2C2H6 + 7O2 --> 4CO2 + 6H20 given 7.5 X 10 to the 3rd of C2H6 how many grams of CO2 is emitted
the 7.5 x 10 to the third is 7500 what do i do to figure out the rest
4/2 = 2 mols of CO2 for every mol of C2H6
mol of C2H6 = 2*12+6 = 30 g
mol of CO2 = 12+32 = 44 g
7500 * 2 * 44/30
The following procedure will work these stoichiometry problems.
1. Write and balance the equation. You have that.
2. Convert What you have (C2H6) to mols. mols = grams/molar mass = ?
3. Using the coefficients in the balanced equation, convert mols what you have (C2H6) to mols of what you want (CO2).
4. Now convert mols of what you want (CO2 in this case) to grams. g = mols x molar mass = ?
To figure out the number of grams of CO2 emitted, you need to use the stoichiometry of the balanced chemical equation. The stoichiometry tells you the quantitative relationship between the reactants and products in a chemical reaction.
In the balanced equation, the coefficient of C2H6 is 2, which means that for every 2 moles of C2H6, you produce 4 moles of CO2. Therefore, the ratio of moles of CO2 to moles of C2H6 is 4/2, which simplifies to 2/1.
Given that you have 7.5 x 10^3 moles of C2H6, you can set up the following calculation:
moles of CO2 = (moles of C2H6) x (moles of CO2 / moles of C2H6)
Let's plug in the values:
moles of CO2 = (7.5 x 10^3 moles C2H6) x (2 moles CO2 / 1 mole C2H6)
Now, you can calculate the moles of CO2:
moles of CO2 = 7.5 x 10^3 moles C2H6 x 2/1 = 1.5 x 10^4 moles CO2
Finally, to convert moles of CO2 to grams, you need to use the molar mass of CO2, which is 44.01 g/mol. The formula to convert moles to grams is:
grams of CO2 = (moles of CO2) x (molar mass of CO2)
Plugging in the values:
grams of CO2 = (1.5 x 10^4 moles CO2) x (44.01 g/mol) = 6.6 x 10^5 g CO2
Therefore, if you have 7.5 x 10^3 moles of C2H6, approximately 6.6 x 10^5 grams of CO2 will be emitted.