chemistry

The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn.

For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar.

Sn(s) + 2Cl2(g) --> SnCl4(l)
ΔH°rxn = -511.3 kJ/mol
ΔU°rxn = -506.3

H2(g) + Cl2(g) --> 2HCl(g)
ΔH°rxn = -184.6 kJ/mol
ΔU°rxn = ?

I know ΔU°rxn = q + work
q = ΔH°rxn

How do I find work for the second reaction?

  1. 👍
  2. 👎
  3. 👁
  1. Since the number of moles of the reactants is 1+1 and the number of moles of the product is 2, they are equal which means that the change in the number of moles is zero. This means that ΔU°rxn is going to be equal to ΔH°rxn. ΔU°rxn= -184.6

    1. 👍
    2. 👎
  2. Avery is correct

    1. 👍
    2. 👎
  3. The standard internal energy change for a reaction can be symbolized as Δ𝑈∘rxn or Δ𝐸∘rxn . For each reaction equation, calculate the energy change of the reaction at 21 ∘C and 1.00 bar .
    2H2(g)+O2(g)⟶2H2O(l)Δ𝐻∘rxn=−561.2 kJ/mol

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) standard enthalpy: -133.5 Find the change in internal energy for this reaction. Enter in kJ.

  2. Chemistry

    For the reaction described by the chemical equation: 3C2H2(g) -> C6H6(l) .. Delta H rxn = -633.1 kJ/mol a) Calculate the value of Delta S rxn at 25.0 C... b) Calculate Delta G rxn... c) In which direction is the reaction, as

  3. chemistry

    Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 NO(g) + O2(g) → 2 NO2(g), ΔH°rxn = ? Given: N2(g) + O2(g) → 2 NO(g), ΔH°rxn = +183 kJ 1/2 N2(g) + O2(g) → NO2(g),

  4. CHEMISTRY

    Given the following heats of combustion. CH3OH(l) + 3/2 O2(g) -> CO2(g) + 2 H2O(l) ΔH°rxn = -726.4 kJ C(graphite) + O2(g) ->CO2(g) ΔH°rxn = -393.5 kJ H2(g) + 1/2 O2(g) -> H2O(l) ΔH°rxn = -285.8 kJ Calculate the enthalpy of

  1. Chemistry- please help ASAP!!!! thank you

    S(rhombic)+O2(g)--->SO2(g) change in H(rxn)= -296.06 kJ/mol S(monoclinic)+O2(g)--->SO2(g) change in H(rxn)= -296.36 kJ/mol 1. Calculate the enthalpy change for the transformation. S(rhombic)-->S(monoclinic) Our goal is to

  2. Chemistry

    CaO(s) + 3C(s) > CaC2(s) + CO(g) deltaHrxn = +464.8 kJ/mol-rxn Is the reaction endothermic or exothermic? What is the enthalpy change if 10.0 g of CaO is allowed to react with an excess of carbon?

  3. Chemistry

    You wish to know the enthalpy change for the formation of liquid PCl3 from the elements shown below. P4(s) + 6 Cl2(g)--> 4 PCl3(l) ΔH°f = ? The enthalpy change for the formation of PCl5 from the elements can be determined

  4. Chem

    RXN #1: H2 (g) + O2 (g) --> H2O2 (l) ; delta-H =? Calculate the enthalpy change (delta-H1) for the reaction above (RXN #1) using the information below and Hess' Law. RXN A: H2O2 (l) --> H2O (l) + 1/2 O2 (g); delta-H=-98.0 kJ/mol

  1. Chemistry

    Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –44.2 kJ·mol–1. C2H4(G)+H20 ---> C5H5OH ΔS°rxn= ______

  2. CHEMISTRY..

    1. Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined? If so, write the net ionic equation for the reaction. 2. Will a precipitate form if solutions of potassium nitrate and magnesium sulfate

  3. Chemistry

    Given the thermochemical equation 2SO2 + O2 → 2SO3, ΔH°rxn = -198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO3?

  4. chemistry

    How much energy is required to decompose 765 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g) → P4(s) + 6 Cl2(g), ΔH°rxn = +1207 kJ

You can view more similar questions or ask a new question.