CHEMWORK A sample of solid ammonium chloride was placed in an evacuated chamber, and then heated causing it to decompose according to the following reaction: NH Cl(s) NH3(g) + HCl(g) In a particular experiment the pressure of NH3(g) in the container was found to be 2.1 atm. Calculate the value of K, for the decomposition of NH Cl(s) at this temperature. Kp

10) For the reaction: 2 V PC13(g) + Cl2(g) → PC15(g) at 85°C, Kp = 1.19 = If one starts with 2.00 atm pressure of PC13, 1.00 atm pressure of Cl2 and no PC15, what is the partial pressure of PC15(g) at equilibrium? A) 0.739 atm B) 0.621 atm C) 0.465 atm D) 0.167 atm E) 0.553 atm

The elementary reaction 2 H, O(g) = 2 H, (g) + 0, (g) proceeds at a certain temperature until the partial pressures of H,O, H,, and O, reach 0.0350 atm, 0.00650 atm, and 0.00150 atm, respectively. What is the value of the equilibrium constant at this temperature? Kp

Br2(g) + Cl2(g)  2BrCl(g)If the partial pressures in an equilibrium mixture of Br2, Cl2, and BrCl are 1.12 atm, 1.26 atm, and 3.14 atm, respectively, Find Kp for this reaction at this temperature.

The value of Kp for the reaction 2 A(g) + B(g) + 3 C(g) → 2 D(g) + E(g) is 12770 at a particular temperature. What does the magnitude of Kp tell us about the equilibrium position of the reaction? A) There are many more products than reactants. B) There are only a few more products than reactants. C) There are many more reactants than products. D) There are only a few more reactants than products.

Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4NO(g)+6H2O(g)——> 4NH3(g)+ 5O2(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, water, ammonia, and oxygen has the following composition(picture). Calculate the value of the equilibrium constant Kp for this reaction. Round your answer to 2 significant digits.

The elementary reaction 2 H,O(g) = 2 H,(g)+ 0,(g) proceeds at a certain temperature until the partial pressures of H,0, H,, and O, reach 0.0500 atm, 0.00350 atm, and 0.00150 atm, respectively. What is the value of the equilibrium constant at this temperature? Kp =

4. IBr decomposes according to the reaction at 150 C: 2 IB (g) = 12 (g) + Brz (g) If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its equilibrium pressure at 150°C? K = 8.3 x 10-3

At 150°C, Kp = 1.2x10- for the reaction 12(g) + Br2(g) 5 2Brl(g). A rigid cylinder at that temperature contains 0.127 atm of bromine, 0.134 atm of iodine, and 1.055 atm of bromine monoiodide. What is the value of the reaction quotient, Qp? O 55.2 62.0 O 65.4 O 88.3

Phosphine gas (PH3), decomposes by the reaction shown below.  A total pressure of 0.64 atm of pure phosphine gas was placed in a sealed 1.00-L flask at 298 K. After equilibrium was attained, the total pressure inside the flask was found to be 0.93 atm. Calculate the mass of solid phosphorous in the flask. PH3(g)   <-->   P(s)   +   3 H2(g)