What happens if 0.1 mole methane reacts with 0.1 mole oxygen gas?
Lets start with the reaction of methane fully reacting with oxygen:
CH4 + 2 O2 --> CO2 + 2 H2O
The ratio CH4:O2 is 1:2
So 0.1 mole of methane can potentially react with 0.2 mole of oxygen.
Seeing as we only have 0.1 mole oxygen we know that we have excess of methane.
Because of the lack of oxygen the methane can form carbonmonoxide (CO) instead of CO2.
(if someone knows the composition of the final product, please add here. As far as i know, you cant predict the CO:CO2 ratio.)
If 1 mole of methane reacts with oxygen to produce carbon dioxide and water what is the mass of water produced?
The reactants when methane burns in oxygen are methane and oxygen. The products are CO2, water and heat about 890 Kj/mole is given out. The equation is : CH4(g) + 2O2 _______> CO2 + 2H2O + Heat (-890 Kj/mole) When one mole of methane gas reacts with (burns in) 2 moles of oxygen gas we get 1 mole of carbon dioxide and 2 moles of water and 890 Kilo joules of heat is released. This…
Use the mole ratio to determine the number of moles of carbon dioxide produced when 0.136 mole of propanol reacts with excess oxygen in a combustion reaction?
HOOH + NaOCl ---------> H2O + NaCl + O2 I mole of hydrogen peroxide reacts with 1 mole of sodium hypochlorite (bleach) to form 1 mole each of sodium chloride, water, and diatomic oxygen gas. Macroscopically there will be a large release of oxygen gas, potentially hazardous if the release is too quick
Natural gas + Oxygen -> Carbon dioxide + Water eg: CH4 + 2O2 -> CO2 + 2H2O Where complete combustion of methane (CH4, a natural gas) is achieved. After stating what precisely is meant by 'natural gas' (could be methane o.s.e.) then, in words, it could be something like: "One mole of the natural gas 'methane' reacts with two moles of oxygen to form one mole of carbon dioxide and two moles of water" Well…
The equation for the combustion of methane is CH4 + 2 O2 -> CO2 + 2 H2O. This means that for every mole of methane, two moles of oxygen are needed. In .009 g of methane, there are .00561 moles (molar mass of methane: 16.0425 g/mol). So there are .01122 moles of oxygen, meaning that with a molar mass of 31.9988 g/mol, there are .18 grams of O2 needed.
Is this reaction Endothermic The combustion of propane in oxygen to produce carbon dioxide and water vapor. And does methane or propane produce more energy combustion I just dont understand this?
All the combustion reactions I know of are exothermic because heat is released instead of absorbed. And propane gives more energy than methane cause it has more Cs and Hs to react with Oxygen, so one mole of propane will react more and form more product than one mole of methane and giving out more energy. All the combustion reactions I know of are exothermic because heat is released instead of absorbed. And propane gives…
With any chemical reaction you have reactants and products, for this question I'll use the example of the formation of water from it's parts, Hydrogen and Oxygen. The equation would look like this: 2H2 (g) + O2 (g) -> 2H2O (l) Let's say you start out with 3 moles of Hydrogen and 1 mole of Oxygen. From the reaction you can see that for every mole of O2 that reacts, 2 moles of H2 are…
CH4 + 2 O2 --> CO2 + 2 H2O x / 64 = 1 / 16 x = 4 g oxygen Assuming oxygen is 20% oxygen... 4 = .2 x x = 20 g air that is one possible answer. A better answer--- air is 20% oxygen by volume and 80% nitrogen by volume. 1g methane / 16 = 0.0625 mole 0.0625 / 1mole meth = x / 2mole oxy x = 0.125 mole oxygen…
Methane gives off more heat. Burning something is an oxidation reaction. Energy is released by forming more and more bonds between carbon and oxygen. Since methyl alcohol already has a C-O bond, it is already more oxidized than methane, so burning methyl alcohol releases less energy (heat) than burning methane (mole for mole).
The coefficients are the numbers written in front of the chemical formulas in a chemical equation, and tells how much of a certain substance is involved in the reaction. When there is no number, it is understood to be one. For example, the following equation, which represents the combustion of methane (CH4), could be read in a couple of different ways. CH4 + 2O2 --> CO2 + 2H2O One molecule of methane plus two molecules…
The solving of mole to mole problems through stoichiometry is based in ratios. Assuming the reaction formulas are simplified and balanced the moles consumed and produced can be calculated. For example in the simple combustion reaction of ethane and oxygen of:CH4 + 2O2 = CO2 +2H20 we see a molar ratio of 1:2 between methane combusted and waters produced.
When gasoline is heated in the presence of hydrogen gas and a catalyst the gasoline cracks During the cracking gasoline decomposes to 1 mole of methane 2 mole of ethane and 1 mole of propane for?
However, the surface oxide layer is not very thick, so in practical terms the difference is going to be small (and since the total mass of a current US penny is 2.5 grams and only 2.5% of that is copper, even if every bit of copper were totally oxidized we're talking about a mass difference of well under 1%).