Final answer:
The flammability limits of acetylene are from 2.5% to 12.5% by volume. The empirical formula for acetylene is CH, and the molecular formula is C2H2. Using stoichiometry and ideal gas laws, the volume of oxygen needed for the combustion of acetylene can be calculated for practical applications.
Step-by-step explanation:
The question pertains to the flammability limits of acetylene gas, which are important for safety considerations when using acetylene as a fuel in welding torches.
The correct answer for the flammability limits of acetylene is option B) 2.5% to 12.5% by volume. This range indicates the concentration of acetylene in the air between which it can ignite and burn. In concentrations below 2.5% or above 12.5%, acetylene will not burn as the mixture is too lean or too rich, respectively.
Finding the empirical formula of a compound requires calculating the simplest whole-number ratio of elements in the compound. For acetylene, with 92.3% carbon and 7.7% hydrogen by mass, the empirical formula can be determined to be CH.
To find the molecular formula, we need to use the provided data of acetylene's mass and volume under given conditions to determine its molar mass, which lets us relate the empirical formula to the actual molecular formula of the gas, which is C2H2.
In the combustion of acetylene, acetylene gas reacts with oxygen to form carbon dioxide and water. Using stoichiometry and ideal gas laws, calculations involve finding the required volume of oxygen gas to combust a certain volume of acetylene, leading to the determination of how many tanks of oxygen would be needed for the full combustion of the provided acetylene. This exemplifies the practical application of chemical reaction equations in real-world problems.