Final answer:
The claim that a gas reacts with oxygen in a one-to-three ratio to produce a blue flame is false. Methane combusts with oxygen in a one-to-two ratio, yielding carbon dioxide and water vapor with a blue flame indicating complete combustion.
Step-by-step explanation:
The statement suggesting that a gas reacts with oxygen in a one-to-three ratio to produce a blue flame is false. The burning of methane (CH4), a common gas used in burners, reacts with oxygen in a one-to-two ratio as demonstrated in the equation: CH4 (g) + 2O2 (g) = CO2 (g) + 2H2O(g). This stoichiometry indicates that each methane molecule requires two oxygen molecules to combust completely, yielding carbon dioxide and water as products. A blue flame typically signifies complete combustion, indicating a sufficient supply of oxygen.
It is important to note that while combustion reactions often involve oxygen and some type of fuel, like the liquid fuel/oxidant mixture or solid mixture mentioned, the specific ratios of reactant gases depend on the chemical identities of the substances involved. In the context of a Bunsen burner, the typical reaction uses methane, which requires two molecules of oxygen for each molecule of methane, resulting in a blue flame when the combustion is complete.