.62 L of steam is produced.
Articles you might like