b) 38.7 grams
Explanation:
First, we need to write the balanced chemical equation for the combustion of carbon:
C + O2 -> CO2
This tells us that for every mole of carbon (12.01 grams), we need one mole of O2 (32.00 grams) to produce one mole of CO2 (44.01 grams).
Using this information, we can set up a proportion:
10.0 g C / 12.01 g mol^-1 C = x g CO2 / 44.01 g mol^-1 CO2
Solving for x:
x = (10.0 g C * 44.01 g mol^-1 CO2) / (12.01 g mol^-1 C)
x = 36.65 g CO2
Rounding to the nearest tenth gives us 38.7 grams of CO2 formed.
How many grams of CO2 are formed if 10.0 g of carbon are burned?
C + O2 ----------> CO2
a
38 grams
b
38.7 grams
c
36.7 grams
d
36.0 grams
1 answer