Ethane gas, or dicarbon hexahydride, undergoes combustion to produce carbon dioxide gas and water vapor.
A.) What mass of the un named reactant is required to react with 2.20 moles of ethane?
B.) How many molecules of the porduct, with the smaller percent composition of the non-oxide component, are produced if the reaction only goes 57.8 percent to completion?
A. Write and balance the equation.
2C2H6 + 7O2 ==> 4CO2 + 6H2O
2.2 moles C2H6 x (7 moles O2/2 moles C2H6) = ??moles O2.
B. I gave you the link for solving this problem earlier. You may not know what product is being discussed; you can calculate percent composition easily.
%C in CO2 = (12/molar mass CO2)*100= ??
%H in H2O = (2/molar mass H2O)*100 = ??
Write the formula for dicarbon hexa hydride
CO2+H2O
To solve these questions, we need to use the balanced equation for the combustion of ethane:
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
A.) We need to determine the mass of the unknown reactant required to react with 2.20 moles of ethane. To do this, we'll use stoichiometry.
Step 1: Find the molar ratio between the unknown reactant and ethane.
From the balanced equation, we see that the stoichiometric ratio between unknown reactant (X) and ethane (C2H6) is 2:2. This means that for every 2 moles of C2H6, we need 2 moles of X.
Step 2: Convert moles of ethane to moles of the unknown reactant.
Since we have 2.20 moles of ethane, we can use the molar ratio to calculate the moles of X:
2.20 moles C2H6 × (2 moles X / 2 moles C2H6) = 2.20 moles X
Step 3: Convert moles of the unknown reactant to grams.
To convert moles to grams, we need to know the molar mass of the unknown reactant.
B.) We need to determine the number of molecules of the product with the smaller percent composition of the non-oxide component if the reaction only goes 57.8 percent to completion.
Step 1: Calculate the theoretical yield.
The theoretical yield is the maximum amount of product that can be obtained from the given amount of reactant. In this case, it will be based on the limiting reactant.
Step 2: Calculate the actual yield.
To calculate the actual yield, we multiply the theoretical yield by the percent yield (given as 57.8%) and convert it to the number of molecules.
This way, we can find the mass of the unnamed reactant in question A and the number of molecules of the product in question B.