5.00 mol of ammonia are introduced into a 5.00 Liter reactor vessel in which it partially dissociates at high temperatures. 2 NHsubnumber3(g) = 3Hsubnumber2(g) +Nsubnumber2(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate Ksubletterc for the reaction. Please show work. Also, briefly descr
50.0 g of N2O4 is introduced into an evacuated 2.00 Litre vessel and allowed to come to equilibrium with its decomposition product, N2O4(g) = 2 NO2(g). For this reaction Kc=0.133. Once the system has reached equilibrium, 5.00 g of NO2 additional is injected in to the vessel, and the system is allowed to equilibrate once again. C
At 700 K, the reaction 2SO2(g) + O2(g) = 2SO3(g) has the equilibrium constant Kc = 4.3 x 10^6, and the following concentration are present:[SO2] = 0.010 M: [SO3] = 10.M : [O2] =0.010 M When the reaction system reaches equilibrium, what is the SO3 concentration? Please show work.
Consider the reaction Nsubnumber2(g) + Osubnumber2 = 2NO(g), for which Ksubletterc =0.10 at 2,000 degrees celcius. Starting with initial concentrations of 0.040 M of Nsubletter2 and 0.040 M of 0subnumber2, determine the equilibrium concentration of NO = means two arrows pointing opposite directions
Phosgene, OCCLsubnumber2, a poisonous gas, decomposes according to the equation OCCLsubnumber2(g) = CO(g) +CLsubnumber2(g). Calculate K,subletterp, for this reaction if Ksublettterc = 0.083 at 900 degrees celcius please show work.
The equation constant for the reaction Ni(s) = 4CO(g) = Ni(CO)subnumber 4(g) is 5.0 x10^4 at 25 degrees celcius. What is the equilibrium constant for the reaction Ni(CO) subnumber4 (g)= NI(s) = 4CO(g)? the equal sign is actually two arrows pointing opposite directions.
I do not understand why a reaction (oxidation and reduction) can continue producing electricity if equilibrium (at a given temperature) has already been reached. For example, the conversion of Fe2+(aq) ion to Fe3+(aq) ion is necessary for the anode half reaction to continue producing electrons while the continued conversion of
Please show all work and explain the formulas through to the answer. 1. The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write the chemical equilibrium equation that describes the salt partially dissolving in water and the solubility product expression. Calculate the Ksp value for lead(II) bromide if the
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
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
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?
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.)
Calculate solubility of AbBr in 6.0 M NH3. Assume the highest complex formed is Ag(NH3)2 +.
Calculate molar solubility of Fe(OH)2 in 0.10 Molar NaOH.
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?
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?
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?
Given two isomers (anomers) of a sugar with a specific rotational character, knowing the specific rotatoin of the equilibrium mixture, what are the percentages of each in the mix?
Q1. à¿-D-Galactopyranose has [à¿]D = +150.7o, and à¿-D-galactopyranose has [à¿]D = +52.8o. When either of them is dissolved in water and allowed to reach equilibrium, the specific rotation of the solution will be +80.2o. What are the percentages of each anomer at equilibrium?
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
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?
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.
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
When VO2+ reacts with Ti2+ in acid solution the products are V2+ and TiO2+. a) What is the potential of the cell Pt/VO2+, V2+//TiO2+, Ti2+/Pt if all species are a 1 M. b) Write the equilibrium constant expression and calculate the value of the equilibrium constant.
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) +
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
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
Multiple choice question about what can change the ratio of products to reactants in an equilibrium gaseous mixture.
Which of the following will NOT change the ratio of the products to reactants in an equilibrium mixture for a chemical reaction involving gaseous species? a. increasing the pressure b. decreasing the volume c. addition of a solid reactant d. removal of a gaseus product e. none of the above
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
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.
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)