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Methane is a chemical compound with the chemical formula CH|4. It is the simplest alkane, and the principal component of natural gas. Methane's bond angles are 109.5 degrees. Burning methane in the presence of oxygen produces carbon dioxide and water. The relative abundance of methane
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Question:i believe i have correctly correctly balanced the combustion equation.
CH4 + 2O2 -----> CO2 + 2H2O
using formula n = m / Mm
the no. of moles of CH4 = 0.093505
is this equal to the number of moles of the CO2 or is further working required?
Answers:Yes, as can be seen from the balanced reaction, there is 1 mole of CO2 produced for every 1 mole of CH4 reacted. Thus moles of CH4 = moles of CO2 = 0.09375 moles CO2. Since you need grams of CO2, simply multiply by molar mass of CO2 (or about 44 g/mol).
grams of CO2 = 0.09375 mol x 44g/mol = 4.125 g CO2
Question:A furnace that provides heat by buring methane gas (CH) must have the correct mixture of air and fuel to operate effeciently. What is the mole ratio of air to methane gas in
the combustion of methane? Hint Air is 20% oxygen.
Answers:Methane = CH4
CH4 + 2 O2 --> CO2 + 2H2O
molar ratio of O2 to CH4 = 2 to 1
molar ratio of air to CH4 = 10 to 1
Question:How many grams of methane gas must be combusted to heat 1.15kg of water from 23.0 to 88.0 , assuming as a product and 100% efficiency in heat transfer?
Answers:I advise you to make it your self follow the following steps
1- right the equation as of the reaction as follow
CH4 + O2-----CO2 + 2H2O
2- calculate the energy needed to break the following bonds.
a-4 bonds of C-H
b- Calculate the energy needed to break 2of O=O bond
Add a+b this will be the energy reactants.
3- calculate the energy produced on formation of the products
a1- calculate the energy needed to form 2C=O
b2- calculate the energy needed to form 4 H-O
add a1 +b2= that will be the energy produced
4- calculate the reaction energy using the following
Energy of the reaction = energy of product- energy of reactants
5- calculate the energy needed to heat 1.15kg of water from 230 to 88.0
Answers:4 CH4 + 3O2 >> 2C2H2+ 6 H2O
Methane Bubbles Combustion Reaction :A chemistry teacher demonstrating the combustion of methane bubbles. CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (l)
Combustion of acetylene (Pembakaran asetilena) :Experiment about the combustion of acetylene, Info of acetylene:Acetylene (systematic name: ethyne) is the chemical compound with the formula C2H2. It is a hydrocarbon and the simplest alkyne. This colorless gas is widely used as a fuel and a chemical building block. It is unstable in pure form and thus is usually handled as a solution. As an alkyne, acetylene is unsaturated because its two carbon atoms are bonded together in a triple bond. The carbon-carbon triple bond places all four atoms in the same straight line, with CCH bond angles of 180 . Since acetylene is a linear symmetrical molecule, it possesses the D h point group. Acetylene was discovered in 1836 by Edmund Davy who identified it as a "new carburet of hydrogen". It was rediscovered in 1860 by French chemist Marcellin Berthelot, who coined the name "acetylene". Berthelot was able to prepare this gas by passing vapours of organic compounds (methanol, ethanol, etc.) through a red-hot tube and collecting the effluent. He also found acetylene was formed by sparking electricity through mixed cyanogen and hydrogen gases. Berthelot later obtained acetylene directly by passing hydrogen between the poles of a carbon arc. Today acetylene is mainly manufactured by the partial combustion of methane or appears as a side product in the ethylene stream from cracking of hydrocarbons. Approximately 400000 tonnes are produced this way annually.Its presence in ethylene is usually undesirable because of its explosive character ...