How much heat is released when a mixture containing 10.0g CS2 and 10.0 g Cl2 reacts by the equation.
CS2 + 3Cl2 ----> S2Cl2 + CCl4
Delta H = -230 kJ
Determine which is the limiting reagent using simple stoichiometry.
I assume that is -230 kJ/MOLE CS2.
Then use proportions to determine delta H.
what do you mean by proportions???
After you find the limiting reagent, (let's assume it is Cl2 but you will need to do the arithmetic to determine if it is), use that number to determine the mols CS2 that reacts, then a proportion is as follows:
(1 mol CS2/-230 kJ) = (??mols CS2/xx kJ.
The ??mols CS2 is from your first calculation, and that leaves only the 1 unknown (xx kJ).
Of course you may use dimensional analysis for the same thing.
-230 kJ * (xx mols CS2/1 mol CS2) = ??
To determine the amount of heat released when a reaction occurs, we need to use the balanced equation and the given molar enthalpy change (ΔH) value.
First, we'll find the moles of CS2 and Cl2 in the given mixture.
The molar mass of CS2 (carbon disulfide) is 76.14 g/mol, and that of Cl2 (chlorine gas) is 70.90 g/mol.
Moles of CS2 = Mass of CS2 / Molar mass of CS2
Moles of CS2 = 10.0 g / 76.14 g/mol
Moles of Cl2 = Mass of Cl2 / Molar mass of Cl2
Moles of Cl2 = 10.0 g / 70.90 g/mol
Next, we review the stoichiometric coefficients of the balanced equation to determine the ratio in which CS2 and Cl2 react.
From the equation:
1 mole of CS2 reacts with 3 moles of Cl2 to produce 1 mole of S2Cl2 and 1 mole of CCl4.
Now, we'll calculate the limiting reactant, which is the reactant that limits the amount of product formed.
Let's compare the moles of CS2 and Cl2 to see which one is the limiting reactant.
The mole ratio between CS2 and Cl2 is 1:3. So, if the ratio is higher than 1/3, CS2 is the limiting reactant. Otherwise, Cl2 is the limiting reactant.
Ratio = Moles of CS2 / Moles of Cl2
Ratio = (10.0 g / 76.14 g/mol) / (10.0 g / 70.90 g/mol)
If the ratio is larger than 1/3, CS2 is the limiting reactant. If it is smaller, Cl2 is the limiting reactant.
Next, we calculate the moles of each product formed based on the limiting reactant.
Since 1 mole of CS2 reacts to form 1 mole of S2Cl2, and 1 mole of CS2 reacts to form 1 mole of CCl4, the moles of S2Cl2 and CCl4 formed are equal to the moles of CS2.
Now, we can calculate the amount of heat released using the molar enthalpy change (ΔH) value.
Heat released = (Moles of CS2) × (ΔH)
Heat released = (Moles of CS2) × (-230 kJ)
Remember to convert the moles of CS2 into grams if necessary.
Finally, calculate the actual amount of heat released in kilojoules (kJ).
I hope this explanation helps you calculate the amount of heat released in this reaction based on the given information!