Q: How many liters of water vapor will be produced when 8 liters of ethane gas (C2H10) are burned completely?

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13000, liters a day but only about 2 and half comes out

1100 liters of fuel with a specific gravity of 0.9 is equivalent to approximately 290.6 US gallons.

At STP (Standard Temperature and Pressure), 1 mole of gas occupies 22.4 liters. Therefore, 1.50 mol of C2H4 gas would occupy 1.50 x 22.4 = 33.6 liters of volume at STP.

380 However, this figure is quite approximate as gasoline expands with temperature. A gallon of gasoline weighs around 6 pounds (US) but can approach 5 pounds in extreme heat. (Buying gasoline in the summer in Phoenix or Houston gives you less energy per dollar than you are paying for.)

Related questions

Ethane is C2H6.The answer is 24,23 L water vapors (for a density of 0,804 g/cm3).

When 15 liters of propane are completely burned, it produces 110 grams of carbon dioxide.

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If 32 liters of SO2 react completely, they will produce an equal volume of SO3, because the reaction is balanced. Therefore, the total number of liters of SO3 produced will also be 32 liters.

For the complete combustion of ethane (C2H6), each molecule of ethane reacts with 3.5 molecules of oxygen (O2). At standard conditions, 22.4 liters of any gas corresponds to 1 mole. Therefore, you would need 3.5 moles of oxygen to burn 1 mole of ethane at standard conditions.

Why don't you do your own school assignment? Just take the Carbon part of ethane. We will ignore the Hydrogen that turns to water. When carbon burns, it will produce carbon dioxide. If one molecule contains two carbon atoms, that molecule will burn to produce two molecules of carbon dioxide. Now, you figure it out. To answer this question we need to know what the experimental temperature and pressures are and if ethane is to be considered an ideal gas. STP? RTP? That is not what your question asks. Your question asks, "How many liters of carbon dioxide will be produced. I would assume that it is talking about the same pressure, however I would not know. I would guess that the real issue is asking how much carbon dioxide will be dissolve in the water to form a weak acid and how much will remain free gas. Without more information, Ethane should be considered to be an ideal gas as should water above 100c. You can guess at the temperature by looking up the delta H and calculating with a formula. ---------------------------------------------------------- Lets suppose that the experiment is conducted at STP and that Ethane is an ideal gas. Ethane oxidizes via the formula C2H6 + 7/2 O2 -> 2 CO2 + 3H2O at STP (0'C) water will become a liquid and not contribute significantly to the final volume. At STP pressures are constant and all reactions are exothermic so T remains at 0'C (after everything settles down that is). And lets say that the water remains pure, without significant levels of Carbonic Acid. The question stated that there were 269 litres of Ethane so lets suppose that we are ignoring the initial oxygen gases as well, only considering the volume occupied by the ethane. Oxidized Ethane will produce double the volume of Carbon Dioxide so, at the very simplest, the final volume of Carbon Dioxide with be double the initial volume (of Ethane) so that would be 538 litres. This question gets a lot more complicated if you consider that real behavior of non-ideal gases and that it all takes place in a bomb calorminitor at constant pressure.

7 liters approximately

at STP 1 mole occupies 22.4 litres. 64.28 / 22.4 is 2.8696428 moles. Multiply this by avagadro's constant (6.022*10^23) gives 1.7281x10^24 molecules

In the reaction between HCl and NaOH, they react in a 1:1 ratio to form water and salt. Given that both solutions are 1M, 30 ml of each will contain 30 mmol of each reactant. They will completely react to form the same amount of water, which is also 30 mmol. Thus, 30 mmol of water is produced in this reaction.

Since the reaction is balanced as: 2SO2 + O2 → 2SO3 and sulfur trioxide is produced in a 1:1 ratio with sulfur dioxide, 4.0 liters of sulfur dioxide will produce 4.0 liters of sulfur trioxide.

Calculate the mass in grams of water vapor produced if 3.11 moles of propane is burned

2.0 billion gallons