CH4(g)+2CO2(g)->CO2(g)+2H2O(g)
44g CO2(g) is obtained from 16 g CH4(g)
mole of CO2 g
=22g CO2(g)*1mol CO2/44g CO2
=0.5 mol CO2 (g)
Methane (CH4) has four atoms of hydrogen per molecule. If there are 3 moles of methane, then there are 12 moles of hydrogen.
8.02 / 16.04 = 0.5 moles
This is not a common reaction at standard temperature and pressure.
When methane undergoes complete combustion, the equation for the reaction is CH4 + 2 O2 -> CO2 + 2 H2O. This shows that the number of moles of carbon dioxide formed are the same as the number of moles of methane reacted, so that 14 moles of carbon dioxide will be formed from 14 moles of methane.
First a balanced chemical equation is needed.CH4 + 2O2 -> CO2 + 2H2OThere is a 1:1 ratio of moles between methane and carbon dioxide so the amount of moles of methane used is the exact number of moles of carbon dioxide yielded.To determine the number of moles of methane we take the amount used and divide by methane's mass which is about 16.04 g/mol.100g/ 16.04g/mol=6.234moles of methane.6.234 moles of methane are used and 6.234 moles of carbon dioxide are produced.
Methane (CH4) has four atoms of hydrogen per molecule. If there are 3 moles of methane, then there are 12 moles of hydrogen.
800 g oxygen are needed.
8.02 / 16.04 = 0.5 moles
This is not a common reaction at standard temperature and pressure.
the required equation is HgCl2+4KI>>2KCl+K2HgI4. according to stoichiometric calculations 4 moles of KI gives 1 mole of k2HgI4 THEREFORE 0.4 moles of K2HgI4 requires----- ? 0.4 moles x 4 moles/1 mole=1.6 moles therefore 1.6 moles of KI is required to produce 0.4 moles of K2HgI4
0.25 moles
When methane undergoes complete combustion, the equation for the reaction is CH4 + 2 O2 -> CO2 + 2 H2O. This shows that the number of moles of carbon dioxide formed are the same as the number of moles of methane reacted, so that 14 moles of carbon dioxide will be formed from 14 moles of methane.
If you think to 4 moles of methane the number is 24,088563428.10e+23.
First a balanced chemical equation is needed.CH4 + 2O2 -> CO2 + 2H2OThere is a 1:1 ratio of moles between methane and carbon dioxide so the amount of moles of methane used is the exact number of moles of carbon dioxide yielded.To determine the number of moles of methane we take the amount used and divide by methane's mass which is about 16.04 g/mol.100g/ 16.04g/mol=6.234moles of methane.6.234 moles of methane are used and 6.234 moles of carbon dioxide are produced.
Moles = weight (in g) / molecular weight = 0.289 / 16 = 0.0180 moles.
The complete combustion of methane proceeds according to the equation: CH4 + 2 O2 = CO2 + 2 H2O. Therefore, each mole of methane produces two moles of water and 4 moles of methane will produce eight moles of water.
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