The combustion of liquid ethanol (C2H5OH)(C2H5OH) produces carbon dioxide and water. After 4.63 mLmL of ethanol (density=0.789g/ml)(density=0.789g/ml) was allowed to burn in the presence of 15.50 gg of oxygen gas, 3.70 mLmL of water (density=1.00g/ml)(density=1.00g/ml) was collected.   Determine the theoretical and percent yeild of h2o in the reaction.

Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining

Which reaction would it be possible to calculate (Triangle H)?

The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5  × 104 kJ of heat?                                            2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ