The heat of reaction (in kcal) is minus: BaCl2(aq) + H2SO4(aq) ⟶ BaSO4(s) + 2HCl(aq) is__________.
Question
The heat of reaction (in kcal) is minus:
BaCl2(aq) + H2SO4(aq) ⟶ BaSO4(s) + 2HCl(aq)
is__________.
Solution
To find the heat of reaction for the given chemical equation, we can use calorimetry or standard enthalpy changes if provided. However, since the specific value is not given in your question, I can guide you through the steps you would typically follow to determine it.
1. Break Down the Problem
You are provided with a reaction: We need to determine the heat of reaction, .
2. Relevant Concepts
The heat of reaction can typically be determined using standard enthalpy values of the reactants and products: If the standard enthalpy of formation values () are known for each compound, we can apply this formula.
3. Analysis and Detail
-
Identify the standard enthalpy of formation for each reactant and product:
-
Substitute these values into the equation for .
Assuming the following values (for example purposes, you would need to check reference data for accurate values):
- = -100.0 kcal/mol
- = -200.0 kcal/mol
- = -250.0 kcal/mol
- = -30.0 kcal/mol
Now calculate: Finally, applying these to the enthalpy equation:
4. Verify and Summarize
- Make sure each value used from the reference is accurate.
- Confirm that the signs of enthalpy values are consistent with formation definitions.
Final Answer
The heat of reaction is approximately .
Please verify with actual standard enthalpy data as this is a general guide using assumed values.
Similar Questions
The ΔfH∘ of BaSO4(s), Ba2+(aq) and SO42−(aq) are −350.6, −128.3 and −216.3kcal . The heat of reaction (in kcal) is minus:
Which would not have a heat of formation of 0 kJ/mol? Group of answer choicesF2(g)H2(g)S2(g)Kr(g)
b. If we assume that the specific heat of the solution is 1.0 cal/g · °C, calculate the ΔHsol for this compound in kcal/g and in kcal/mol. Show your work.
Which of the following salt(s) when heated give(s) oxygen?KMnO4Ag2OPb(NO3)2FeSO4
At 298 K, H0 = -314 kJ/mol and S0 = -0.372 kJ/(K•mol). What is the Gibbs free energy of the reaction?A.-425 kJB.0.393 kJC.34,900 kJD.-203 kJ
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.