A rigid stainless steel chamber contains 180 Torr of methane, CH 4 , and excess oxygen, O 2 , at 160.0 °C. A spark is ignited in
side the chamber, completely combusting the methane. What is the change in total pressure within the chamber following the reaction? Assume a constant temperature throughout the process.
No pressure will change in the chamber at reactions end
Explanation:
CH4 + 2O2 ---> CO2 + 2H2O
According the above reaction
There are 3 moles total of gaseous reactants, and 3 moles total of gaseous products, so this reaction results in no change of volume. Therefore, since this happens at constant volume and constant temperature, the pressures are directly related to the moles used and produced. This way, no pressure will change in the chamber at reactions end
Ethanol is polar because the oxygen atoms attract electrons because of their higher electronegativity than other atoms in the molecule. Thus the -OH group in ethanol has a slight negative charge. Ammonia (NH3) is polar. Sulfur dioxide (SO2) is polar.
