Question

2CH₃OH(g)-->2CH₄(g)+O2(g),?H=+252.8 kJ

For a given sample of CH₃OH , the enthalpy change during the reaction is 82.6kJ . What mass of methane gas is produced?

Answer 1

Using stoichiometry and the provided enthalpy change, the mass of methane gas produced can be calculated by setting up a proportion with the reaction's enthalpy change and converting the resulting moles to mass using the molar mass of methane.

Step-by-step explanation:

When considering the reaction 2CH₃OH(g) → 2CH₄(g) + O₂(g), with an enthalpy change (∆H) of +252.8 kJ, we can use stoichiometry to determine the mass of methane gas produced, given that the enthalpy change during the reaction is 82.6 kJ for a specific sample of CH₃OH. First, we establish a ratio based on the provided enthalpy change:

252.8 kJ of heat → 2 moles of CH₄ (32 g of CH₄)

82.6 kJ of heat → x moles of CH₄

By setting up a proportion, x can be found as follows:

x = (82.6 kJ * 2 moles of CH₄) / 252.8 kJ

Once x is determined, we can convert moles of CH₄ to mass using the molar mass of CH₄ (16.04 g/mol). The stoichiometry and enthalpy changes are crucial to solving this problem.