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    Enthalpy of A Reaction Using Hess' Law

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    This solution will discuss how to determine the enthalpy of a chemical reaction primarily using Hess's law. The use of the general formula for enthalpy will also be addressed. These problems will be solved using both Hess's law and the general formula for enthalpy. A step by step example and answers are included.

    © BrainMass Inc. brainmass.com December 24, 2021, 11:07 pm ad1c9bdddf
    https://brainmass.com/chemistry/hess-law/enthalpy-reaction-using-hess-law-538891

    SOLUTION This solution is FREE courtesy of BrainMass!

    Calculating Entropy using Hess's law

    Find the enthalpy of the following reactions:

    NOg + ½ o2 NO2
    Cgraphite C diamond

    5C(s) +6H2(g) C5H12

    1. There are 2 ways to solve these problems. One can solve them using Hess's law or one can solve them using the following formula:
    ∑ { (ΔH products) x (mol products)} - ∑{ ( ΔH reactants) x ( mol reactants)}

    I will solve them using hess's law and I will use the above formula to check my answers for some of the problems.

    Formation of NO2

    Add ΔH of each component reaction. Don't forget to reverse the reaction if necessary to obtain the desired product. If one reverses the reaction, one needs to assign the opposite sign to the ΔH value.

    Write the equation for the formation of NO as follows:
    ½ N2(g) + ½ o2(g) NO(g) Δ H = 90.29 kj

    We must reverse this reaction because we want a reaction in which NO is the reactant. We can do this because according to Hess's law, it does not matter which way a reaction proceeded. So we have the following equation:
    NO(g) ½ N2(g) + ½ o2 ΔH=-90.29kj

    ½ N2(g) + o2(g) NO2(g) ΔH=33.2kj

    NO(G) + ½ o2(g)* NO2 ΔH=-57.1kj

    *o2 partially cancels, If you cancel out ½ o2. That leaves you with ½ o2.

    You can check the answer using the general formula for enthalpy, as mentioned previously. If one substitutes ΔH values it is as follows:

    33.2 kj/mol - 90.29kj/mol = -57.1 kj

    Since o2 is in its ground state or natural state, it's ΔH value is 0.
    2. Cgraphite C diamond

    Cgraphite + o2 co2(g) ΔH = -394 kj
    Cdiamond + o2 co2(g) ΔH= -396 kj

    Keep the 1st equation as is but reverse the second because cdiamondhas to be a product.

    C graphite + O2 CO2 ΔH = -394 kj
    CO2 Cdiamond + O2 ΔH =+ 396kj

    Cgraphite C diamond ΔH = 2 kj

    Check with formula

    -394 kj + 396 kj = 2 kj

    3. Formation of Pentane

    5C(s) +6 H2(g) C5H12
    For this reaction one needs to use the combustion reactions of each of the reactants as follows:

    C(s) + O2(g) CO2(g) ΔH = -393.5 kj
    H2(g) + ½ O2 H2O(l) ΔH = -285.8 kj
    C5H12(g) + 8O2(g) 5CO2(g) + 6 H2O(l) ΔH=-3535.6kj

    By combining equations we can solve this as follows:

    5C(s) + 5O2(g) 5 CO2(g) ΔH=5(-393.5)kj

    6 H2 + 3O2 6H2O ΔH=6(-285.8)kj

    5CO2 +6H2O C5H12 + 8O2 ΔH=3535.6 kj

    5 C + 6H2 C5H12 ΔH=146.7 kj

    Using the general formula for enthalpy we can compute the answer as follows:

    -3535.6-[5(-393.5)+6(-285.8)]

    -3535.6-{(-1967.5 +(-1714.8)}
    -3535.6-(-3682.3)
    -3535.6+3682.3=146.7

    Modern Chemistry,Holt, Rinehart, Winston 2006 Austin TX, Raymond E. Davis et al.

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    © BrainMass Inc. brainmass.com December 24, 2021, 11:07 pm ad1c9bdddf>
    https://brainmass.com/chemistry/hess-law/enthalpy-reaction-using-hess-law-538891

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