owLV2 | Online teachin × + O sic.cengagenow com irn takeAssignment takecovalentA

Question

owLV2 | Online teachin × + O sic.cengagenow com irn takeAssignment takecovalentActivity.do?locator=assignment nmentSessionLocator= assignment-take Chapter 10: Mastery 1 pts M 1 pts M 1 pts 2req 1 pts 2req 1 pts 2req 1. Compare Absolute Entropies Use the References to access important values if needed for this question. 2. Predict the Sign of AS For the reaction 2NH3(g) + 2O2(g)-N20(g) 3H20(1) Ho =-683.1 kJ and So-365.6 JK The standard free energy change for the reaction of 2.11 moles of NH3(g) at 324 K., 1 atm would be This reaction is (reactant, product) Assume that H° and are independent of temperature 4. Standard Entropy of Reaction kJ Question Question Question favored under standard conditions at 324 K. 6 G: Predict Signs 1 pts 2req 7-d& Enthalpy. Entropy and Temper.. 1 pts 8AG: Calculate Temperature Limit pts 2req 9. Thermodynamics of Refining Met pts 2req 10. AG from Free Energies of Form. 1pts 2req Submit Answe Retry Entire Group 9 more group attempts remaining

Explanation / Answer

deltaH = -683.1 KJ/mol

deltaS = -365.6 J/mol.K

= -0.3656 KJ/mol.K

T = 324 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = -683.1 - 324.0 * -0.3656

deltaG = -564.6456 KJ

As per reaction, this is when 2 moles of NH3 react

So,

for 2.11 moles,

delta G = 2.11* -564.6456 KJ / 2

= -595.7 KJ

Answer: -595.7 KJ

negative sign shows it is product favoured

Answer: product

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