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1. a) Show that: , equals: AGpuC")_ACC"= Hem , assuming AHxn is constant over these ranges....
9. Calculate ASⓇ, ASsurr, AStot, and AGⓇ at 298 K for the following reaction N2(g) + 3H2(g) → 2NH3(g) at 25*C. AH°...
9. Calculate ASⓇ, ASsurr, AStot, and AGⓇ at 298 K for the following reaction N2(g) + 3H2(g) → 2NH3(g) at 25*C. AH° = -92.22 kJ/mol Using: Smº[N2, gas) = 191.6J/(K-mol); Sm"[H2, gas) = 130.7J/(K-mol); Sm*[NH3, gas) = 192.4
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N2(g) + 3 H2(g) = 2 NH3(g) the standard change in Gibbs free energy is AGⓇ = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.200 bar, Ph, = 0.150 bar, and PnHz = 0.800 bar. kJ AG = mol
QUESTION 12 Given that AG for NH=-16.667999999999999 kJ/mol, calculate the equilibrium constant for the following reaction...
QUESTION 12 Given that AG for NH=-16.667999999999999 kJ/mol, calculate the equilibrium constant for the following reaction at 298 K: N2(8)+3 H2()2 NH3(g) Oa5.820000000000003 x 108 b8 349999999999996 x 102 Oc1.01 Od696999 998 x 10s O4.5099999999999998 x <1069
Need help with #6,7&9 to make sure I did it right. Will rate high if it...
Need help with #6,7&9 to make sure I
did it right. Will rate high if it is correct! Thank you.
6. Use given data to calculate the standard free- energy change for the reaction Pa(g) + 6 Cl2(g) → 4 PC13(g) at 298 K. (ii) What is AGº for the reverse of this reaction? PA(g) Cl2(g) PC13(g) 24.4 -299.6 kJ/mol AGE 9. Calculate AG at 298 K for a mixture of 2.0 atm N2, 3.0 atm H2, and 0.50 atm...
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a....
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a. Is this reaction spontaneous? Explain. b. Predict the sign of AS. Explain. C. Based on your answer to part b, is this reaction exothermic or endothermic? Explain. For the reaction N2(g) + 3H2(g) 2NH3 (8) a. Using values in Appendix Cin your book, calculate AHⓇ and AS. b. Assuming that AHºand ASº don't change with temperature, calculate the value for AG at 400K Is...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N2(g)+3H2(g)↽−−⇀2NH3(g) the standard change in Gibbs free energy is Δ?∘=−69.0 kJ/mol. What is Δ? for this reaction at 298 K when the partial pressures are ?N2=0.500 bar, ?H2=0.150 bar, and ?NH3=0.750 bar? Show work please!
1 2 Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the inte...
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Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the interval 298-600 K. Kp = 2.31x106 Submit Previous Answers ✓ Correct Part B Calculate Kp at 477 K for this reaction assuming that AHR is constant over the interval 298-600 K. PO AQ * o o ? Kp = | Submit Previous Answers Request Answer Revie For the reaction 2CH4 (g) = C2H2(g) +...
only do part (c) **please explain how to solve M^-2 The Haber process is used to...
only do part (c) **please explain how to solve M^-2
The Haber process is used to make ammonia, N2(g) + 3H2(g) = 2NH3(g) a) Write down the condition for equilibrium for this reaction in terms of the concentrations of reactants and products. At 298 K, this reaction has AH° = -46 kJ mol"', and AS° = -100 J K-mol?. Assume that AH° and ASº are independent of temperature. At what temperature does AGº vanish, i.e. AG° = 0? (c) Under...
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? N2 (g)...
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) The conditions for this reaction are: PN2 = 1.47 bar PH2 = 0.35 bar PNH3 = 1.45 bar
1.A) What is the equilibrium constant for a reaction at temperature 31.5 °C if the equilibrium...
1.A) What is the equilibrium constant for a reaction at temperature 31.5 °C if the equilibrium constant at 55.4 °C is 1.53? For this reaction, ΔrH = 20.2 kJ mol-1 . You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". 1B) What is the ΔrG° for the following reaction (in kJ mol-1)? N2(g) + O2(g) + Cl2(g)...
9. Calculate ASⓇ, ASsurr, AStot, and AGⓇ at 298 K for the following reaction N2(g) + 3H2(g) → 2NH3(g) at 25*C. AH° = -92.22 kJ/mol Using: Smº[N2, gas) = 191.6J/(K-mol); Sm"[H2, gas) = 130.7J/(K-mol); Sm*[NH3, gas) = 192.4
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N2(g) + 3 H2(g) = 2 NH3(g) the standard change in Gibbs free energy is AGⓇ = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.200 bar, Ph, = 0.150 bar, and PnHz = 0.800 bar. kJ AG = mol
QUESTION 12 Given that AG for NH=-16.667999999999999 kJ/mol, calculate the equilibrium constant for the following reaction at 298 K: N2(8)+3 H2()2 NH3(g) Oa5.820000000000003 x 108 b8 349999999999996 x 102 Oc1.01 Od696999 998 x 10s O4.5099999999999998 x <1069
Need help with #6,7&9 to make sure I
did it right. Will rate high if it is correct! Thank you.
6. Use given data to calculate the standard free- energy change for the reaction Pa(g) + 6 Cl2(g) → 4 PC13(g) at 298 K. (ii) What is AGº for the reverse of this reaction? PA(g) Cl2(g) PC13(g) 24.4 -299.6 kJ/mol AGE 9. Calculate AG at 298 K for a mixture of 2.0 atm N2, 3.0 atm H2, and 0.50 atm...
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a. Is this reaction spontaneous? Explain. b. Predict the sign of AS. Explain. C. Based on your answer to part b, is this reaction exothermic or endothermic? Explain. For the reaction N2(g) + 3H2(g) 2NH3 (8) a. Using values in Appendix Cin your book, calculate AHⓇ and AS. b. Assuming that AHºand ASº don't change with temperature, calculate the value for AG at 400K Is...
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Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the interval 298-600 K. Kp = 2.31x106 Submit Previous Answers ✓ Correct Part B Calculate Kp at 477 K for this reaction assuming that AHR is constant over the interval 298-600 K. PO AQ * o o ? Kp = | Submit Previous Answers Request Answer Revie For the reaction 2CH4 (g) = C2H2(g) +...
only do part (c) **please explain how to solve M^-2
The Haber process is used to make ammonia, N2(g) + 3H2(g) = 2NH3(g) a) Write down the condition for equilibrium for this reaction in terms of the concentrations of reactants and products. At 298 K, this reaction has AH° = -46 kJ mol"', and AS° = -100 J K-mol?. Assume that AH° and ASº are independent of temperature. At what temperature does AGº vanish, i.e. AG° = 0? (c) Under...
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