Table of Contents
How many molecules of water will be produced if 5 moles of propane C3H8 react with oxygen?
C3H8(g) + O2(g) ——> CO2(g) + H2O(g) . Every one mole of C3H8 propane will react with 5 moles of O2 to yield or produce 3 moles of Carbon dioxide CO2 and 4 moles of H2O water.
How many moles of water are produced from the complete combustion of two moles of propane?
Clearly, four moles of water result from each mole of propane. And if 1.638⋅g of propane are combusted this represents a molar quantity of…
How many moles of propane were burned?
The molar mass of propane is 44 g/mole, so burning propane will release (2030kJ/mole) / (44g/mole) = about 46 kJ/g of fuel burned….ANSWERS TO HOMEWORK #1 – THE WHOLE THING.
| CH4 | C3H8 | |
|---|---|---|
| kJ released per gram of fuel used | 51 | 46 |
How many moles of water can you make from 5 moles h₂?
From this you can see that 5 moles of hydrogen gas would react with 2.5 of the available 3 moles of oxygen gas, to form 5 moles of water. The molar mass of water is 18 g/mol, so you would end up with 5 x 18 = 90 g of water.
How many moles of of co2 are produced when 10 moles of propane are burned?
There will be 30 moles of carbon dioxide that will be released into the air.
How many moles of CS2 are formed when 2.7 moles C reacts?
Answer and Explanation: Therefore 0.54 mol of CS2 C S 2 is formed.
How many moles of of CO2 are produced when 10 moles of propane are burned?
How many grams of water are produced when propane ( C3H8 )?
How many grams of water are produced when propane (C3H8) burns with 12.0 L of oxygen at STP? The NIE for the complete combustion of propane is:
How many liters are in a mole of gas?
To find out how much that is, we need to convert liters of O2 to moles of O2 using the fact that at STP, a mole of gas is equivalent to 22.4 liters. The molar ratio of O2 to H2O is 5 4 and the molecular weight of H2O is 18.0g, so:
How many liters of O2 are produced when propane is burned?
The problem doesn’t state how much propane is burned, so we’re going to assume that there is enough to use up all the oxygen. To find out how much that is, we need to convert liters of O2 to moles of O2 using the fact that at STP, a mole of gas is equivalent to 22.4 liters.
How to calculate the amount of water produced by the combustion?
Yes the complete combustion equation is correct as you stated and the equation of the incomplete combustion is certainly one possibility. A more general formula is: CX5HX12 + (x 2 + y + 3)OX2 ⟶ (5 − x − y)C + xCO + yCOX2 + 6HX2O {x, y ∈ R + 0; (x + y) ≤ 5} This is assuming all the hydrogen will be converted into water.