Posted by blahblah on Saturday, April 18, 2009 at 3:06pm.
assistance needed
Please type your subject in the School Subject box. Any other words are likely to delay responses from a teacher who knows that subject well.
Calculate the heat of formation of water from its constituent elements from the following information:
3 H2 (g) + O3 (g) → 3H2O ∆H = ?
2 H2 (g) + O2 (g) → 2H2O ∆H = - 483.6
3 O2 (g) → 2O3 (g) ∆H = 284.5
You are given 2.0 grams of zinc and 2.5 grams of silver nitrate and are told they react in the following manner: Zn¬(s) + 2AgNO3(aq) → 2Ag(s) + Zn(NO3)2 (aq). How many grams of silver are produced?
#1 makes no sense. You have the heat of formation from the constituent elements listed in your question and the question marks by a reaction that is not the formation of water from its constituent elements.
#2.
Write the equation.
Convert 2 g Zn to moles.
Convert 2.5 g AgNO3 to mols.
Using the coefficients in the balanced equation, convert each of the moles into moles of any one (I suggest Ag) of the products.
The smaller number of moles of product formed from either of the reactants will be the limiting reagent; therefore, that will be the number of grams Ag produced. Post your work if you get stuck.
2.0g Zn= 0.0305mol 2.5gAgNO3 =0.0147mol
I am stuck after this. I cannot come to the correct answer.
Related Questions
chemistry - Calculate the heat of formation of water from its constituent ...
chemistry - Calculate the heat of formation of water from its constituent ...
chemistry - Calculate the standared enthalpy of formation of solid Mg(OH)2 given...
Chemistry - Given the following thermodynamic data, 2H2O(g) → O2(g) + ...
Chemistry - use the table below to calculate ΔHo reaction: Standard ...
Chemistry - ∆H⁰rxn, for the reaction of Ca(s) + 2H+(aq) -&...
chem - Determine whether the following are endothermic or exothermic. 2H2O2 (l...
Chemistry - Hydrogen cyanide is a highly poisonous, volatile liquid. It can be ...
chemistry - Hydrogen cyanide is a highly poisonous, volatile liquid. It can be ...
Chemistry - Using the bond entalpies ∆H: C---C: 348kJ C=C: 612 kJ C&#...
For Further Reading
