Consider the following balanced equation for the combustion of butane, a fuel of

Question

Consider the following balanced equation for the combustion of butane, a fuel often used in lighters. 2 C_4H_10 (g) + 13 O_2(g) rightarrow 8 CO_2 (g) + 10 H_2O(g) Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.

Explanation / Answer

2 C4H10 (g) + 13 O2 (g)--------à 8 CO2 (g) + 10 H2O (g)

Calculate molar mass of each species, and then compare with each other.

Molar mass of C4H10 = 58 g/mol

Molar mass of O2 = 32 g/mol

Molar mass of CO2= 44 g/mol

Molar mass of H2O = 18 g/mol

Mass of C4H10                Mass of O2                       Mass of CO2                    Mass of H2O

0.59g                                 2.11g                                 1.79g                                 0.91g

5.12g                                 18.36g                               15.54g                               7.94g

5.38g                                 19.29g                               16.32g                               8.35g    

5.70g                                 20.43g                               17.28g                               8.84g

212g                                   760.27g                                           643.31g                                           328.97g

45.48g                               163.09g                                           138g                                  70.57g

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.