how many moles of carbon dioxide will be produced when 2.8 moles of oxygen react (consider the combustion of ethylene:
C2H4 + 3 Oxygen2 -->2CO2 +2H2Oxygen
2.8/3 = x/2
working it as a ratio with the coefficents.
can you explain where did the 2 come from also the 3, i'm not an expert at chemistry and i need explaination to see how to do these problems.
thank you
The 2 and 3 are coefficients in the balanced equation for O2 and CO2
To determine the number of moles of carbon dioxide produced when 2.8 moles of oxygen react, you need to use the balanced chemical equation.
The given balanced equation is: C2H4 + 3O2 --> 2CO2 + 2H2O
From the equation, you can see that for every 3 moles of oxygen (O2) consumed, 2 moles of carbon dioxide (CO2) are produced.
So, you need to use the stoichiometry ratio to find the number of moles of carbon dioxide produced.
Step 1: Identify the stoichiometry ratio for oxygen and carbon dioxide from the balanced equation.
From the equation, it is 3 moles of oxygen (O2) : 2 moles of carbon dioxide (CO2).
Step 2: Use the stoichiometry ratio to calculate the number of moles of carbon dioxide produced.
Given moles of oxygen = 2.8 moles.
Using the stoichiometry ratio, we can set up a proportion:
2.8 moles O2 / 3 moles O2 = x moles CO2 / 2 moles CO2
Cross-multiply and solve for x:
(2.8 moles O2 * 2 moles CO2) / 3 moles O2 = x moles CO2
x = (2.8 * 2) / 3 = 1.87 moles CO2
Therefore, 2.8 moles of oxygen will produce approximately 1.87 moles of carbon dioxide.