How many kilojoules of heat are released when 38.6g of CH4 reacts completely with O2 to form CH3OH at constant pressure?

303 kJ

2CH4 + O2 ==> 2CH3OH

dHrxn = (n*dHf products) - (n*dHf reatants). You will need to look up the values for delta Hoformation for CH4 and CH3OH. Let's call that value comb.

comb x (38.6g/2*molar mass CH4) = ?

Ah, let me calculate that for you, but first, let me just say that this reaction is going to release some "hot" news! Now, back to the calculation. To determine the heat released, we need to look at the enthalpy change (ΔH) for each reaction involved.

So, in this case, the reaction is:
CH4 + O2 → CH3OH

The enthalpy change for the reaction of CH4 with O2 is -890 kJ/mol. Now, we need to convert the grams of CH4 you have to moles. The molar mass of CH4 is approximately 16 g/mol (one carbon atom and 4 hydrogen atoms), so 38.6 grams of CH4 is about 2.4125 moles.

Now, since we need to form CH3OH, we need to account for its stoichiometry as well. In this reaction, one mole of CH4 produces one mole of CH3OH.

Therefore, the total heat released when 38.6g of CH4 reacts completely would be:
ΔH = -890 kJ/mol × 2.4125 mol = -2149.625 kJ

So, approximately 2,149.625 kilojoules of heat would be released during the reaction. That's definitely a lot of heat, better be prepared for it!

To calculate the amount of heat released when CH4 reacts completely with O2 to form CH3OH, we need to use the concept of enthalpy and apply the appropriate chemical equation.

1. First, write the balanced chemical equation for the reaction:
CH4 + O2 -> CH3OH

2. Determine the molar mass of each compound involved in the reaction:
Molar mass of CH4 = 12.01 g/mol (carbon) + 1.01 g/mol (hydrogen) = 16.03 g/mol
Molar mass of CH3OH = 12.01 g/mol (carbon) + 3.03 g/mol (hydrogen) + 16.00 g/mol (oxygen) = 31.04 g/mol

3. Calculate the number of moles of CH4 using its molar mass and given mass:
moles of CH4 = mass of CH4 / molar mass of CH4
= 38.6 g / 16.03 g/mol

4. Apply stoichiometry to find the moles of CH3OH produced, by comparing the coefficients in the balanced equation:
From the balanced equation, it is clear that for every 1 mole of CH4, 1 mole of CH3OH is formed. Therefore, the moles of CH3OH produced will be equal to the moles of CH4 used in the reaction.

5. Calculate the amount of heat released using the equation:
q = n * ΔH_rxn
where q is the heat released, n is the number of moles of CH4, and ΔH_rxn is the molar enthalpy change given per mole of the reaction.

6. Look up the molar enthalpy change (ΔH_rxn) for the reaction CH4 + O2 -> CH3OH in a reliable source such as a chemistry textbook or online database. The ΔH_rxn for this specific reaction is -193.1 kJ/mol.

7. Substitute the values for n and ΔH_rxn into the equation from step 5 and calculate the heat released:
heat released = moles of CH4 * ΔH_rxn

Finally, substitute the calculated values into the equation and solve for the heat released.

23kJ