Question

Use the reaction enthalpies below to determine Hrxn for the following reaction: Ca(s)+2H20(l)--Ca(OH)2(s)+H2(g) Given: H2(g)+1/2O2(g)--H20(l) Hrxn=...

Use the reaction enthalpies below to determine Hrxn for the following reaction:

Ca(s)+2H20(l)--Ca(OH)2(s)+H2(g)

Given:

H2(g)+1/2O2(g)--H20(l) Hrxn= -285kJ

Ca(OH)2(s)--CaO(s)+H2O(l) Hrxn= 64kJ

2Ca(s)+O2(g)--2CaO(s) Hrxn= -1270kJ

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
Given the following data: H2(g) + 1/2O2(g) → H2O(l) ΔH° = -286.0 kJ C(s) + O2(g)...
Given the following data: H2(g) + 1/2O2(g) → H2O(l) ΔH° = -286.0 kJ C(s) + O2(g) → CO2(g) ΔH° = -394.0 kJ 2CO2(g) + H2O(l) → C2H2(g) + 5/2O2(g) ΔH° = 1300.0 kJ Calculate ΔH° for the reaction: 2C(s) + H2(g) → C2H2(g)
Use the following reaction enthalpies to determine the reaction enthalpy for 2 HCl(g) + F2(g) →...
Use the following reaction enthalpies to determine the reaction enthalpy for 2 HCl(g) + F2(g) → 2 HF(g) + Cl2(g). 4 HCl(g) + O2(g) → 2 H2O(l) + 2 Cl2(g) ΔHrxn = - 202.4 kJ/mol rxn 1/2 H2(g) + 1/2 F2(g) → HF(g) ΔHrxn = - 271.0 kJ/mol rxn H2(g) + 1/2 O2(g) → H2O(l) ΔHrxn = - 285.8 kJ/mol rxn
Given the following reactions and their enthalpies: ΔH(kJ/mol)−−−−−−−−−−− H2(g)⟶2H(g)   +436 O2(g)⟶2O(g)   +495 H2+1/2O2(g)⟶H2O(g)   −242 A. Devise...
Given the following reactions and their enthalpies: ΔH(kJ/mol)−−−−−−−−−−− H2(g)⟶2H(g)   +436 O2(g)⟶2O(g)   +495 H2+1/2O2(g)⟶H2O(g)   −242 A. Devise a way to calculate ΔH for the reaction H2O(g)⟶2H(g)+O(g) B. estimate the H-O bond energy
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s)...
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ Please explain in detail.
For the reaction:                                 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalp
For the reaction:                                 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalpy of reaction (DHrxn) from the following reactions: Reaction                                                             Δ Hrxn(kJ/mol)2 C2H2(g)+ 5 O2(g) → 4 CO2(g) + 2 H2O (l)              -2599.2 C (s) + O2(g) → CO2(g)                                            - 393.5 2 H2(g) + O2(g) → 2H2O (l)                                      -571.8 b) If the DS for the reaction is equal to 652 J/mol, and the reaction proceeds at 25°C, would you expect the reaction to be spontaneous?
Consider the balanced chemical reaction shown below. 1 Ca3P2(s) + 6 H2O(l) 3 Ca(OH)2(s) + 2...
Consider the balanced chemical reaction shown below. 1 Ca3P2(s) + 6 H2O(l) 3 Ca(OH)2(s) + 2 PH3(g) In a certain experiment, 3.981 g of Ca3P2(s) reacts with 4.412 g of H2O(l). (a) Which is the limiting reactant? (Example: type Ca3P2 for Ca3P2(s)) (b) How many grams of Ca(OH)2(s) form? (c) How many grams of PH3(g) form? (d) How many grams of the excess reactant remains after the limiting reactant is completely consumed?
Consider the reaction C6H4(OH)2 (l) + H2O2 (l) ⎯→ C6H4O2 (l) + 2 H2O (l) (a)...
Consider the reaction C6H4(OH)2 (l) + H2O2 (l) ⎯→ C6H4O2 (l) + 2 H2O (l) (a) Use the following information to calculate ΔH° for the above reaction. Show all work. ΔH° C6H4(OH)2 (l) ⎯⎯→ C6H4O2 (l) + H2 (g) +177.4 kJ H2 (g) + O2 (g) ⎯⎯→ H2O2 (l) -187.8 kJ H2 (g) + € 1 2 O2 (g) ⎯⎯→ H2O (l) -285.8 kJ (b) Based on your answer to part a, above, would heat be gained or lost by...
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)
use standard enthalpies of format to calculate Hrxn for each reaction. 1:2H2S (g) +3O2 (g)     2H2O...
use standard enthalpies of format to calculate Hrxn for each reaction. 1:2H2S (g) +3O2 (g)     2H2O (l) 2SO2 (g) 2: 3NO2 (g)+H2O (l)       2HNO3 (aq) +NO (g) 3: N2O4 (g) + 4H2 (g)      N2 (g) +4H2O (g) 4: CR2O3 (S) +3CO (g)     2CR (S)+3CO2 (g) Calculate Kc for each reaction and predict whether reactant and product s will be favor at equilibrium 1: CH3OH(g)         CO (g) + 2H2 (g) 2: 2CO2 (g)+2CF2 (g)        4COF2 (g) 3: 6COF2 (g)         3CO2(g)+3CF2 (g)...
6-56) Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. a) 2 H2S(g) +...
6-56) Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. a) 2 H2S(g) + 3 O2(g) ⇒2 H2O(l) + 2 SO2(g) b) SO2(g) + 12 O2(g) ⇒ SO3(g) c) C(s) + H2O(g) ⇒ CO(g) + H2(g) d) N2O4(g) + 4 H2(g) ⇒ N2(g) + 4 H2O(g)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT