What happened to the Hindenberg? Nobody seems to know. Was it a spark? Sabotage? Lightening? Either...
What happened to the Hindenberg? Nobody seems to know. Was it a spark? Sabotage? Lightening? Either way it did burn, a lot. We do know it was filled with hydrogen gas.
The Zeppelin was filled with 2.0 x 108 L of H2. Show all work for the below.
a) Calculate the enthalpy of the reaction(kJ/mol) below using the heat of formation for the reactants and products from appendix C from your text book.
2H2(g) + O2(g) à 2H2O(l) DHorxn= ?
b) Hydrogen gas and oxygen gas can also produce liquid hydrogen peroxide(H2O2) according to the following equation:
H2(g) + O2(g) H2O2(l) Horxn= ?
Calculate the enthalpy of the reaction(kJ/mol) below using the heat of formation for the reactants and products from appendix C from your text book.
c) Using Hess's Law and the chemical equations and enthalpies from parts a) and b), calculate the enthalpy for the decomposition of hydrogen peroxide to liquid water and oxygen gas. Show all work as to how you applied Hess's law to this problem.
d) If the 2.0 x 108 L of hydrogen gas corresponds to 8.32 x 106 mol of H2, how much heat was exchanged upon the burning of this H2 gas? Comment on the magnitude of this number.
Homework Answers
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What happened to the Hindenberg? Nobody seems to know. Was it a
spark? Sabotage? Lightening? Either...
Consider the following gas reaction at STP: H2(g) +O2(g) -->H2O2(g). Calculate the final volume if 2.0...
Consider the following gas reaction at STP: H2(g) +O2(g) -->H2O2(g). Calculate the final volume if 2.0 moles of hydrogen gas react with 2.0 moles of oxygen gas. (R=0.08206 L*atm/mol*K)
need the Hess law calculations please!!! Thanks 3% Trial 4 What is the concentration of the...
need the Hess law calculations please!!!
Thanks
3% Trial 4 What is the concentration of the stock H.O, solution? How much heat should be released when 10.0 mL of H., decompose? Your answer must be in units of kJ Trial Trial 2 Trial 3 Mass of H.Ozused (9) 0.055g 0.0589 0.052g Moles of H.O.decomposed (mol) 0.0016 0.0017 0.0015 Final Temperature (T) (°C) 38.00 138.4°C 13.1°C Initial temperature (T) ("C) 22:2°C 22.30 22.3°C Change in temperature: AT= T.-T (°C) 15.800 16.1°C...
When one mole of gaseous hydrogen peroxide, H2O2, is made from hydrogen and oxygen gases, the enthalpy change is –136 kJ...
When one mole of gaseous hydrogen peroxide, H2O2, is made from hydrogen and oxygen gases, the enthalpy change is –136 kJ. Which of the following correctly represents the thermochemical equation? i. H2(g) + O2(g) → H2O2(g) + 136 kJ ii. H2(g) + O2(g) + 136 kJ → H2O2(g) iii. H2(g) + O2(g) → H2O2(g) ΔH = –136 kJ iv. H2(g) + O2(g) → H2O2(g) ΔH = +136 kJ A.i only B.ii only C.iii only D.i and iii E.ii and iv
Hydrogen peroxide (H2O2) decomposes to produce water and oxygen according to the following reaction: 2 H2O2...
Hydrogen peroxide (H2O2) decomposes to produce water and oxygen according to the following reaction: 2 H2O2 (l) -----------> 2 H2O (l) + O2 (g) Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? Group of answer choices 2 molecules of H2O2 -----------------> 2 molecules of H2O + 1 molecule of O2 2 mol of H2O2 ----------------->2 mol of H2O + 1 mol of O2 68.0 g of H2O2 -----------------> 36.0 g of H2O...
72. Hydrogen peroxide is a very common oxidizing agent. It has been used as an oxidizer...
72. Hydrogen peroxide is a very common oxidizing agent. It has been used as an oxidizer for rocket engines, it is a readily available antiseptic for home use and we have used it several times in the general chemistry lab. Below is some thermodynamic data for hydrogen peroxide xide at 25 C H (kJ/mol AG (k.J/mol Chemical Thermodvnamics of hydrogen 188 266 H20:1) H2(g) 02(g) H:0:(1) 20H(g H2O2(g) → 20H(g) H202(g) HO:(g) +H(g) H2O2(l) H2O(l)+%O2(g) 120 188 174 332 365...
Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an...
Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2O2 can be prepared in a process whose overall change is H, O2 (1) H2(g) +O2(g) Calculate the enthalpy change using the following data: 2H2O2()2H2 O (l) + O2(g); AH = -196.0 kJ H2(g) +O2(g)H2O(); AH= -285.8 kJ ΔΗ- kJ 10 item attempts remaining Try Another Version Submit Answer
You will be using 25.00 mL of 3.00% by mass solution ({mass H2O2/mass solution}*100) of hydrogen...
You will be using 25.00 mL of 3.00% by mass solution ({mass H2O2/mass solution}*100) of hydrogen peroxide. Assume the density of this solution is 1.000 g/mL. If all of hydrogen peroxide decomposes to water and oxygen according to the reaction 2H2O2(aq) ↔2H2O(l) +O2(g) what is the total volume of oxygen gas generated if the temperature is 27° C and the pressure is 775 Torr (ignore the effects of water vapor present)? 760 Torr = 1 atm R = 0.08206 L•atm/K•mol...
Be sure to answer all parts. Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel...
Be sure to answer all parts. Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition: 2 H2O2(1) + 2 H2O(1) + O2(g) AHpxn=-196.1 kJ Calculate the heat for the decomposition of 384 kg of H2O2. x 10 kJ (Enter your answer in scientific notation.)
Be sure to answer all parts. Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel...
Be sure to answer all parts. Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition: 2 H2O2(1)→ 2H2O(1) + O2(g) AH r = -196.1 kJ Calculate the heat for the decomposition of 587 kg of H2O2. x 10 kJ (Enter your answer in scientific notation.)
Hydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and...
Hydrogen peroxide can be prepared in several ways. One method is
the reaction between hydrogen and oxygen, another method is the
reaction between water and oxygen. Calculate the ?G°rxn of each
reaction below using values from this table.
(1) H2(g) + O2(g)
H2O2(l)
G =
(2) H2O(l) + 1/2O2(g)
H2O2(l) G
=
Which method requires less energy under standard conditions?
need the Hess law calculations please!!!
Thanks
3% Trial 4 What is the concentration of the stock H.O, solution? How much heat should be released when 10.0 mL of H., decompose? Your answer must be in units of kJ Trial Trial 2 Trial 3 Mass of H.Ozused (9) 0.055g 0.0589 0.052g Moles of H.O.decomposed (mol) 0.0016 0.0017 0.0015 Final Temperature (T) (°C) 38.00 138.4°C 13.1°C Initial temperature (T) ("C) 22:2°C 22.30 22.3°C Change in temperature: AT= T.-T (°C) 15.800 16.1°C...
72. Hydrogen peroxide is a very common oxidizing agent. It has been used as an oxidizer for rocket engines, it is a readily available antiseptic for home use and we have used it several times in the general chemistry lab. Below is some thermodynamic data for hydrogen peroxide xide at 25 C H (kJ/mol AG (k.J/mol Chemical Thermodvnamics of hydrogen 188 266 H20:1) H2(g) 02(g) H:0:(1) 20H(g H2O2(g) → 20H(g) H202(g) HO:(g) +H(g) H2O2(l) H2O(l)+%O2(g) 120 188 174 332 365...
Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2O2 can be prepared in a process whose overall change is H, O2 (1) H2(g) +O2(g) Calculate the enthalpy change using the following data: 2H2O2()2H2 O (l) + O2(g); AH = -196.0 kJ H2(g) +O2(g)H2O(); AH= -285.8 kJ ΔΗ- kJ 10 item attempts remaining Try Another Version Submit Answer
Be sure to answer all parts. Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition: 2 H2O2(1) + 2 H2O(1) + O2(g) AHpxn=-196.1 kJ Calculate the heat for the decomposition of 384 kg of H2O2. x 10 kJ (Enter your answer in scientific notation.)
Be sure to answer all parts. Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition: 2 H2O2(1)→ 2H2O(1) + O2(g) AH r = -196.1 kJ Calculate the heat for the decomposition of 587 kg of H2O2. x 10 kJ (Enter your answer in scientific notation.)
Hydrogen peroxide can be prepared in several ways. One method is
the reaction between hydrogen and oxygen, another method is the
reaction between water and oxygen. Calculate the ?G°rxn of each
reaction below using values from this table.
(1) H2(g) + O2(g)
H2O2(l)
G =
(2) H2O(l) + 1/2O2(g)
H2O2(l) G
=
Which method requires less energy under standard conditions?
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