The following reaction is investigated (assume an ideal gas mixture):2N2O(g) + N2H4(g) 3N2(g) + 2H2O(g)Initially there are 0.10 moles of N2O and 0.25 moles of N2H4, in a 10.0-L container. If there are 0.046 moles of N2O at equilibrium, how many moles of N2 are present at equilibrium? Calculate the K for this system.

For the equilibrium2IBr(g)⇌I2(g)+Br2(g)2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 Kp=8.5×10−3 at 150 ∘C a) If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? b)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? c)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of Br2 after equilibrium is reached?

At a certain temperature, an equilibrium mixture of O2, SO2, and SO3 contains equal concentrations of of SO2 and SO3.  Calculate the concentration of O2 at this temperature if Kc = 70 for the reaction at this temperature. 2 SO2(g)  +  O2(g)  ⇆ 2 SO3(g)

Consider the following system at equilibrium: N2(g) + 3H2(g)  2NH3(g) + 92.94 kJWhich of the following changes will shift the equilibrium to the right? I. increasing the temperature II. decreasing the temperature III. increasing the volume IV. decreasing the volume V. removing some NH3 VI. adding some NH3 VII. removing some N2 VIII. adding some N2 ​ Group of answer choices I, IV, VI, VII II, III, V, VIII I, VI, VIII I, III, V, VII II, IV, V, VIII

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:COCl2(g) CO(g) + Cl2(g)If 2.98×10-2 moles of COCl2, 0.206 moles of CO, and 0.304 moles of Cl2 are at equilibrium in a 17.8 L container at 672 K, the value of the equilibrium constant, Kp, is .

Consider the following equilibrium: 2NOCI (g) - 2NO (g) + Cl, (g) AG-41. kJ Now suppose a reaction vessel is filed with 4.69 atm of nitrosyl chloride (NOCI) and 4.34 atm of chlorine (CI,) at 641. "C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCI tend to rise or fall? O fall ? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fal by adding NO? Similarly, if you said the pressure of NOCI wil tend to fall, can that be changed to a tendency to rise by adding NO? O yes O no Ir you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits.

Gaseous SO3 is placed in a closed container at 685 oC, where it partially decomposes to SO2 and O2: 2 SO3(g)  2 SO2(g) + 1 O2(g) At equilibrium it is found that p(SO3) = 0.001810 atm, p(SO2) = 0.007320 atm, and p(O2) = 0.009270 atm. What is the value of KP at this temperature? KP =  _______