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![Coc c o + Cl2 Kc [product [ Reactant → Ke - [60] [612] [cocia ke: (1.2 x 102). (0.054) (0.14) Kc = 0.463 x 10-2 Kc = 4.63 x 1](http://img.homeworklib.com/questions/691feb40-7808-11ea-a2bb-e1f24ef281f2.png?x-oss-process=image/resize,w_560)
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In an experiment conducted at 74°C, the equilibrium concentrations of...
Notice the Kp is given, not Kc In an experiment conducted at 74°C, the equilibrium concentrations were 0.012 M CO and 0...
Notice the Kp is given, not Kc
In an experiment conducted at 74°C, the equilibrium concentrations were 0.012 M CO and 0.054 M Cl2. CO(g) + Cl2(g) CoCl2g Kp = 2.2 x102 at 74°C What is the equilibrium concentration of CoCl2? A. 0.14 M B. 7.0 M C. 0.32 M D. 2.1 M
would an expert verify if this is right. thank you ave u 2. In an experiment...
would an expert verify if this is right. thank you
ave u 2. In an experiment conducted at 74°C, the equilibrium concentrations of reactants and products for the equation shown below were [CO] = 1.2 x 102M, [Cl2] = 0.054 M and [COCI:] =0.14 M. COCI, (g) - CO(g) + Cl2 (g) a) What is the equilibrium expression for this reaction? K = [co] [cle] [Coco Ke@ 740 b) Calculate the value of the equilibrium constant, Kc. K. (1.24 16...
Please show how X is derived For the following reaction Kc = 2.20 x 102 at...
Please show how X is derived
For the following reaction Kc = 2.20 x 102 at 74°C | CO(g) + Cl2(g) ←→ COCI2(g) Find the equilibrium concentrations of all chemical species starting with [CO]-0.161 M and [C12] = 0.205 M. [CO] = [C2] - [coci2)- COCI2]
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at...
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
At 100 °C the equilibrium constant for the reaction COCI2 (g) CO (g) +Cl2 (g) has...
At 100 °C the equilibrium constant for the reaction COCI2 (g) CO (g) +Cl2 (g) has the value Ke following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. 2.19 x 1010. Are the Part A 3.3 x 10-6 M. [Cl2] = 6.62 x 10- M [COCI2] = 2.00 x 10-3 M. [CO] The reaction is at equilibrium. The reaction will proceed right to attain...
1. 1.75 moles of H202 were placed in a 2.50 L reaction chamber at 307°C. After...
1. 1.75 moles of H202 were placed in a 2.50 L reaction chamber at 307°C. After equilibrium was reached, 1.20 moles of H202 remained. Calculate the equilibrium constant, Kc, for the reaction. 2. Phosgene, COCl,, a poisonous gas, decomposes according to the equation COC2(g) CO(g)+ Cl2(g) Calculate Kp for this reaction if Kc- 0.083 at 900°C. K K.(PT) 3. Calculate Kc for the reaction 2HI(g) H2(g) +12(g) given that the concentrations of each species at equilibrium are as follows: [HI...
Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl, is all...
Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl, is allowed to dissociate into CO and Cl, at 873 K. At equilibrium, [COCI2] = 0.184 M, and [CO] = [Cl2] = 0.113 M. Additional CO is added so that (CO)new = 0.175 M and the system is allowed to once again reach equilibrium. K= COC12(g) CO(g) + Cl2(g) 6.98x10-2 at 873 K (a) In which direction will the reaction proceed to reach equilibrium?...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. A) For the reaction 3A(g)+3B(g)⇌C(g) Kc =...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)?n where R=0.08206 L?atm/(K?mol), T is the absolute temperature, and ?n is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)?2NH3(g) for which ?n=2?(1+3)=?2. Part A For the reaction 3A(g)+3B(g)?C(g) Kc...
if someone can help answer these questions tion 18 O out of 4 points At the...
if someone can help answer these questions
tion 18 O out of 4 points At the start of a reaction, there are 1.05 moles of NO, 0.955 moles of Bry, and 1.15 moles of NOBr in a 5.5 L reaction vessel at 727 "C. From these initial molar concentrations, decide whether the system is at equilibrium. If not, predict which direction the net reaction will proceed. (Hint: Reaction Quotient) 2NO(g) + Br2(g) + 2NOBr() Ke 0.013 Question 19 O out...
Notice the Kp is given, not Kc
In an experiment conducted at 74°C, the equilibrium concentrations were 0.012 M CO and 0.054 M Cl2. CO(g) + Cl2(g) CoCl2g Kp = 2.2 x102 at 74°C What is the equilibrium concentration of CoCl2? A. 0.14 M B. 7.0 M C. 0.32 M D. 2.1 M
would an expert verify if this is right. thank you
ave u 2. In an experiment conducted at 74°C, the equilibrium concentrations of reactants and products for the equation shown below were [CO] = 1.2 x 102M, [Cl2] = 0.054 M and [COCI:] =0.14 M. COCI, (g) - CO(g) + Cl2 (g) a) What is the equilibrium expression for this reaction? K = [co] [cle] [Coco Ke@ 740 b) Calculate the value of the equilibrium constant, Kc. K. (1.24 16...
Please show how X is derived
For the following reaction Kc = 2.20 x 102 at 74°C | CO(g) + Cl2(g) ←→ COCI2(g) Find the equilibrium concentrations of all chemical species starting with [CO]-0.161 M and [C12] = 0.205 M. [CO] = [C2] - [coci2)- COCI2]
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
At 100 °C the equilibrium constant for the reaction COCI2 (g) CO (g) +Cl2 (g) has the value Ke following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. 2.19 x 1010. Are the Part A 3.3 x 10-6 M. [Cl2] = 6.62 x 10- M [COCI2] = 2.00 x 10-3 M. [CO] The reaction is at equilibrium. The reaction will proceed right to attain...
1. 1.75 moles of H202 were placed in a 2.50 L reaction chamber at 307°C. After equilibrium was reached, 1.20 moles of H202 remained. Calculate the equilibrium constant, Kc, for the reaction. 2. Phosgene, COCl,, a poisonous gas, decomposes according to the equation COC2(g) CO(g)+ Cl2(g) Calculate Kp for this reaction if Kc- 0.083 at 900°C. K K.(PT) 3. Calculate Kc for the reaction 2HI(g) H2(g) +12(g) given that the concentrations of each species at equilibrium are as follows: [HI...
Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl, is allowed to dissociate into CO and Cl, at 873 K. At equilibrium, [COCI2] = 0.184 M, and [CO] = [Cl2] = 0.113 M. Additional CO is added so that (CO)new = 0.175 M and the system is allowed to once again reach equilibrium. K= COC12(g) CO(g) + Cl2(g) 6.98x10-2 at 873 K (a) In which direction will the reaction proceed to reach equilibrium?...
if someone can help answer these questions
tion 18 O out of 4 points At the start of a reaction, there are 1.05 moles of NO, 0.955 moles of Bry, and 1.15 moles of NOBr in a 5.5 L reaction vessel at 727 "C. From these initial molar concentrations, decide whether the system is at equilibrium. If not, predict which direction the net reaction will proceed. (Hint: Reaction Quotient) 2NO(g) + Br2(g) + 2NOBr() Ke 0.013 Question 19 O out...
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