How many kilojoules of heat are released when 25.0 g of {\rm CO}(g) reacts completely with {\rm H_2}(g) to form {\rm CH_3OH}(g) at constant pressure?
To calculate the amount of heat released when a reaction occurs, you need to determine the change in enthalpy (ΔH) of the reaction and use the equation:
q = ΔH × n
q is the amount of heat released, ΔH is the change in enthalpy, and n is the number of moles of the substance undergoing the reaction.
In this case, the reaction is:
CO(g) + 2H₂(g) → CH₃OH(g)
First, you need to calculate the number of moles of CO(g) involved in the reaction. You can use the molar mass of CO (28.01 g/mol) to convert grams of CO to moles of CO:
n(CO) = mass(CO) / molar mass(CO)
n(CO) = 25.0 g / 28.01 g/mol
Next, you need to determine the change in enthalpy (ΔH) for the reaction. The ΔH is provided in the question or you can consult a reference source or database.
Finally, you can substitute the values into the equation:
q = ΔH × n(CO)
Calculate the value of q to get the amount of heat released in kilojoules.
think of your first paging.....the answer is written in the question!
dont give up Ryan!!