a) Calculate the molar ratio of carbon / hydrogen in the fuel and use the result to prove that the fuel cannot be natural gas. b) Assuming that C, H and S are the elements present in the fuel, calculate the mass carbon / hydrogen ratio and the weight% ratio of sulfur in the fuel.
Suppose you are hired by the Environmental Protection Agency as an engineer to measure sulfur dioxide (SO2) emissions in a small industrial power plant. And suppose you analyze a gas sample and get the following composition: 75.66% N2, 10.24% CO2, 8.27% H2O, 5.75% O2, and 0.0825% SO2. You show these figures to the factory clerk the next day, and he insists that this analysis is erroneous and states that the fuel is natural gas, contains methane and ethane and does not contain sulfur. You ask if another fuel is used, and sometimes they say they use fuel as fuel, but at the time of analysis they say that this fuel is not used. However, your measurements show that the enterprise is using fuel at the time of measurement, and the responsible person accepts this later and accepts that they have made mistakes.
a) Calculate the molar ratio of carbon / hydrogen in the fuel and use the result to prove that the fuel cannot be natural gas.
b) Assuming that C, H and S are the elements present in the fuel, calculate the mass carbon / hydrogen ratio and the weight% ratio of sulfur in the fuel.
Hint: Take the foundation from the gas at the outlet and go through atomic balance. C / H: 0.25 for methane (CH4), C / H: 0.333 for ethane (C2H6).
Reactions: C + O2 = CO2, 2H + 0.5O2 = H2O, S + O2 = SO2
H2: 2 g / mol, H2O: 18 g / mol, CO2: 44 g / mol, CH4: 16 g / mol, SO2: 64 g / mol, N2: 28 g / mol.
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
