Assuming butane undergoes complete combustion in 1 mole of oxygen, 8/13 moles of carbon dioxide and 10/13 moles of water are formed.
Incomplete combustion of the butane. Which means that there is a lack of oxygen getting into the system. C4H10 + 4½O2 -> 4CO + 5H2O In excess O2 only CO2 and H2O are produced. C4H10 + 6½O2 -> 4CO2 + 5H2O
Burning of propane:CH3H8 + 5 O2 = 3 CO2 + H2OBurning of butane:2 CH4H10 + 13 O2 = 8 CO2 + 10 H2O
h2 is water because when divide by 2 equals into 5 so i am very handsome
Balanced equation first. 2H2 + O2 >> 2H2O 1.42 mol H2 ( 1mol O2/2mol H2 ) = 0.71mol O2 to react with H2
No; 1 mole of molcular oxygen (O2) is 31,998 g and 1 mole of sulfur (S) is 32,06 g.
They will react together. will form O2 and H2O as results.
CH4 + 2O2 gives CO2 and 2H2O.So 16g of CH4 react with 64g of O2.So 24g react with 96g of O2
how do metals react with oxygen
2so2 + o2 ----> 2so3
Incomplete combustion of the butane. Which means that there is a lack of oxygen getting into the system. C4H10 + 4½O2 -> 4CO + 5H2O In excess O2 only CO2 and H2O are produced. C4H10 + 6½O2 -> 4CO2 + 5H2O
They react to form sulphuric acid. 2 SO2 + 2 H2O + O2 → 2 H2SO4
First you must find out what mass of each would react perfectly, then, if you have more than is needed of one of the reactants (if it is in excess) all of the reactant will react. Here is the calculation you need, for example, say you have 50g of each reactant. Step 1-Write out formula of reactants Mg + O2 = MgO2 1mole 1 mole Step 2 - Find the gram formula mass of reactants 1 mole Mg= 24.3 g 1 mole O2= 32 g 24.3g Mg reacts with 32g O2 Step 3 - Find amount required to react 50g Mg -- 50/32x24.3 =37.9 =37.9g Mg From that we can see that since there is 37.5g Mg and only 24.3g is needed to react completely with O2, the Mg is in excess. Substitute your starting weights in there and use that calculation, and add more than the required amount, that way you can be sure.
It is ethanol, normal alcohol, it burns with oxygen from air.The balanced reaction equation is:CH3CH2OH + 3 O2 --> 2 CO2 + 3 H2O
Burning of propane:CH3H8 + 5 O2 = 3 CO2 + H2OBurning of butane:2 CH4H10 + 13 O2 = 8 CO2 + 10 H2O
Assuming no change in temperature and pressure, calculate the volume of O2 (in liters) required for the complete combustion of 14.9 L of butane (C4H10):
2.24 L O2 (= 0.100 mol O2) is needed to react with 0.200 moles of SO2 to form SO3
h2 is water because when divide by 2 equals into 5 so i am very handsome