1. Calculate the standard enthalpy change for the reaction:
C2H4(g) + H2(g) → C2H6(g)
given that the enthalpy of combustion for the reactants and products are:
ΔHºc(C2H4)(g) = -1411 kJ mol^-1
ΔHºc(C2H6)(g) = -1560 kJ mol^-1
ΔHºc(H2)(g) = -286 kJ mol^-1

  1. 👍 1
  2. 👎 3
  3. 👁 4,359
  1. See your post above.

    1. 👍 0
    2. 👎 2
  2. 137

    1. 👍 0
    2. 👎 2

Respond to this Question

First Name

Your Response

Similar Questions

  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

    Consider the reaction, C2H4 (g) + H2 (g)- C2H6 (g) where -137kJ of heat is released. How many kilojoules are released when 55.3g of C2H4 reacts?

  3. Chem

    For the reaction, 3C2H2(g) ===> C6H6 at 25°C, the standard enthalpy change is -631 kJ and the standard entropy change is -430 J/K, Calculate the standard free energy change (in kJ) at 25°C. What is the formula that relates

  4. AP Chemistry

    C2H2(g) + 2H2(g) --> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following table: C2H2(g) 226.7 kj/mol C2H6(g) -84.7 kj/mol [the values are the change in enthalpy] a.

  1. Chemistry

    Calculate the entropy change in the surroundings when 1.00 mol N2O4(g) is formed from 2.00 mol NO2(g) under standard conditions at 298 K. I get +192 J/K. The book says -192 J/K. Here is my work, where am I going wrong? Standard

  2. chemistry

    NH4NO3(s) NH4+(aq) + NO3−(aq) In order to measure the enthalpy change for this reaction above, 1.07 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8°C and the final

  3. chemistry

    Consider the reaction, C2H4(g) + H2(g) ® C2H6(g), where DH = – 137 kJ. How many kilojoules are released when 55.3 g of C2H4 reacts?

  4. Chemistry

    Calculate the enthalpy change for: C2H4(g) + H2 --> C2H6(g) delta Hrxn: H2(g) + 1/2O2 --> H2O (l) C2H4(g) + 3O2 --> 2H20(l) + 2CO2(g) C2H6(g) + 7/2O2(g) --> 3H20(l) + 2CO2(g) I know I have to flip the third reaction but I don't

  1. chemistry

    A scientist measures the standard enthalpy change for the following reaction to be -2923.0 kJ : 2C2H6(g) + 7 O2(g) 4CO2(g) + 6 H2O(g) Based on this value and the standard enthalpies of formation for the other substances, the

  2. Chemistry

    O3 + NO --> O2 + NO2 (all in gas state) Calculate the change in enthalpy for the reaction at room temp. using the following data ^Hf: O3 = 143 NO = 90 NO2 = 33 So, I have 143+90--> X + 33. I don't know what the enthalpy of O2 is.

  3. chemistry

    The enthalpy change for the following reaction is -483.6 kJ: 2H2(g) + O2(g) = 2H2O(g) Therefore, the enthalpy change for the following reaction is _______ kJ: 4H2(g) + 2O2(g) = 4H2O(g)

  4. chemistry

    If you need to multiply the following reaction by 2 to be an intermediate reaction in a Hess's law problem, what would be the final value for the enthalpy of reaction you use for this intermediate reaction? C2H4 + 3 O2 2 CO2 + 2

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