Question

How many grams of water are produced if you combust 1.28 g of C6H14? The balanced equation is:

2C6H14 + 1902 - 12C02 + 14H2O

Answer 1

Step-by-step explanation:

according to the balance chemical equation

2 moles of c6h14 give us 14 moles of H2O

now mass(in gram) of 2 moles of C6H14 is

moles=mass/molar mass

mass=molar mass*moles

molar mass of C6H14 is 86 therefore

mass=86*2=172

now mass of 14 moles of water is

mass=molar mass*moles

molar mass of water is 18

mass=18*14=252

from the above calculations we conclude that

172 grams of C6H14 produce 252 grams of water

so 1.28 grams of C6H14 produce =252*1.28/172=1.87 grams of water

result is that 1.28 grams of C6H14 produced 1.87 grams of water