Chem

posted by .

2H2(g)+O2(g) ---> 2H2O(l)
delta H= -572kJ/mole of O2

Calculate the amount of heat evolved when 10g of hydrogen are burned in excess oxygen.

Can someone please explain step by step? =D

  • Chem -

    I worked this for you below. You didn't look or you don't understand? If you don't understand, go step by step and be specific about what you don't understand.

  • Chem -

    I looked at the solution from below but i do not understand where the 4g of H2 came from and why 572kJ x 10/4?

    Would you mind explaining please? I'm quite new to this topic.

  • Chem -

    Look at the equation.
    2H2 + O2 ==> 2H2O
    2 mols H2 react with 1 mol O2.
    That's 4 g H2 (4*1 = 4) react with 32 g O2 (2*16=32).

    So you would get 572 kJ if you had 32 g O2 or 4 g H2. Suppose you had 4 g H2. You would have
    572 x 4/4 = ?

    Suppose you had twice as much H2 (8 g H2)?
    You would obtain twice as much or 572 x 2 = ? How do you get that? It's 572 x (8/4) = ?
    If you have 10 g it's 572 x (10/4) = ?

    What about apples? If apples cost 5.72 for 4 apples, how much will 10 apples cost? That's $5.72 x (10/4) = ?

  • Chem -

    Thank you very much, I understand now (:

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Hydrogen H2, is used asa rocker fuel. The hydrogen is burned in oxygen to produce water vapor. 2H2 + O2 ----> 2H2O Delta H= -484 kJ What is the enthalpy change per gram of hydrogen.
  2. Chemistry

    Hydrogen H2 is used as a rocker fuel. The hydrogen is burned in oxygen to produce water vapor. 2H2 + O2 ----> 2H2O Delta H = -484 kJ What is the enthalpy change per gram of hydrogen?
  3. Chem

    Calculate delta H for the formation of one mole of N2O5 from the elements at 25 degrees C using the following data. 2H2 + O2 - 2H2O delta H = -571.6 kJ N2O5 + H2O - 2HNO3 deltaH = -73.7 kJ 1/2N2 + 3/2O2 + 1/2H2 - HNO3 delta H = -174.1 …
  4. Chemistry

    Consider the following reaction: CH4 +2O2 -> CO2 + 2H2O. Delta H = -891 kJ Calculate the enthalpy change for each of the following cases: a. 1.00 g methane is burned in excess oxygen b. 1.00 x 10^3 L methane gas at 740. torr and …
  5. Chemistry

    Hydrogen and methanol (CH3OH) have both been proposed as alternatives to hydrocarbon fuels. a) Write balanced chemical equations for the complete combustion of hydrogen and the complete combustion of gaseous methanol. Combustion reaction …
  6. chemistry

    1. Nitrogen gas and sodium liquid are produced by the decomposition of sodium azide NaN3 (s). what volume of nitrogen gas, measured at 25 C and 0.980 atm, is produced by the decomposition of 62.5 g of sodium azide?
  7. Chemistry

    3. A liquid hydrocarbon (Cx Hy) is found to be 16.37% H by mass. A 1.158-g vaporized sample of the hydrocarbon has a 358 mL volume at 71.0 C and 749 mmHg. what is the molecular formula for this hydrocarbon?
  8. Chem

    2H2(g)+O2(g) ---> 2H2O(l) delta H= -572kJ/mole of O2 Calculate the amount of heat evolved when 10g of hydrogen are burned in excess oxygen.
  9. chemistry

    Consider the following reaction: 2H2 (g) + O2 (g)  2H2O (l) ΔH = -572 kJ a. How much heat is evolved for the production of 1.00 mol H2O (l)?
  10. chem

    If you burn 13.7 g of methane (CH4) burns in oxygen, then 686 kJ is evolved. What is the amount of heat produced per mole of methane burned?

More Similar Questions