If by "air" you mean oxygen, then the mole ratio can by found by balancing a reaction equation. CH4 + 202 -> CO2 + 2H2O The ratio is 1:2.
The balanced chemical equation for the combustion of methane is CH4 + 2O2 -> CO2 + 2H2O. This means that the mole ratio of air to methane gas is 2:1, as two moles of oxygen from the air are required to react with one mole of methane gas.
The stoichiometric air-fuel ratio for nitromethane (CH3NO2) is approximately 1.7:1, which means that 1.7 moles of air are needed for every mole of nitromethane to achieve complete combustion. This ratio is based on the stoichiometry of the reaction between nitromethane and oxygen (O2) in air.
Methane gas settles down because methane gas is heavier than and is carried by the upward displacement of air. ---------------------------------------------- The density of methane is 0,717 g/L and the density of air is 1,2 g/L at 0 0C; consequently methane gas raise in the air.
For complete combustion of 1g of methane (CH4), 4g of oxygen (O2) is required. This would result in the formation of 3g of carbon dioxide (CO2) and 2g of water (H2O). The total mass of air involved will be 4g of oxygen plus the mass of nitrogen present in air.
The mole fraction of oxygen gas in air is approximately 0.21. This means that out of every 1 mole of air, 0.21 moles are oxygen gas molecules.
The balanced chemical equation for methane (CH4) burning in air (O2) is: CH4 + 2O2 → CO2 + 2H2O
Wrong air/fuel ratio Poor atomisation of fuel Poor spark Incorrect timing of spark
The stoichiometric air-fuel ratio for nitromethane (CH3NO2) is approximately 1.7:1, which means that 1.7 moles of air are needed for every mole of nitromethane to achieve complete combustion. This ratio is based on the stoichiometry of the reaction between nitromethane and oxygen (O2) in air.
air,fuel and a heat source
Methane gas settles down because methane gas is heavier than and is carried by the upward displacement of air. ---------------------------------------------- The density of methane is 0,717 g/L and the density of air is 1,2 g/L at 0 0C; consequently methane gas raise in the air.
Yes methane is lighter than air because it is less dense than air.
For complete combustion of 1g of methane (CH4), 4g of oxygen (O2) is required. This would result in the formation of 3g of carbon dioxide (CO2) and 2g of water (H2O). The total mass of air involved will be 4g of oxygen plus the mass of nitrogen present in air.
The fact that it oxidizes in air is a chemical property of methane.
The specific gravity of methane at 25°C is around 0.554. This value represents the ratio of the density of methane to the density of air at the same temperature and pressure.
Flatulence contains a portion of methane gas, and the methane portion is lighter than air.
Yes, methane can explode when there is a sufficient amount mixed with air in the presence of an ignition source. Methane is highly flammable and can form explosive mixtures in the air at certain concentrations.
nowhere
combustible?