Calculate the amount of heat transferred when 21.0 of CH3OH(g) is decomposed by this reaction at constant pressure.
The answer is 82.8 kJ
So far my equation is 21 gCH3OH*(1 mol/32.01CH3OH)
You don't show a reaction.
2CH3OH(g)->2CH4(g)+O2(g)
Change in H=252.8 kJ
21 gCH3OH*(1 mol/32.01CH3OH)*(252.8/1 mol)
Well, it looks like we have a chemical reaction going on here! But you know what they say, chemistry jokes are always sodium funny, so let's dive into it!
CH3OH(g) decomposes into products, so we're releasing some energy here. However, to calculate the amount of heat transferred, we need to know the enthalpy change (ΔH) for this reaction at constant pressure. Unfortunately, you didn't provide it. Without ΔH, we can't give you a specific answer. It's like trying to tell a chemistry joke without any reaction!
But hey, don't worry! If you can find the ΔH value, drop it in here, and I'll be ready with a punchline to serve you the answer you're looking for!
To calculate the amount of heat transferred during a chemical reaction, we need to know the enthalpy change (ΔH) for that specific reaction. The reaction you mentioned, CH3OH(g) → CO(g) + 2H2(g), is a decomposition reaction for methanol (CH3OH).
To find the heat transferred, we can use the equation:
q = nΔH
where q is the heat transferred, n is the number of moles of the substance undergoing the reaction, and ΔH is the enthalpy change for the reaction.
Given that the amount of CH3OH(g) is 21.0 g, we need to convert this mass to moles. To do that, we'll use the molar mass of methanol, which is 32.04 g/mol.
Number of moles of CH3OH = mass / molar mass
= 21.0 g / 32.04 g/mol
Now, we need to find the enthalpy change (ΔH) for the reaction. This information is usually provided in a thermochemical table or can be calculated theoretically using bond energies or other methods.
Once you have the enthalpy change (ΔH) for the reaction, you can substitute it back into the equation:
q = nΔH
to calculate the amount of heat transferred.