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.

  1. 👍
  2. 👎
  3. 👁
  1. I assume you have a set of tables.
    delta Hrxn = (delta Hproducts)-(delta H reactants).
    Then delta Hrxn x (2.7/molar mass C4H10).

    1. 👍
    2. 👎
  2. goobs

    1. 👍
    2. 👎
  3. kklkl

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate the standard enthalpy of reaction for the reaction 2Na + 2H2O——> 2NaOH+ H2. Standard enthalpies of formation are -285.8 kJ/mol for H2O and -470.11 kJ/mol for NaOH.

  2. chemistry

    Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. (See the appendix. Enter your answer to the tenth place.) (a) 2 H2S(g) + 3 O2(g) 2 H2O(l) + 2 SO2(g) (b) N2O4(g) + 4 H2(g) N2(g) + 4 H2O(g) (c) SO2(g) +

  3. chemistry

    The fuel used in many disposable lighters is liquid butane, C4H10. Butane has a molecular weight of 58.1 grams in one mole. How many carbon atoms are in 2.50 g of butane?

  4. Chemistry

    Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is: 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atm and 23 ∘C, what is the

  1. General chemistry

    Many portable gas heaters and grills use propane, C3H8(g). Using enthalpies of formation, calculate the quantity of heat produced when 16.0g of propane is completely combusted in air under standard conditions. Assume that liquid

  2. 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

  3. chemistry

    The standard enthalpy of combustion of C2H6O(l) is -1,367 kJ mol-1 at 298 K. What is the standard enthalpy of formation of C2H6O(l) at 298 K? Give your answer in kJ mol-1, rounded to the nearest kilojoule. Do not include units as

  4. chemistry

    calculate the heat of combustion for the following reactions from the standard enthalpies of formation 2H2(g) + O2(g) = 2H2O(l) 2C2H2(g) + 502(g) = 4CO2(g) + 2 H2O(l)

  1. biology

    Butane gas (C4H10) is burned to produce carbon dioxide and water vapour. If 12.8 mol of butane are completely burned, how many moles of water vapour are produced?

  2. CHEM

    Propane (C3H8) burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Part A Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of

  3. chemistry

    C2H4(g)+ 3O2(g) --> 2 CO2 (g) + 2H2O (l) The complete combustion of 11.22g of ethylene, C2H4 (g), via the given equation, produces 564,4 KJ of heat. Calculate the standard enthalpy of formation for C2H4(g), using the standard

  4. Chemistry

    Calculate the mass of water produced when 3.94 g of butane reacts with excess oxygen. Butane, C4H10, reacts with oxygen, O2, to form water, H2O, and carbon dioxide, CO2, as shown in the following chemical equation:

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