ZuoTi.Pro
Question

7.    (20 pts)      The production of sulfuric acid, a component of acid rain occurs according to...

7.    (20 pts)      The production of sulfuric acid, a component of acid rain occurs according to

                        SO3(g) + H2O(l) →   H2SO4(aq); ∆r HƟ = -227.72 kJ/mol

                        a) Using the thermodynamic data given below state whether this reaction is spontaneous at

                            25 oC. Explain your answer.

                        Substance          ∆f GƟ (kJ/mol)     

                        H2SO4(aq)               -744.53

                        H2O(l)                     -237.13

                        SO3(g)                    -371.06

                         b) Calculate the equilibrium constant at 25 oC.

                        c) Assuming the enthalpy change is independent of temperature calculate the equilibrium constant at 500 oC.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
7.    (20 pts)      The production of sulfuric acid, a component of acid rain occurs according to...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • please help! Answer: 7. Sulfuric acid is produced through the reaction of sulfur trioxide with water....

    please help! Answer: 7. Sulfuric acid is produced through the reaction of sulfur trioxide with water. SO3(g) + H200 = H2SO4(aq) a. At standard state, the forward reaction is (10 pts) Spontaneous at all temperatures. ii. Not spontaneous at any temperature. iii. Spontaneous at temperatures greater than iv. Spontaneous at temperatures less than (calculate the value) (calculate the value). Book Pro b. 0.801 g sulfur trioxide is added to 1.00 L of water at 298 K. Calculate the equilibrium concentration...

  • When a 3.13-g sample of liquid sulfuric acid dissolves in 33.6 g of water in a...

    When a 3.13-g sample of liquid sulfuric acid dissolves in 33.6 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 22.00 oC to 41.81 oC. Calculate H in kJ/mol H2SO4 for the solution process. H2SO4(l) 2 H+(aq) + SO42-(aq) The specific heat of water is 4.18 J/g-K. Hsolution =____ kJ/mol H2SO4.

  • 7. Sulfuric acid is produced through the reaction of sulfur trioxide with water. S03(g) + H20(1)...

    7. Sulfuric acid is produced through the reaction of sulfur trioxide with water. S03(g) + H20(1) = H2SO4(aq) a. At standard state, the forward reaction is (10 pts) i. ii. Spontaneous at all temperatures. Not spontaneous at any temperature. Spontaneous at temperatures greater than Spontaneous at temperatures less than iii. (calculate the value). (calculate the value) iv. b. 0.801 g sulfur trioxide is added to 1.00 L of water at 298 K. Calculate the equilibrium concentration of each substance in...

  • 9. Nitrogen dioxide (NO2) can react with water to form aqueous nitric acid according to the...

    9. Nitrogen dioxide (NO2) can react with water to form aqueous nitric acid according to the following reaction. This is one way that acid rain forms in the atmosphere. Also listed are the standard free energies of formation for the species involved in the reaction. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) Compound AG, (kJ/mol) NO2(g) 51.3 H2O(0) -237.1 HNO3(aq) -110.9 NO(g) 87.6 a. Calculate AGºrx (6 points) b. Is the reaction spontaneous at standard conditions? Circle one and explain...

  • Shown here are the four steps that show how sulfur in coal is converted to sulfuric...

    Shown here are the four steps that show how sulfur in coal is converted to sulfuric acid in acid rain. Which step, if any, shows an unbalanced equation? Multiple Choice S(s) + O2(g) → SO2(g) SO2(g) + OH(g) → HOSO2(g) HOSO2(g) + O2 → HO2(g) + SO3(g) SO3(g) + H2O(l) → H2SO4(aq) None of the above are unbalanced equations

  • 25.0 mL of 1.3 mol/L sulfuric acid is reacted with 35.0 mL of 0.67 mol/L sodium...

    25.0 mL of 1.3 mol/L sulfuric acid is reacted with 35.0 mL of 0.67 mol/L sodium hydroxide. The solution warms from 20.0°C to 28.6°C. H2SO4 (aq) + 2NaOH (aq) => Na2SO4 (aq) + 2H20 (aq) What is the enthalpy change of the reaction (in kJ/mol)?

  • < Question 4 of 9 > A 0.196 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H2SO...

    < Question 4 of 9 > A 0.196 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H2SO4 (aq) → MSO4 (aq) + H2(g) A volume of 205 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. Calculate the molar mass of the metal. molar mass: g/mol

  • Given the thermodynamic data below, determine the equilibrium constant for the following two reactions at 25...

    Given the thermodynamic data below, determine the equilibrium constant for the following two reactions at 25 oC. Predict what will happen to ΔG, how the direction of the reaction will shift, and how the spontaneity will be affected when more BaSO4(s) is added to reaction a), and more NH4+(aq) is added to reaction b). Substance ∆Gof(kJ/mol) Substance ∆Gof(kJ/mol) Substance ∆Gof kJ/mol) BaSO4(s) –1353.1 SO42–(aq) –741.99 NH3(aq) –26.5 Ba2+(aq) –560.66 OH–(aq) –157.30 H2O(l) –237.2 NH4+(aq) –79.5 a. BaSO4(s) ⇌ Ba2+(aq) +...

  • plesae ASAP The contact process for producing sulfuric acid is: Sg(s) + 8 O2(g) — 2...

    plesae ASAP The contact process for producing sulfuric acid is: Sg(s) + 8 O2(g) — 2 SO2(g) + O2(g) SO3(g) + H2O(l) 8 SO2(g) +2 SO3(g) H2SO4(aq) each step has a percent yield of 77.1%, how many grams of Sg are needed to produce 1.50 kg sulfuric acid? 637 g 1.07*10^3 g 378 9 2.25*10^3 g 0 212 g

  • A) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g)...

    a) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g): 2. 2SO2(g) O2(g)SO3(g) dGo, ΔΗο, and ASo values for the reaction are-141 .6kJ/mol,-1984kJ/mol and -187.9J/Kmol, respectively. Evaluate whether or not the reaction is spontaneous under standard conditions at 298K, predict the effect of increasing temperature on spontaneity and calculate the value of T at which the reaction becomes nonspontaneous. b) The reaction described in part (a) is too slow at room temperature to...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT