Question

For the balanced equation, I got: C6H12+9O2=6CO2+6H2O...is this correct?

A student in the chemistry lab reacted liquid hexane (C_6H_14) with oxygen of the air to produce carbon dioxide gas and liquid water. Write a balanced chemical equation for the reaction How many O_2 molecules are required to react completely with 48.8 g of C_6H_14? How many grams of carbon dioxide are produced from 48.8 g of C_6H_14?

Answer 1

a) Balanced equation is 2C_6H_14 + 19O_2 rightarrow 12CO_2 + 14H_2O b) no.of C_6H_14 given = 48.8g/869 g/mole = 0.567 mole from the reaction 2 moles of C_6H_14 react with 19 moles of O_2 then 0.567 moles of C_6H_14 react with 19 times 0.567/2 = 5.39 moles of O_2 has 6.023 times 5.39 times 10^23 = 3.25 times 10^24 molecule c) from the reaction 2 moles of C_6H_14 produces 12 moles of CO_2 then 0.567 moles of C_6H_14 = 12 times 0.567/2 = 3.402 moles of CO_2 Therefore mass of CO_2 formed = 3.402 moles times 44 g/mole = 149.68 grams