A mole of methane reacts with 64g of oxygen at 1 atm, 425 K. There are two ways in which methane can react with oxygen. It can either form water vapor and carbon dioxide or water vapor and carbon monoxide. After reaction the final gas density is 0.7282 g/L.
What is the fraction of methane that reacted to produce CO2? What is the fraction of methane that reacted to produce CO?
(Assume that methane is fully reacted)
Can someone just guide me in the right direction?
Here's what I have so far:
64g O2 --> 2 mol O2
CH4 + 2 O2 --> 2 H2O + CO2
2 CH4 + 3 O2 --> 4 H20 + 2 CO
A mixture og gases has a total pressure off 28.3 atm, it is made of: 5.8 atm of hydrogen gas, 7.2 atm of nitrogen gas, 3.5 atm of oxygen gas and some amount of methane. What is the pressure of methane? what is the pressure of
My question is more conceptual. It is expressed in a series of two problems: What energy change occurs when 1.2 moles of methane combust with an enthalpppy change of -434 KJ? CH4+2O2 TO CO2+2H20 I understand it is simply the moles
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