Question

Acetylene (C_2H_2) burns in oxygen (O_2) to produce carbon dioxide (CO_2) and water (H_2O). 8.64 L of gaseous acetylene (C_2H_2) is burned at STP according to the equation:

A) C_2H_2 + 2.5O_2 → 2CO_2 + H_2O
B) 2C_2H_2 + 5O_2 → 4CO_2 + 2H_2O
C) 4C_2H_2 + 10O_2 → 8CO_2 + 4H_2O
D) 3C_2H_2 + 7.5O_2 → 6CO_2 + 3H_2O

Answer 1

To determine how many tanks of oxygen are required to burn the acetylene, we need to use stoichiometry and the given balanced equation.

Step-by-step explanation:

To determine how many tanks of oxygen are required to burn the acetylene, we need to use stoichiometry and the given balanced equation: 2C₂H₂ + 5O₂ → 4CO₂ + 2H₂O.

First, convert the volume of acetylene gas to moles using the ideal gas law. Then, use the mole ratio from the balanced equation to find the moles of oxygen required. Finally, convert the moles of oxygen to the volume of oxygen gas using the ideal gas law.

By following these steps, you will be able to determine how many tanks of oxygen are needed to burn the acetylene gas.