2C2H2 + 5O2 --> 4CO2 + 2H20
How many grams of CO2 is produced when 2.50 x 10^4gC2H2 burns completely
2.50 x 10^4gC2H2 * 44.009gCO2/26.038gC2H2 = 4.23x10^4gCO2?
or am i wrong
you erred. You did not use the balanced equation coefficents.
2.50 x 10^4gC2H2 * 4*44.009gCO2/2*26.038gC2H2 = you do it.
Your calculation for finding the grams of CO2 produced when 2.50 x 10^4g of C2H2 burns completely is incorrect. Let's go through the steps again:
First, we need to calculate the molar mass of C2H2 (acetylene) and CO2 (carbon dioxide). The molar mass of C2H2 is 26.038 g/mol, while the molar mass of CO2 is 44.009 g/mol.
Next, we need to set up a conversion factor to convert grams of C2H2 to grams of CO2. This can be done using the ratio of the molar masses of the two compounds:
(44.009 g CO2 / 26.038 g C2H2)
Finally, we can calculate the grams of CO2 produced by multiplying the given mass of C2H2 by the conversion factor:
2.50 x 10^4 g C2H2 * (44.009 g CO2 / 26.038 g C2H2) = 4.23 x 10^4 g CO2
So, your calculation is correct. The correct answer is 4.23 x 10^4 g CO2.