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Chemical Equilibrium

Chemical equilibrium and molarity

Please show all work and identify all parts of equations. Please remember that this is a first year course and keep answers simple. 1. The Equilibrium Expression. Write the equilibrium expression for each of the following systems. a. 3 NO(g) ----> N2O(g) + NO2(g) b. Zn(s) + 2 H+(aq) ----> Zn2+(aq) + H2(g) c. Ti

Chemical equilibrium of PCl5(g)<---> PCl3(g) + Cl2(g)

For the following reaction at 600. K, the equilibrium constant, Kp, is 11.5 PCl5(g)<---> PCl3(g) + Cl2(g) Suppose that 3.010 g of PCl5 is placed in an evacuated 580. mL bulb, which is then heated to 600. K. a)What would be the pressure of PCl5 if it did not dissociate? b)What is the partial pressure of PCl5 at equilibri

Equlibrium Concentrations

For the equilibrium PH3BCl <=> PH3 + BCl3, Kp = .052 at 60 degrees Celcius. Further, a solid PH3BCl3 is added to a closed .500 L vessel at 60 degrees celcius; the vessel is then charged with .0216 mol of BCl3. How would I calculate Kc and what would be the equlibrium concentration of PH3?

Total Gas Pressure

For the reaction 2NaHCO3 = Na2CO3 + CO2 + H20 a 5.00 gram sample of NaHCO3 is placed in an evacuated flask and the temperature is increased to 50 degrees celcius. What is the Total Gas Pressure in the flask at equilibrium? Kp=3.90 X 10-4 = (PCO2)(PH2O.)

Calculating solubility

Calculate solubility of AbBr in 6.0 M NH3. Assume the highest complex formed is Ag(NH3)2 +.

Equilibrium

Kf=1.38 x 10 -28th power M/s. Kr = 9.3 x 10 10th power M/s. Both constants are at 25 degrees Celsius, how would I find the equilibrium constant at 25 degrees Celsius?

Concentration and equilibrium

At 1495 degrees Celcius Kc for H2 + Br2 > 2HBR = 3 x 10 to the 4th power. H2 = .10 M Br2 = .20M What eqation(s)would I use or steps would I take to find the concentration of HBr?

Solving Equilibrium

Question: 4HCl + O2 > 2Cl2 + 2H2O HCl is at 2.30 atm, O2 is at 1.00 atm and they both react at 750 K. Equilibrium pressure of Cl2 is .93 atm. How do you go about finding the Kp at 750 K?

Equilibrium Concentrations

The equilibrium constant of the reaction A <--> 2B + C shown in Figure 9.3 (attached file) is 25.6 mol^2/L^2 at an unspecified temperature. The equilibrium concentrations in this system are [A]= 0.110 M, [B]= 1.78 M and [C]= 0.890 M. The reaction system is slugged with an additional amount of reactant, equal to a concentration o

Equilibrium

At an unspecified temperature, the equilibrium reaction system I2(g) + Cl2(g) <--> 2ICl(g) has a partial pressure of ICl(g) that is 5520 times the partial pressure of I2(g). In turn, the partial pressure of I2(g) is 2.75 times the partial pressure of Cl2(g). What is Kp for the equilibrium at this unspecified temperature?

Equilibrium Disassociation Constants

The equilibrium dissociation constant, K(subscript p), of the reaction H2-->2H/H2<--2H is 3.6 x 10^-33 atm. 1.00 mol of H2 is injected into a 10.5-L oven at 600 K and allowed to reach equilibrium. Calculate the total number of free hydrogen atoms in the reaction system.

Number of Moles

Part A: If we start with 0.500 moles of H2 (subscript) and 0.500 moles of I2 (subscript) in a 5.25 L reaction vessel at 698 K, how many moles of each of the three gases will be present at equilibrium? Equation: H2(subscript) + I2(subscript) <--> 2HI KEQ= 54.3 at 698 K Part B: The same set up as part A, but this time

Chemical-Reaction Equilibria: Molar Ratio Calculations

Please see the attached file for the fully formatted problem(s). Hydrogen gas is produced by the reaction of steam with "water gas," an equimolar mixture of H2 and CO obtained by the reaction of steam with coal. A stream of "water gas" mixed with steam is passed over a catalyst to convert CO to CO2 by the reaction: H2O(g) +

Chemistry Word Problem

The Apparatus shown below consists of 3 temperature-jacketed 1.000 L bulbs connected by stopcocks. Bulb A contains a mixture of H2O(g), CO2(g), and N2(g) at 25 degrees C and a total pressure of 564 mmHg. Bulb B is empty and is held at a temperature of -70 degrees C. Bulb C is also empty and is held at a temperature of -196 degre

Find Kp and Kc given an equilibrium equation, T, and P and % dissociation.

2NOBr(g) + Br2(g) <----> 2BrNO(g) @ equilibrium. NOBr is 34% dissociated at 25degreesC and total pressure is 0.25 atm. Calculate Kp and Kc. I know how to get Kp and Kc with given # of moles @ equilibrium, but cannot figure out how to get it from the percent dissociation. I tried inputting various values that I thought wer

Equilibrium partial pressure of a gas

For the system CO(g)+H2O(g) <--> CO2(g)+H2(g) Kp is 1.6 at 900K. If 0.500 atm CO(g) and 0.500 atm H2O(g) are combined in a sealed flask, what is the equilibrium partial pressure of CO2(g)? a. 0.279 atm b. 0.308 atm c. 0.471 atm d. 0.608 atm e. 0.942 atm

Chemistry help: Equilibrium constant

Nitrosyl chloride decomposes according to this reaction: 2NOCl(g) (equilibrium sign) 2NO(g)+Cl2(g) 0.600 atm of nitrosyl chloride is sealed in a flask and allowed to reach equilibrium. If 27% of the NOCl decomposes, what is the equlibrium constant for the reaction? a. 0.00485 b. 0.781 c. 0.0300 d. 0.370 e.

Finding the value of the equilibrium constant.

For the reaction below, the partial pressures of gases at equilibrium are as follows: H2=7.1x10^-5 atm, Cl2=2.5x10^-6 atm, and HCl=3.0atm. What is the value of the equilibrium constant Kp? H2(g)+Cl2(g) = 2HCl(g)

Reactions

For which of the following reactions does Kc equal Kp? a. C2H4(g)+H2(g) (equilibrium sign) C2H6(g) b. H2(g)+l2(s) (equilibrium sign) 2Hl(g) c. 2S(s)+3O2(g) (equilibrium sign) 2SO3(g) d. SO2(g)+NO2(g) (equilibrium sign) SO3(g)+NO(g) e. both answers b and d

Equilibrium constant reaction

The equilibrium constant for a gas phase reaction is measured at two temperatures. At 100 degrees Celsius, the equilibrium constant is 36. At 200 degrees Celsius, the equilibrium constant is 147. Which of the following statements is correct for this equilibrium? a. the reaction is first order b. the reaction is endother

Equilibrium

The value of the equilibrium constant for the following reaction is 345. A+2B(equilibrium sign)3C+D What is the value of the equilibrium constant for the following reaction? 2A+4B(equilibrium sign)6C+2D K=?

Equilibrium Pressure in a System

Hydrogen iodide can decompose into hydrogen and iodide gases. Kp for the reaction is 0.016. If 0.350 atm of Hl(g) is sealed in a flask, what would be the total pressure of the system when equilibrium is established? a. 0.258atm b. 0.279atm c. 0.350atm d. 0.385atm e. 0.412atm

Equilibrium pressure and constant

At 25 degrees Celsius, the decomposition of dinitrogen tetraoxide has an equilibrium constant(Kp) of 0.144. If the equilibrium pressure of nitrogen dioxide is 0.298 atm, what is the pressure of dinitrogen tetraoxide? a. 2.07atm b. 0.162atm c. 0.617atm d. 0.0128atm

Calculating the equilibrium constant.

At 100 degrees celsius, the molarities of dinitrogen tetraoxide and nitrogen dioxide are as follows: [N204]=0.037mol/L and [NO2]=0.12mol/L What is the value of the equilibrium constant Kp?