▾ Part CFind A-G at 25.0 °C under the following nonstandard conditions:P₁₂ = 0.105 mbarExpress your answer using two significant figures.A,G=SubmitIVE ΑΣΦRequest Answerboood?kJ mol-¹ Consider the sublimation of iodine at 25.0 °C:12 (s) → 12 (9)→ Show Transcribed TextPart BFind A,G at 25.0 °C under the following nonstandard conditions:P₁ = 1.95 mbarExpress your answer using two signifigures.195] ΑΣΦΑ3A,G= 12Submit Previous Answers Request Answer* Incorrect; Try Again; One attempt remaining?kJ mol-¹

In the given question we have to calculate the change in free energy of the reaction, first of all,…

Consider the sublimation of iodine at 25.0 °C: I2 (s) → 12 (9) Show Transcribed Text Part B Find A,G at 25.0 °C under the following nonstandard conditions: P₁ = 1.95 mbar Express your answer using two signifigures. ΤΕΙ ΑΣΦΑΛΟ 195] A,G= 12 Submit Previous Anwe n ? kJ mol-¹

Consider the sublimation of iodine at 25.0 °C: I2 (s) → 12 (9) Show Transcribed Text Part B Find A,G at 25.0 °C under the following nonstandard conditions: P₁ = 1.95 mbar Express your answer using two signifigures. ΤΕΙ ΑΣΦΑΛΟ 195] A,G= 12 Submit Previous Anwe n ? kJ mol-¹

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. Use the data oven i the table to calculate AHrxn, ASrxn, AGrxn, and Keq for the following reaction at 298 K. With showing all work. 2 HNO3(aq) + NO(g) →3 NO2(g) + H2O(1) K=? S° ΔΗ/ (kJ/mol) Compound (J /mol-K) 146 HNO3(aq) NO(g) NO2(g) H20(1) - 206.57 90.29 210.65 A. Calculate 4H°rxn: 33.2 239.9 -285.84 69.94 B. Calculate AS`rxn: C. Using the answers from a. And b. Calculate. AGʻrxn.:
Which of the following changes will result in an increase in the amount of phosphorous pentachloride formed?
der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.
C(s) + 2H2(g) CH4(g) ΔH° = –75 kJ exo/endo - thermic Δν(gas) = __, (decrease)Vtot --> which way will equation shift? what will happen if there is an increase in: P(CH4) shift? __ ...two ways to to lose mass(C)? ___________ higher T shift? __
Give Hand written answer Consider the reaction: X2(g)→2X(g). When a vessel initially containing 763 torr of X2 comes to equilibrium at 298 K, the equilibrium partial pressure of X is 114 torr . The same reaction is repeated with an initial partial pressure of 798 torr of X2 at 749 KK ; the equilibrium partial pressure of X is 537 torr. Find ΔH∘ for the reaction.
For the reaction A(g) + 2 B(g) = C(g) the initial partial pressures of gases A, B, and C are all 0.111 atm. Once equilibrium has been established, it is found that Pc = 0.050 atm. What is AG for this reaction (in kJ/mol) at 25°C? kJ/mol
Consider the following reactions at 25◦C:reaction Kc2 NO(g) ⇀↽ N2(g) + O2(g) 1 × 10302 H2O(g) ⇀↽ 2 H2(g) + O2(g) 5 × 10−822 CO(g) + O2(g) ⇀↽ 2 CO2(g) 3 × 1091Which compound is most likely to dissociateand give O2(g) at 25◦C?1. CO2. CO23. NO4. H2O
71. In which of the following processes would one expect AS to have the value closest to zero? - C₂H4(g) + Bra(1)→ C₂H4Br2(1) gl G H₂(B)+12(s) → 2HI(g) → CH₂CH-0₂08200) 2NO(g) + O2(g) →→ 2NO2(g) An(0 Ⓒ N2(g) + O2(g) →→→ 2NO(g) 2 A pg. 15 21₂0(g) 450 gg
Question 15 of 16 Submit Consider the reaction below: 2 SO3(g) =2 SO2(g) + O2(g) The Kp is 1.81 × 10-5 at 350.0°C. Calculate Kc at the same temperature. (R = 0.08314 L·bar/ mol · K.) 1 2 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources LO
The salt ammonium nitrate can follow three modes of decomposition: (a) to HNO; (g) and NH3(g), (b) to N₂O(g) and H₂O(g), and (c) to N₂ (g), O2 (g) and H₂O(g). Calculate AGixn for each mode of decomposition at 298 K. Compound AG NH3(g) -16.4 NH4NO3(s) -183.9 HNO3(g) -73.5 N₂O(g) 103.7 H₂O(g) -228.6 (kJ/mol) (b) to N₂O(g) and H₂O(g) Express your answer kilojoules per mole to one decimal place. AGIX = Submit Part C AGix= IT ΑΣΦ A Submit Request Answer (c) to N₂ (g), O₂(g), and H₂O(g) Express your answer in kilojoules per mole to one decimal place. | ΑΣΦ A ? Request Answer kJ/mol ? kJ/mol
how do I complete this? i am unsure of how to work this out.