given this balance equation, C2H5OH+3O2=3H2O+2CO2 HOW MANY GRAMS OF CO2 ARE PRODUCED FROM 18.5 GRAMS OF OXYGEN GAS?
mols o2 gas = grams/molar mass
Using the coefficients in the balanced equation, convert mols O2 gas to mols CO2
Now convert mols CO2 to grams. grams = mols CO2 x molar mass CO2
All caps makes your post difficult to read.
To find out how many grams of CO2 are produced from 18.5 grams of oxygen gas, you need to use the balanced equation provided.
Step 1: Determine the molecular weight of O2 (oxygen gas).
Looking at the periodic table, the atomic weight of oxygen is approximately 16 grams per mole. Since oxygen gas (O2) consists of two oxygen atoms, the molecular weight of O2 is 2 * 16 = 32 grams per mole.
Step 2: Use stoichiometry to relate the amount of oxygen gas to CO2 produced.
Based on the balanced equation C2H5OH + 3O2 → 3H2O + 2CO2, we can see that for every 3 moles of O2, we get 2 moles of CO2.
Step 3: Convert grams of oxygen gas to moles.
Using the molecular weight of O2 (32 g/mol) calculated in Step 1, we can convert the mass of oxygen gas to moles.
18.5 grams of O2 * (1 mole/32 grams) = 0.5781 moles of O2
Step 4: Use the stoichiometry ratio to calculate the moles of CO2 produced.
Since the mole ratio between O2 and CO2 is 3:2, we can set up a proportion to find the moles of CO2 produced:
0.5781 moles of O2 * (2 moles of CO2/3 moles of O2) = 0.3854 moles of CO2
Step 5: Convert moles of CO2 to grams.
Using the molecular weight of CO2 (44 g/mol), we can convert the moles of CO2 to grams:
0.3854 moles of CO2 * (44 grams/1 mole) = 16.9456 grams of CO2
Therefore, approximately 16.95 grams of CO2 are produced from 18.5 grams of oxygen gas.