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.
Which statement describes how you can determine ∆Hrxn for the reaction of H2(g) and O2(g) to...
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...
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?
Determine Heat of reaction (Hrxn) for: 2 C (s, graphite) + 3 H2 (g) ------> C2H6 (g) from the following C (s, graphite) + O2 (g) ------> CO2 (g) delta H = -393.5 kJ H2 (g) + 1/2 O2 (g) ------> H2O (l) delta H = -285.8 kJ 2 C2H6 (g) + 7 O2 (g) ------> 6 H2O (l) + 4 CO2 (g) delta H = -3,119.6 kJ
6. Given H2(g) + 22 O2(g) → H2O(1), AH° = -286 kJ/mol, Determine the standard enthalpy change for the reaction 2H2O(l) → 2H2(g) + O2(g) (2 pt)
2. Use Hess’s Law to determine the enthalpy of the reaction below. 2F2(g) + 2H2O(l) → 4HF(aq) + O2(g) DH˚= ? H2(g) + F2(g) → 2HF(aq) DH˚ = -546.6 kJ 2H2 (g) + O2(g) → 2H2O(l) DH˚ = -571.6 kJ a. 42 kJ b. -1120 kJ c. -251 kJ d. -521 kJ e. -1690 kJ
From the following balanced equation, 2H2(g)+O2(g)⟶2H2O(g) how many molecules of H2O can be formed from 5.58mol H2?
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!!!
11 If 50.0 g of H2 and 130.0 g of O2 react, how many moles of H2O can be produced in the reaction below? 2 H2(g) + O2(g) → 2 H2O(g) Attempts remaining: 2 12 If 41.1 g of NO and 26.9 g of Oz react together, how many grams of NO2 can be formed via the reaction below? 2 NO (g) + O2(g) → 2 NO2 (g) Attempts remaining: 2 13 - You have 2.2 mol Xe and 1.9...
consider the following reaction 2H2(g)+O2(g)--> 2H2O (I) delta H= -572KJ A) how much heat is evolved when 1.00 mole of H2O (I) is produced? B) how much heat is evolved when 4.03g H2 are reacted with 40.0g of O2? C) the total volume of hydrogen gas needed to fill the Hindenburg was 2.0*10^8 L at 1.0 atm and 25 degree C. How much HEAT was evolved when the Hidenburg exploded, assuming all of the hydrogen reacted (plenty of oxygen)?
The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ: 2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ A) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol of O2 at atmospheric pressure if the volume change is -3.8 L ? B) What is the value of ΔE in kilojoules.