For the reaction 2HF(g) H2(g) + F2(g), ΔG° = 38.3 kJ, at 1000 K. If, at this temperature, 5.00 moles of HF(g), 0.500 moles of H2(g), and 0.75 moles of F2(g) are mixed in a 1.00-L container: Group of answer choices A) Some HF will decompose (to yield H2 and F2). B) The system is at equilibrium. C) Some HF will be formed (from H2 and F2). D) Not enough data are given to answer this question. E) None of these (A-D)

Phosgene (COCl2) is used in the manufacture of foam rubber and bulletproof glass. It is formed from carbon monoxide and chlorine in the following reaction:Cl2​(g)+CO(g) ----> COCl2​(g)   The value of Kc for the reaction is 17.1 at 540.4 °C. What is the value of Kp at 540.4 °C?

Use the data below to calculate ΔG at 245 K for each of the following reactions.  Compound   ΔH°f (kJ/mol) ΔS°f (J/mol·K)  H2S(g)    -20.17  205.6  O2(g)    0  205.0  H2O(g)    -241.8  188.7  SO2(g)    -296.8  248.2                                   2H2​S(g)+3O2​(g) --> 2H2​O(g)+2SO2​(g) ΔG245  =   ___  kJ

Consider the following reaction, the equilibrium constant for this reaction at 298 K is 0.113: 2NO2(g) ⇌ N2O4(g) A) You have a system with 5.00 atm of NO2 and 7.00 atm of N2O4 is this reaction at equilibrium? Calculate Q tosupport your answer.B) Which way will the reaction proceed to reach equilibrium? C) Using the value of K, calculate the value for ΔG°.

Consider the following reaction:    A (g) + B(g) ↔ 2C(g)                   Kp = 0.0825 at 298 K   Calculate ΔG (J/mol) at 25°C when P(A) = 1.50 atm, P(B) = 3.20 atm and P(C) = 4.00 atm   Enter your answer with the correct number of sig figs, without any units.  If you want to use scientific notation, use the #e# format.

-) Phosphorous and chlorine gases combine to produce phosphorous trichloride: P2(g) + 3C12(g) → 2PC13(g) AG° at 298 K for this reaction is -642.9 kJ/mol. At 298 K for a reaction mixture that consists of 2.0 atm P2, 2.0 atm Cl and 1.0 atm PC13 what is the value of AG?

For the following reaction, AH = 2816 kJ. 6 CO₂(g) + 6 H₂O(I) ⇒ C6H12O6(s) + 6 O₂(g) Select ONE combination of strategies that when applied to this system at equilibrium will result in an increase in the amount of C6H₁2O6 as equilibrium is re-established? a. Increasing Po₂ by adding more O2; increasing the temperature; decreasing the volume; or removing CO₂ b. Increasing Po₂ by adding more O₂ and decreasing the volume C. Decreasing the volume d. Increasing Po₂ by adding more O₂ e. Increasing the temperature

In which of the following reactions is ASº expected to be negative? O L(s)I(g) O 2NH;(g) → N(g) + 3H3(g) O 2H,0(g) → 2H,(g) + O>(g) O CH;OH(g) → CH;OH(I) O AS° is not expected to be negative for any of these.

∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true?   To make this reaction go forward, 33.3 kJ must be added.   This reaction is non-spontaneous.   This reaction is spontaneous.   This reaction cannot be at equilibrium.

Consider the following equilibrium: N₂ (g) + 3H₂(g)2NH₂ (g) AG = -34. KJ 2 Now suppose a reaction vessel is filled with 3.70 atm of hydrogen (H₂) and 8.46 atm of ammonia (NH3) at 1099. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of H ₂ tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding N₂? x Ś ? In other words, if you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the yes no pressure of H₂ will tend to fall, can that be changed to a tendency to rise 2 by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. atm Round your answer to 2 significant digits. ● O