CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ .
Calculate the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure
You forgot to include an --> in your reaction.
Convert 35.0 g of methanol to moles
The units of your reaction should have been kJ per mole of CH3OH.
All you have to do is multiply kJ/mole by moles
To calculate the amount of heat transferred (ΔH) when 35.0 g of CH3OH(g) decompose, we can use the concept of stoichiometry and the given enthalpy change (H).
1. Calculate the moles of CH3OH(g):
Molar mass of CH3OH (CH3OH(g)) = 32.04 g/mol + 1.01 g/mol + 16.00 g/mol = 32.04 g/mol + 1.01 g/mol + 16.00 g/mol = 32.04 g/mol
Moles of CH3OH(g) = mass / molar mass
Moles of CH3OH(g) = 35.0 g / 32.04 g/mol ≈ 1.092 mol
2. Use the stoichiometric coefficients of the reaction to determine the heat transferred:
From the balanced chemical equation, we see that 1 mole of CH3OH(g) decomposes to produce 1 mole of CO(g) and 2 moles of H2(g).
Therefore, the molar quantity of heat transferred (ΔH) is equal to the enthalpy change (H) for the reaction.
3. Calculate the heat transferred when 1.092 moles of CH3OH decompose:
Heat transferred per mole of CH3OH = ΔH / moles of CH3OH
Heat transferred per mole of CH3OH = +90.7 kJ / 1.092 mol ≈ 83.2 kJ/mol
4. Calculate the heat transferred when 35.0 g of CH3OH decompose:
Heat transferred = heat transferred per mole of CH3OH * moles of CH3OH
Heat transferred = 83.2 kJ/mol * 1.092 mol ≈ 90.7 kJ
Therefore, the amount of heat transferred when 35.0 g of CH3OH(g) decompose is approximately 90.7 kJ.
To calculate the amount of heat transferred in the given reaction, you can use the concept of heat transfer during chemical reactions, which is given by the equation:
q = mcΔT
Where:
q = heat transferred
m = mass of the substance
c = specific heat capacity of the substance
ΔT = change in temperature
In this case, we need to consider the heat of the reaction (H = +90.7 kJ) and the mass of the CH3OH(g) (35.0 g). Therefore, we need to find the ΔT (change in temperature) and the specific heat capacity for CH3OH(g).
However, since the reaction occurs at constant pressure, we can assume that ΔT is negligible. This means that there is no significant temperature change during the reaction. Therefore, we can simplify the equation to:
q = ΔH
Where:
q = heat transferred
ΔH = change in enthalpy (heat of the reaction)
Given that the change in enthalpy (ΔH) is +90.7 kJ, we can directly calculate the amount of heat transferred:
q = 90.7 kJ
Therefore, the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure is 90.7 kJ.