Answer:
a) 0.0860 moles butane
b) 0.559 moles O2
c) 17.9 grams O2
d) 0.344 moles CO2
e) 15.14 grams CO2
f) 0.430 moles H2O
g) 7.75 grams H2O
h) Total mass of reactants = 22.9 grams
Total mass of products ≈ 22.9 grams
The total mass of reactants should be the same as the total mass of products
Explanation:
Step 1: Data given
Mass of butane = 5.00 grams
Molar mass of butane = 58.12 g/mol
Step 2: The balanced equation
2C4H10 + 13O2 → 8CO2 + 10H2O
Step 3: Find the number of moles of butane in 5.00 grams?
Moles butane = mass butane / molar mass butane
Moles butane = 5.00 grams / 58.12 g/mol
Moles butane = 0.0860 moles butane
Step 4: Find the number of moles of oxygen that will react with 5.00g of butane?
For 2 moles butane we need 13 moles O2
For 0.0860 moles butane we'll need 6.5 0.0860 = 0.559 moles O2
Step 5: Find the number of grams of oygen that will react with the butane?
Mass O2 = moles O2 molar mass O2
Mass O2 = 0.559 moles 32.0 g/mol
Mass O2 = 17.9 grams O2
Step 6: Find the number of moles of carbon dioxide produced
For 2 moles butane consumed, we'll have 8 moles CO2
For 0.0860 moles butane we'll have 40.0860 = 0.344 moles CO2
Step 7: Find the number of grams of carbon dioxide produced
Mass CO2 = 0.344 moles 44.01 g/mol
Mass CO2 = 15.14 grams CO2
Step 8: Find the number of moles of water produced
For 2 moles butane consumed, we'll have 10 moles H2O
For 0.0860 moles we'll have 50.0860 = 0.430 moles H2O
Step 9: Find the number of grams of water produced
Mass H2O = 0.430 moles * 18.02 g/mol
Mass H2O = 7.75 grams H2O
Step 10: Find the total mass of the reactants and compare to the total mass of the products
Total mass of reactants = 5.00 grams + 17.9 grams = 22.9 grams
Total mass of products = 15.14 grams + 7.75 grams≈ 22.9 grams
The total mass of reactants should be the same as the total mass of products
