ethane gas, or dicarbon hexahydride, undergoes cmbustion to produce carbon dioxide gas and water vapor.
A. What mass of the un named reactant is required to react with 2.2 moles of ethane?
B. How amny molecules of the product with the smaller % composition of the non oxide component are produced if the reaction only goes 57.8% to completion?
I gave you some hints to work this problem day before yesterday. What did you do with them? Show your work if you need further assistance.
To answer both questions, we need to first balance the chemical equation for the combustion of ethane. The balanced chemical equation is:
C2H6 + O2 -> CO2 + H2O
A. To find the mass of the unnamed reactant required to react with 2.2 moles of ethane, we need to use stoichiometry. The stoichiometric ratio is given by the balanced equation. From the equation, we see that 1 mole of ethane reacts with 3 moles of oxygen.
So, for every 1 mole of ethane, we need 3 moles of the unnamed reactant.
Given that we have 2.2 moles of ethane, we can calculate the moles of the unnamed reactant:
2.2 moles ethane x (3 moles unnamed reactant / 1 mole ethane) = 6.6 moles unnamed reactant
B. To find the number of molecules of the product with the smaller percentage composition of the non-oxide component, we need to consider the percentage composition of carbon dioxide (CO2) and water vapor (H2O).
From the balanced equation, we see that for every 1 mole of ethane, we get 1 mole of CO2 and 3 moles of H2O. Since the reaction only goes 57.8% to completion, we can calculate the moles of the product formed.
For CO2:
2.2 moles ethane x (57.8 moles CO2/100 moles ethane) = 1.27 moles CO2
For H2O:
2.2 moles ethane x (57.8 moles H2O/100 moles ethane) = 1.27 moles H2O
Since we know that 1 mole of any compound contains Avogadro's number of molecules (6.022 x 10^23), we can calculate the number of molecules for each compound:
Number of molecules of CO2 = 1.27 moles CO2 x (6.022 x 10^23 molecules/mole) = 7.6474 x 10^23 molecules CO2
Number of molecules of H2O = 1.27 moles H2O x (6.022 x 10^23 molecules/mole) = 7.6474 x 10^23 molecules H2O
Therefore, the number of molecules of the product with the smaller percentage composition of the non-oxide component is 7.6474 x 10^23.