Homework Answers
Hi here is the solution for your question.I hope I could help you in future also. If anything is not clear to you please let me know before giving your valuable feedback I would like to elaborate that.
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Solution
Given
Enthalpy of formation of So3 = -395.7 Kj/mol
Enthalpy of formation of So2 = - 296.8 KJ /mol
Solution
We will use formula for calculating standard heat of reaction
Which is equal to
(Sum of enthalpy of products ) - (sum of enthalpy of reactants)
= (- 2 × 395.7 KJ/mol ) - ( -2 × 296.8 KJ/mol)
= - 197.8 KJ/ mol
But in option( C ) -197.8 KJ is given
So it is already given per mole .
I hope it will help. If you have any query please ask before voting
Thanks
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Calculate ΔΗ for the reaction of sulfur dioxide with oxygen. 2SO2 (g) + O2 (g)-+8νβστ2SO, (g)...
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Sulfur dioxide, So, (g), can react with oxygen to produce sulfur trioxide, SO,(g), by the reaction 2 S02(g) + 0, (g...
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Sulfur dioxide, SO, (g), can react with oxygen to produce sulfur trioxide, SO,(g), by the reaction 2 502(g) + O2(g) — 2503(g) The standard enthalpies of formation for SO, (g) and SO2(g) are AH (S02(8)] = -296.8 kJ/mol AH; [s0,() = –395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.46 L of So, (g) is converted to 4.46 L of SO2(g) according to this process at a constant pressure...
Sulfur dioxide and oxygen react to form sulfur trioxide, like
this: 2SO2(g)+O2(g)→2SO3(g)
Also, a chemist finds that at a certain temperature the
equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide
has the following composition:
Calculate the value of the equilibrium constant Kp for this
reaction. Round your answer to 2 significant digits.
compound pressure at equilibrium SO2 58.3 atm 02 84.7 atm SO3 66.3 atm
TUTOR Enthalpy Changes The reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide() proceeds as follows: 2H2S(g) + 302(g)— 2H2O(g) + 2SO2(g) When 11.2 g H2S(g) reacts with sufficient O2(g), 171 kJ is evolved. Calculate the value of AH for the chemical equation given -454.4 X kJ/mol Resubmit Show Approach Hide Tutor Steps
Consider the reaction of NO(g) from its elements. 2 502(g) + O2(g) → 2 SO3(9) Use the thermodynamic data given to determine the following for this reaction: AH°, equal O kJ/mol Asº, equals O J/molk Calculate the AG, at 500 °c with all gases at standard pressure and equilibrium constant K at 500 °C. AG, at 500 °c equals O kJ/mol K at 500 equals tance (kJ/mol) (J/mol-K) O2(g) 205.2 SO2(g) -296.8 248.2 SO3(9) -395.7 240.0 AHO so
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