Butane, C4H10, is widely used as a fuel for disposable lighters. When one mole of butane is burned in oxygen, carbon dioxide and steam are formed and 2658 kJ of heat is evolved.
a) Write the thermochemical equation for the reaction.

First I wrote the chemical equation for the reaction:
2C4H10 + 13O2 --> 8CO2 + 10H2O

Since the problem gives the heat for one mole of butane, would the correct thermochemical equation be this:
C4H10 + 13/2O2 --> 4CO2 + 5H2O delta-H= -2658.3 kJ


  1. 👍
  2. 👎
  3. 👁
  1. 12

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. UCF

    What will be the change in enthalpy when 100.0 g of butane, C4H10, is burned in oxygen as shown in the thermochemical equation below? 2 C4H10(l) + 13 O2(g) → 8 CO2(g) + 10 H2O(g) ΔH = −5271 kJ −2636 kJ −4534 kJ −9087 kJ

  2. Chemistry

    The enthalpy of combustion of butane C4H10 is described by the reaction: C4H10(g) + (13/2) O2(g) -> 4CO2(g) + 5H2O(g) ΔH°rxn = –2613 kJ/mol Given the following enthalpies of formation: ΔH°f[CO2(g)] = -393.5 kJ/mol

  3. Chemistry

    When 0.340 mol of butane, C4H10, are burned with excess oxygen giving CO2 and H2O, how many moles of oxygen are consumed?

  4. chemistry

    how many moles of butane gas c4h10 react to produce 3.50moles of water?

  1. chem

    What is the mass of 0.455 L of butane gas, C4H10, at STP?

  2. College chemistry

    Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.4 C. A 250 mL sealed flask contains 0.5 g of butane at -22 C. How much butane is present as a liquid? If the butane is warmed to 25 C, how

  3. chemistry

    Many cigarette lighters contain liquid butane, C4H10(l). Using standard enthalpies of formation, calculate the quantity of heat produced when 2.7 g of butane is completely combusted in air under standard conditions.

  4. chemistry

    what volume of oxygen gas is needed to completely combust 0.202 L of butane (C4H10) gas?

  1. Chemistry

    How many grams of Butane (C4H10) must be burned to release 6375 KJ of heat? Given: Molar mass of C4H10 =

  2. AP chemistry

    Liquid butane, C4H10, is stored in cylinders, to be used as a fuel. The normal boiling point of butane is listed as -0.5 C. (a) suppose the tank is standing in the sun and reaches a temperature of 35 C. Would you expect the

  3. Chemistry

    The balanced equation for the combustion of butane, C4H10, is 2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g) Calculate the moles of CO2 produced when 2.62 moles of C4H10 are allowed to react with 13.37 moles of O2.

  4. Chemistry

    If 116g of butane burns in presence of 320g of oxygen, how much carbon dioxide will be produced? What is limiting reagent? So This is how I worked it out: 116gC4H10*1/58.12(molar mass of C4H10)*8 moles CO2/2 moles C4H10*44/1(molar

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