Question

what is mass of theoretical oxygen (kg) required for full combustion of 200L methanol and what...

what is mass of theoretical oxygen (kg) required for full combustion of 200L methanol and what is m^3 of CO2 produced (unit:m^3) at that time in the standard state


(The weight of methanol is 0.8)

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What mass of oxygen is required for complete combustion (to CO2 and H2O) of 227 g...
What mass of oxygen is required for complete combustion (to CO2 and H2O) of 227 g of butane. Using balanced equation 2C4H10 + 13O2---> 8 CO2 + 10 H2O.
Certain race cars use methanol (CH3OH; also called wood alcohol) as a fuel. Methanol has a...
Certain race cars use methanol (CH3OH; also called wood alcohol) as a fuel. Methanol has a molecular mass of 32.0 g/mol and a density of 0.79 g/mL. The combustion of methanol occurs according to the following equation: 2CH3OH + 3O2 → 2CO2 + 4H2O In a particular reaction 2.00 L of methanol are reacted with 80.0 kg of oxygen. What is the limiting reactant? What reactant and how many grams of it are left over? How many grams of carbon...
15. Consider the following combustion reaction of propane. 3C3H8 + 5O2 → 3CO2 + 4H2O a)...
15. Consider the following combustion reaction of propane. 3C3H8 + 5O2 → 3CO2 + 4H2O a) What mass of O2 , in g, would be needed to react with 0.421 kg of C3H8? b) What mass of CO2 , in g, would be produced from the combustion of 0.421 kg of C3H8 with excess oxygen?
1. A combustion chamber is fed with 50 kmol/h of butane and 2000 kmol/h of air....
1. A combustion chamber is fed with 50 kmol/h of butane and 2000 kmol/h of air. Calculate the % excess air used and composition of the gases leaving combustion reactor, assuming complete combustion of butane. 2. In manufacture of chlorine, feed containing hydrochloric acid gas and air are fed to the reactor. The product gases leaving the reactor are found to contain 13.2% HCl, 6.3% 02, 42.9% N2, 30% Cl2 and 7.6% H2O (by weight). Calculate: i) The percent excess...
Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043...
Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043 g of CO2 and 0.5670 g of H2O. The molar mass is 532.7 g/mol. What is the molecular formula of the compound?
Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043...
Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043 g of CO2 and 0.5670 g of H2O. The molar mass is 532.7 g/mol. What is the molecular formula of the compound?
C2H5OH + 3O2 --> 2CO2 + 3 H2O If the combustion uses 55.8 mL of oxygen...
C2H5OH + 3O2 --> 2CO2 + 3 H2O If the combustion uses 55.8 mL of oxygen measured at 2.26 atm and 40 degrees Celsius, what volume of CO2 is produced when measured at STP?
1=What mass of water is produced from the complete combustion of 7.30×10−3 g of methane? 2-What...
1=What mass of water is produced from the complete combustion of 7.30×10−3 g of methane? 2-What mass of oxygen is needed for the complete combustion of 7.30×10−3 g of methane?
Ammonia reacts with oxygen gas to form nitrogen monoxide and water. What maximum mass (theoretical yield)...
Ammonia reacts with oxygen gas to form nitrogen monoxide and water. What maximum mass (theoretical yield) of nitrogen monoxide can be produced if 1.00 mol each of ammonia and oxygen gas were mixed ? -37.5g -24.0g -48.0g -17.0g -30.0g
What is the enthalpy of combustion (in kJ/mol) for methanol (CH3OH) under standard conditions (water is...
What is the enthalpy of combustion (in kJ/mol) for methanol (CH3OH) under standard conditions (water is produced as a liquid)? Use the appendix in your textbook, do not enter units, and answer with 4 significant digits. The answer is not -1453 or -726.5