Question

Use Hess's Law to calculate the enthalpy change for the reaction: GdO3 + 3H2(g) -> Gd(s)...

Use Hess's Law to calculate the enthalpy change for the reaction:

GdO3 + 3H2(g) -> Gd(s) + H2O (g)

from the following data:

2Gd(s) + 3O2 --> 2GdO3(s)   ^H=-685.4kJ

2H2 (g) + O2 (g) --> 2H2O(g)     ^H= -47.8kJ

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Use Hess's Law to calculate the enthalpy change for recovering tungsten from its oxide using the...
Use Hess's Law to calculate the enthalpy change for recovering tungsten from its oxide using the reaction:WO3(s) + 3H2(g) --> W(s)+3H2O(g) from the following data : 2W(s)+ 3O2(g)-->2WO3(s) , change in H = -1685.4 kJ 2H2(g)+O2(g)---> 2H2O(g) , change in H = -477.84 kJ
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction...
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction is the conversion of methane to ethylene: 2CH4(g)⟶C2H4(g)+2H2(g) Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l ΔH∘=−3120.8kJ
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction...
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction is the conversion of methane to ethylene: 2CH4(g)⟶C2H4(g)+2H2(g) Part A Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l) ΔH∘=−3120.8kJ Express your answer to four significant figures and include the appropriate units.
Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn, for the reaction in bold...
Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn, for the reaction in bold below given the following chemical steps and their respective enthalpy changes. Show ALL work! 2 C(s) + H2(g) → C2H2(g) ΔH°rxn = ? 1. C2H2(g) + 5/2 O2(g) → 2CO2 (g) + H2O (l) ΔH°rxn = -1299.6 kJ 2. C(s) + O2(g) → CO2 (g) ΔH°rxn = -393.5 kJ 3. H2(g) + ½ O2(g) → H2O (l) ΔH°rxn = -285.8 kJ
Applying Hess’s Law, from the enthalpies of reactions, N2(g) + 3H2(g) → 2 NH3(g) ΔH =...
Applying Hess’s Law, from the enthalpies of reactions, N2(g) + 3H2(g) → 2 NH3(g) ΔH = − 91.8 kJ O2(g) + 2H2(g) → 2H2O (g) ΔH = − 483.7 kJ N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: 4NH3(g) + 5O2(g) → 4 NO (g) + 6H2O(g)
Hess's Law Given the following data: 2C(s) + 2H2(g) + O2(g) → CH3OCHO(l) ΔH°=-366.0 kJ CH3OH(l)...
Hess's Law Given the following data: 2C(s) + 2H2(g) + O2(g) → CH3OCHO(l) ΔH°=-366.0 kJ CH3OH(l) + O2(g) → HCOOH(l) + H2O(l) ΔH°=-473.0 kJ C(s) + 2H2(g) + 1/2O2(g) → CH3OH(l) ΔH°=-238.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction: HCOOH(l) + CH3OH(l) → CH3OCHO(l) + H2O(l)
Using the information below determine the change in enthalpy for the following reaction:             2NO(g) +...
Using the information below determine the change in enthalpy for the following reaction:             2NO(g) + 5 H2(g) → 2NH3(g) + 2H2O(l) H2(g) + ½ O2(g) →   H2O(l)                     ∆H°= -285.8kJ N2(g) + O2(g)   → 2NO(g)                     ∆H°= +180.5 kJ 2NH3(g) → N2(g) + 3H2(g)                    ∆H°= + 92.22 kJ please explain step by step! thanks!
Hess's law states that "the heat released or absorbed in a chemical process is the same...
Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." It is important to recall the following rules: When two reactions are added, their enthalpy values are added. When a reaction is reversed, the sign of its enthalpy value changes. When the coefficients of a reaction are multiplied by a factor, the enthalpy value is multiplied by that same factor. Part A Calculate...
Using the Information below determine the change in enthalpy for the following reaction: 2NO (g) +...
Using the Information below determine the change in enthalpy for the following reaction: 2NO (g) + 5H2 (g)!2NH3 (g) + 2H2O (l) H2 (g) + 1⁄2O2 (g)!H2O (l) ΔH° = -285.8 kJ N2 (g) + O2 (g)!2NO (l) ΔH° = +180.5 kJ 2NH3 (g)!N2 (g) + 3H2 (g)ΔH° = +92.22 kJ a)-197.52 kJ b)-241.7 kJ c)-483.3 kJ d)-659.88 kJ e)-844.3 kJ please show me which equation is first second and thrid and reason why? i may be taking the wrong...
Consider the reaction: 2H2O(l)2H2(g) + O2(g) Using standard thermodynamic data at 298K, calculate the entropy change...
Consider the reaction: 2H2O(l)2H2(g) + O2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.88 moles of H2O(l) react at standard conditions. S°surroundings = J/K
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT