Use bond energies to calculate ?Hrxn for the reaction.
2H2(g)+O2(g)?2H2O(g)
Note: The answer is NOT 442 kJ or 442kJ/mol
It gave me this hint when I got the answer wrong: The bond energies of H?H, O=O, and H?O are provided in the introduction. To determine the enthalpy of this reaction, sum all of the bond energies for the reactants (accounting for stoichiometric ratios as is), and subtract the bond energies for the product. Note how many bonds are in each molecule.
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Use bond energies to calculate ?Hrxn for the
reaction.
2H2(g)+O2(g)?2H2O(g)
Note: The answer is NOT 442...
Consider the reaction 2H2(g) + O2(g) → 2H2O(g). The following bond energies have been determined experimentally:...
Consider the reaction 2H2(g) + O2(g) → 2H2O(g). The following bond energies have been determined experimentally: H-H 436 kJ/mol O=O 497 kJ/mol H-O 464 kJ/mol Suppose we start with 4 mol of hydrogen and end up with 4 mol of H2O. If the system was at 300 K before the reaction took place, what is the final temperature after the reaction?
Consider the reaction 2H2(g) + O2(g) → 2H2O(g). The following bond energies have been determined experimentally:...
Consider the reaction 2H2(g) + O2(g) → 2H2O(g). The following bond energies have been determined experimentally: H-H 436 kJ/mol O=O 497 kJ/mol H-O 464 kJ/mol . Suppose we start with 4 mol of hydrogen. How many moles of oxygen are needed to "use up" all of the hydrogen? How many moles of water molecules are produced? n of O2 = 2 (Correct) n of H2O = 4 (Correct) B. For the number of moles in part A, what is the...
Hydrogen is burned according to the following chemical reaction: 2H2(g) + O2(g) → 2H2O(l) ∆Hrxn =...
Hydrogen is burned according to the following chemical reaction: 2H2(g) + O2(g) → 2H2O(l) ∆Hrxn = -286 kJ Given 100 g of H2 and excess O2, how much heat is released?
Estimate the enthalpy of the reaction below using these average bond energies 2 H-O-H ---> O=O...
Estimate the enthalpy of the reaction below using these average bond energies 2 H-O-H ---> O=O + 2 H-H O-H: 464 kJ/mol O=O: 498 kJ/mol H-H: 436 kJ/mol a. -6 kJ/mol b. -470 kJ/mol c. -442 kJ/mol d. 486 kJ/mol
Which statement describes how you can determine ∆Hrxn for the reaction of H2(g) and O2(g) to...
Which statement describes how you can determine ∆Hrxn for the reaction of H2(g) and O2(g) to form liquid water, H2O(l)? Be sure to take into consideration the intermolecular attractions in H2O(l). 2H2(g) + O2(g) → 2H2O(l) A. You can only use bond energies. B. You can only use heats of formation. C. You can use either bond energies or heats of formation.
is this endo or exo? Use the following bond energies to decide if the reaction of...
is this endo or exo?
Use the following bond energies to decide if the reaction of CO2 +2H2 --> CH4 + O2 is endo or exo thermic. C--H 414 kJ/mol S C=O in CO2 = 799 kJ/mol 0=0 = 298 H-H = 436 Endothermic Exothermic
Calculate the standard entropy change for the reaction 2H2(g)+O2(g)?2H2O(l) using the data from the following table:...
Calculate the standard entropy change for the reaction 2H2(g)+O2(g)?2H2O(l) using the data from the following table: Substance ?H?f (kJ/mol) ?G?f (kJ/mol) S? [J/(K?mol)] H2(g) 0.00 0.00 130.6 O2(g) 0.00 0.00 205.0 H2O(l) -285.8 -237.2 69.90 Express your answer to four significant figures and include the appropriate units. Please show me the steps on how to solve this!!! Thank you!!!
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies:...
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies: F2= 159 kJ/mol; O2 (double bond) = 498 kJ/mol Calculate the bond strength of the O-F bonds in OF2.
Calculate delta Hrxn for the following reaction: 5C(s)+6H2(g)--->C5H12(l) use the following reactions and given d...
Calculate delta Hrxn for the following reaction: 5C(s)+6H2(g)--->C5H12(l) use the following reactions and given delta H's: C5H12(l)+8O2(g)---> 5CO2(g)+6H2O(g) delta H= -3505.8 kJ C(s)+O2(g)--->CO2(g) delta H= -393.5 kJ 2H2(g)+O2(g)---> 2H2O(g) delta H= -483.5 kJ The steps to solving this problem would be greatly appreciated! Thanks so much!
the enthalpy change in a chemical reaction can be determined using bond energies. energy must be...
the enthalpy change in a chemical reaction can be determined using bond energies. energy must be added or absorbed to break bonds and that energy is released when bonds are formed. therefore ,you can calculate the total enthalpy of the reaction using following formula: dH= bonds broken-bonds formed Using bond energies, calculate the change in energy that accompanies the following reaction: H2 + O2 -> 2H2O Bond Bond Energy H-H 432 kJ/mol O-O 498 kJ/mol H-O 467 kJ/mol
is this endo or exo?
Use the following bond energies to decide if the reaction of CO2 +2H2 --> CH4 + O2 is endo or exo thermic. C--H 414 kJ/mol S C=O in CO2 = 799 kJ/mol 0=0 = 298 H-H = 436 Endothermic Exothermic
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