Using the information provided calculate the heat of reaction involved in the conversion of 25.00 g of methane (CH4, MM=16.0426 g/mol) to chloroform (CHCl3, MM=119.3779 g/mol):

CH4(g) + 3 Cl2(g) --> CHCl3(l) + 3 HCl(g)

Given the following:
C(graphite) + 2 H2(g) --> CH4(g)
deltaH = -92.3 kJ

C(graphite) + 1/2 H2(g) + 3/2 Cl2(g) --> CHCl3(l)
dH = -74.5 kJ

1/2 H2(g) + 1/2 Cl2(g) --> HCl(g)
dH = -135.1 kJ

ANS:
-603.9 kJ

Much help is appreciated! Thank you!

To calculate the heat of reaction involved in the conversion of methane to chloroform, we need to sum up the heats of the individual steps involved in the reaction.

Step 1: Calculate the moles of methane (CH4) used.
Molar mass of CH4 = 16.0426 g/mol
Moles of CH4 = Mass of CH4/Molar mass of CH4 = 25.00 g/16.0426 g/mol

Step 2: Calculate the heat of Step 1.
Heat of Step 1 = Moles of CH4 * Heat of Step 1 = (25.00 g/16.0426 g/mol) * (-92.3 kJ)

Step 3: Calculate the moles of chlorine (Cl2) used.
1 mole of CH4 requires 3 moles of Cl2, so the number of moles of Cl2 = 3 * Moles of CH4 = 3 * (25.00 g/16.0426 g/mol)

Step 4: Calculate the heat of Step 3.
Heat of Step 3 = Moles of Cl2 * Heat of Step 3 = 3 * (25.00 g/16.0426 g/mol) * (-135.1 kJ)

Step 5: Calculate the heat of Step 2.
Heat of Step 2 = Heat of Step 2 * Moles of CH4 = (-74.5 kJ) * Moles of CH4 = (-74.5 kJ) * (25.00 g/16.0426 g/mol)

Step 6: Calculate the total heat of reaction.
Total heat of reaction = Heat of Step 2 + Heat of Step 3 + Heat of Step 1

When you plug in the values and calculate the total heat of reaction, you should get -603.9 kJ.

Therefore, the heat of reaction involved in the conversion of 25.00 g of methane to chloroform is -603.9 kJ.

To calculate the heat of reaction involved in the conversion of methane to chloroform, you need to apply the concept of Hess's Law. Hess's Law states that the heat change of a reaction is independent of the path taken, and only depends on the initial and final states.

Here's how you can use Hess's Law to solve this problem step by step:

1. Start by writing the balanced chemical equation for the reaction:

CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g)

2. Identify the given reactions and their corresponding heats of reaction:

Reaction 1: C(graphite) + 2 H2(g) → CH4(g)
ΔH1 = -92.3 kJ

Reaction 2: C(graphite) + 1/2 H2(g) + 3/2 Cl2(g) → CHCl3(l)
ΔH2 = -74.5 kJ

Reaction 3: 1/2 H2(g) + 1/2 Cl2(g) → HCl(g)
ΔH3 = -135.1 kJ

3. Now, since you want to calculate the heat of reaction for the conversion of 25.00 g of methane to chloroform, you need to convert the given mass of methane to moles. Use the molar mass of methane (MM = 16.0426 g/mol) to calculate the number of moles:

Number of moles of CH4 = mass of CH4 / molar mass
Number of moles of CH4 = 25.00 g / 16.0426 g/mol

4. Use the coefficients in the balanced equation to determine the number of moles of chloroform formed. Since the stoichiometric coefficient of CH4 in Reaction 2 is 1, the number of moles of CHCl3 formed will be the same as the number of moles of CH4 used.

5. Multiply the moles of CH4 (from step 3) by the ΔH2 value (from step 2) to calculate the heat of reaction for the conversion of 25.00 g of methane to chloroform:

Heat of reaction = ΔH2 × moles of CH4

6. Finally, convert the heat of reaction from step 5 to the desired units, kJ:

Heat of reaction = (Heat of reaction in J) / 1000

By following these steps and plugging in the given values, you should find that the heat of reaction involved in the conversion of 25.00 g of methane to chloroform is -603.9 kJ.