Consider the following balanced equation for the combustion ofbutane, a fuel often used in lighters:
2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)
Complete the following table, showing the appropriate masses ofreactants and products. If the mass of a reactant is provided, fillin the mass of other reactants required to completely react withthe given mass, as well as the mass of each product formed. If themass of a product is provided, fill in the required masses of eachreactant to make that amount of product, as well as the mass of theother product that is formed.
| Mass C4H10C4H10 | Mass O2O2 | Mass CO2CO2 | Mass H2OH2O |
| _____ | 2.11 gg | _____ | _____ |
| 5.52 gg | _____ | _____ | _____ |
| _____ | _____ | 10.12 gg | _____ |
| _____ | _____ | _____ | 8.04 gg |
| 222 mgmg | _____ | _____ | _____ |
| _____ | _____ | 128 mgmg | _____ |
