A sample of solld ammonlum chloride was placed in an evacuated chamber, and then heated causing it to decompose according to the following reaction: NH4CI(S) NH3(g) + HCl(g) In a particular experiment the pressure of NH3(g) in the container was found to be 2.9 atm. Calculate the value of Kp for the decomposition of NH4Cl(s) at this temperature. Kp = Submit Show Hints Submit Answer Retry Entire Group 9 more group attempts remaining

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.

At 1560 oC the equilibrium constant for the reaction: 2 IBr(g)  I2(g) + Br2(g) is KP = 0.846. If the initial pressure of IBr is 0.00674 atm, what are the equilibrium partial pressures of IBr, I2, and Br2?p(IBr) =  p(I2) =  p(Br2) =

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

Some quantity of NOBr is added to an otherwise empty flask. The reaction: 2 NOBr (g) ⇄ 2 NO (g) + Br2 (g) takes place at a particular temperature for which KP  is 3.5 x 10-5. Assuming an equilibrium pressure of NOBr = 2.46atm, what is the equilibrium pressure of NO?

At 500K, the methanol decomposes according to the following reaction, CH3OH(g) = CO(g) + 2 H2(g) K= 9.60×10-2 Some methanol, CH3OH (molar mass: 32 g/mol), is placed into a rigid 2.00-L vessel, and the temperature is raised to 500K. If the concentration of H2 in the equilibrium mixture is 0.246M, what is the initial concentration of methanol? O A, 0.231 M Ов. 0.866 М OC 0.200 M OD. 1.109 M O E. 0.012 M

The value of K, for the reaction 2 NO, (g) N204 (g) is 1.52 at 319 K. What is the value of the Kp of the reaction NO2 (g) 1/2 N204 (g) at this temperature: 0.761 O2.31 1.23 1.52 0.811 A Moving to another question will save this response. Esc AI C 中 F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 23 %24

The equilibrium constant Kp for the reaction PC15(g) = PC13(g) + Cl₂(g) is 1.05 at 250°C. The reaction starts with a mixture of PC15, PC13, and Cl₂ at pressures 0.177 atm, 0.233 atm, and 0.161 atm, respectively, at 250°C. When the mixture comes to equilibrium at that temperature, which pressure(s) will have decreased? Cl₂ PC13 PC15

At 25 °C, the following concentrations were found for the gases in an equilibrium mixture for the reaction N₂O(g) + NO₂(g) = 3NO(g) [NO₂] = 0.75 M, [NO] = 9.0 × 10-8 M, and [N₂O] = 0.033 M. What is the value of Kp for this reaction? Enter your answer in scientific notation. Kp= i x 10 i

Kp is equal to 25.00 at some temperature for the reaction: H2(g) + I2(g) ⇌ 2 HI(g).  Clair and Pat put the gases in a sealed container with 0.1000 atm each of H2 and I2; and 1.0000 atm of HI, then waited for the system to reach equilibrium several hours later.  Calculate the Reaction Quotient giving the starting concentrations.