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How many grams of carbon dioxide are produced by the combustion of 224 liters of ethane gas CH in standard conditions?
88
What is the mass of 455 ml of ethane gas c2h6 at stp?
To find the mass of 455 mL of ethane (C₂H₆) gas at standard temperature and pressure (STP), we first note that 1 mole of any ideal gas occupies 22.4 liters (or 22,400 mL) at STP. Thus, 455 mL of ethane corresponds to approximately ( \frac{455}{22400} ) moles, which is about 0.0203 moles. The molar mass of ethane is about 30.07 g/mol, so the mass of 455 mL of ethane at STP is approximately ( 0.0203 , \text{moles} \times 30.07 , \text{g/mol} \approx 0.61 , \text{grams} ).
How much urine is produced by an average human?
13000, liters a day but only about 2 and half comes out
What is 1100 liters of fuel with specific gravity 0.9 is equivalent to in us gallons?
1,100 litres is equivalent to 290.589 US gallons (rounded), regardless of what's in the liters. Even if they're completely empty.
What volume will 1.50 mol of C2H4 gas occupy at STP?
1 mole gas = 22.4L 1.5mol C2H4 x 22.4L/mol = 33.6L ethane gas (C2H4)
How many liters of water vapor will be produced when 8 liters of ethane gas are burned completely?
Ethane is C2H6.The answer is 24,23 L water vapors (for a density of 0,804 g/cm3).
If 15 liters of propane are completely consumed how many grams of carbon dioxide are produced?
If 15 liters of propane are completely consumed 90,25 grams of carbon dioxide are produced.
How many grams of carbon dioxide are produced by the combustion of 224 liters of ethane gas CH in standard conditions?
88
What is the total number of liters of SO3 produced when 32 liters of SO2 reacts completely?
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.
How many moles of oxygen are required to burn 22.4 liters of ethane gas C2H6 at standard conditions?
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.
When ethane C2H6 burns it produces carbon dioxide and water How many liters of carbon dioxide will be produced when 269 L of ethane are burned?
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.
How many molecules of ethane are present in 64.28 liters of ethane gas (C2H6) at STP?
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
How many liters of peritoneal fluid are produced and reabsorbed each day?
7 liters approximately
What is the mass of 455 ml of ethane gas c2h6 at stp?
To find the mass of 455 mL of ethane (C₂H₆) gas at standard temperature and pressure (STP), we first note that 1 mole of any ideal gas occupies 22.4 liters (or 22,400 mL) at STP. Thus, 455 mL of ethane corresponds to approximately ( \frac{455}{22400} ) moles, which is about 0.0203 moles. The molar mass of ethane is about 30.07 g/mol, so the mass of 455 mL of ethane at STP is approximately ( 0.0203 , \text{moles} \times 30.07 , \text{g/mol} \approx 0.61 , \text{grams} ).
Can you provide some gas stoichiometry practice problems for me to work on?
Here are some gas stoichiometry practice problems for you to work on: How many liters of oxygen gas are needed to completely react with 5.0 liters of hydrogen gas to produce water vapor? If 2.0 moles of methane gas react with excess oxygen gas, how many moles of carbon dioxide gas will be produced? A reaction produces 4.0 liters of nitrogen gas. If the reaction is 80 efficient, how many liters of nitrogen gas would be produced if the reaction was 100 efficient? These problems will help you practice applying gas stoichiometry concepts.
What is the number of moles of water produced in a reaction of 30.00ml of 1M hcl and 30ml of 1M naoh?
All one to one here. NaOH + HCl --> NaCl + H2O So, getting the moles of either product tell you how many moles H2O produced. Molarity = moles of solute/Liters of solution moles of solute = Liters of solution * Molarity ( 30.00 mL = 0.03 liters ) Moles H2O = 0.03 Liters * 1 M 0.030 moles H2O produced =================
How many liters of sulfur trioxide will be produced when 4.0 liters of sulfur dioxide reacts with an excess of oxygen?
If everything is under gaseous condition and with equal pressure and temperature, then also 4.0 L SO3 gas is produced from 4.0 L SO2,g.
