Write the two balanced quations, one for the incomplete combustion of methane (to form carbon monoxide and water vapor), and another one for the complete combustion of methane (forming carbon dioxide and whater vapor). What are the conditions, at which do you think the incomplete combustion might take place instead of the complete combustion? What is the health risk associated with this process?
CH4 (g) + 5/2 O2 (g) ( less amount or limited) ----------> CO (g) + 2 H2O (g)
CH4 (g) + 2 O2 (g) ( excess) ----------> CO2 (g) + 2 H2O (g)
The produced CO inhale by people in more amount then it is reacts with the blood and forms more stable complex carboxy haemoglobin which is more stable than oxyhaemoglobin complex. so insufficient amount of oxygen to the people become dies
Write the two balanced quations, one for the incomplete combustion of methane (to form carbon monoxide...
Write a balanced equation for the incomplete combustion of ethane (CH3CH3) to form carbon monoxide as one product.
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. mL flask at 20·°C with 4.9 atm of carbon monoxide gas and 2.5 atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains...
13. For each of the following, write a balanced chemical equation and QUALITATIVELY predict the signs for AH, AS, and AG. State whether each reaction is spontaneous, nonspontaneous, or at equilibrium. Justify your answers. (a) The combustion of methane (CHA) under standard conditions. (b) Vaporizing water at 373 K and I atm. (C) Forming methanol (CH3OH) and oxygen gas from water vapor and carbon dioxide at 500.0 °C. BE
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a flask at with of carbon monoxide gas and of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains of carbon monoxide gas, of water vapor...
ynthesis gas, a mixture that includes the fuels carbon monoxide and molecular hydrogen, is used produce liquid hydrocarbons and methanol. It is made at pressures up to 100 atm by oxidation of methane followed by the steam re-forming and water-gas shift reactions. Because the is exothermic, temperatures reach 950 1100°C, and the conditions are such that the amounts of hydrogen, carbon monoxide, carbon dioxide, methane and water leaving the reactor are close to the equilibrium amounts for the steam re-forming...
Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially A chemical engineer studying this reaction fills a 25.0 L tank at 21·°C with 5.4 mol of carbon monoxide gas and 3.8 mol of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains...
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 100.L tank with 45.mol of carbon monoxide gas and 33.mol of water vapor. When the mixture has come to equilibrium she determines that it contains 20.mol of carbon monoxide gas, 8.0mol of water vapor and 25.mol...
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially A chemical engineer studying this reaction fills a 125. L tank at 24. °C with 40. mol of carbon monoxide gas and 47. mol of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it...
Balanced equation: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Part B: What mass of carbon dioxide is produced from the complete combustion of 2.70×10−3 g of methane? Part C: What mass of water is produced from the complete combustion of 2.70×10−3 g of methane? PartD: What mass of oxygen is needed for the complete combustion of 2.70×10−3 g of methane?
A representative formula for a wax is C, HWrite a balanced equation for the combustion of the wax of the candle. CHO+O, Methane is burned as a source of energy. The formula for methane is CH, Again, write a balanced equation for the combustion of methane. CH, +0,- Most combustion gives off energy and the reaction is called an exothermic reaction. On which side of the equation will this energy be shown? To illustrate this redo the equation describing the...