Pencil "lead" is almost pure graphite. Graphite is the stable elemental form of carbon at 25°C and 1 atm. Diamond is an allotrope of graphite. The reaction at equilibrium is Caraphte Caiamond Given diamond: AHP 1.9 kl/mol, S - 24 /mol K Solve for AS 2.39 x kJ/K mol Solve for AH 1.9 v KJ/mol Is there a temperature where the two can be at equilibrium at 1 atm? no

Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. increases.     B. decreases.     C. remains the same.   The value of Q fill in the blank 2 A. is greater than Kc.     B. is equal to Kc.     C. is less than Kc.   The reaction must: fill in the blank 3 A. run in the forward direction to reestablish equilibrium.     B. run in the reverse direction to reestablish equilibrium.     C. remain the same. It is already at equilibrium.   The concentration of H2 will: fill in the blank 4 A. increase.     B. decrease.     C. remain the same.

Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise 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. Round your answer to 2 significant digits. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S

Consider the following reaction: CO2(g) + C(graphite) = 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. If the equilibrium pressure of CO gas is 0.83 atm, find the equilibrium constant (Kp) for the reaction.

A reaction vessel is charged with 0.50 atm of A and 0.300 atm of B. Once the reaction reaches equilibrium, what is the equilibrium partial pressure of B? Kp for this reaction is 67.2 A(g) - 2 B (g)

Consider the following exothermic reaction, used to obtain lead from its ore:2PbS (s) + 3O2 (g) + 2CO (g) ↔ 2 Pb (l) + 2SO2 (g) + 2CO2 (g)Assume that this reaction is in equilibrium. Given the following changes to the system, will the quantity of lead increase, decrease, or remain the same?i) adding more lead sulfide.ii) Adding more carbon monoxide.iii) removing some oxygen.