A. For the reaction 3A(g)+3B(g)⇌C(g) Kc = 36.0 at a temperature of 191 ∘C . Calculate...

A. For the reaction

3A(g)+3B(g)⇌C(g)

Kc = 36.0 at a temperature of 191 ∘C .

Calculate the value of Kp . Kp = __________

B. For the reaction

X(g)+3Y(g)⇌2Z(g)

Kp = 1.47×10⁻² at a temperature of 19 ∘C .

Calculate the value of Kc .

Express your answer numerically. Kc= _______

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

For the reaction 3A(g)+3B(g)⇌C(g) Kc = 30.2 at a temperature of 377 ∘C . Calculate the...

For the reaction 3A(g)+3B(g)⇌C(g) Kc = 30.2 at a temperature of 377 ∘C . Calculate the value of Kp. Express your answer numerically. Kp = Part B For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 2.06×10−2 at a temperature of 357 ∘C . Calculate the value of Kc. Express your answer numerically. Kc =

A) For the reaction: 3A(g)+2B(g)⇌C(g) Kc = 63.4 at a temperature of 377 ∘C . Calculate...

A) For the reaction: 3A(g)+2B(g)⇌C(g) Kc = 63.4 at a temperature of 377 ∘C . Calculate the value of Kp. Express your answer numerically. B) For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 2.91×10−2 at a temperature of 229 ∘C . Calculate the value of Kc. Express your answer numerically. C) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) K = 0.155 at 1774 ∘C . What is Kp for the reaction at this temperature? Express your answer numerically. D) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp =...

± Pressure-Based versus Concentration-Based Equilibrium Constants Part A.) For the reaction 3A(g)+3B(g)⇌C(g) Kc = 67.6 at...

± Pressure-Based versus Concentration-Based Equilibrium Constants Part A.) For the reaction 3A(g)+3B(g)⇌C(g) Kc = 67.6 at a temperature of 287 ∘C . Calculate the value of Kp. Part B.) For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 1.65×10−2 at a temperature of 209 ∘C . Calculate the value of Kc.

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g) <===> 4C(g) K(c) = 2.93 x 10^(27) If, at this temperature, 2.40 mol of A and 3.70 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? [A] = ? M [B] = ? M [C] = ? M

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g) <------> 4C(g) Kc= 3.13x 10^31 If, at this temperature, 1.90 mol of A and 4.00 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium?

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A + 2B -><- 4C kc=1.33x10^27 If at this temperature, 2.00 mol of A and 3.80 mol of B are placed in a 1.00L container, what are the concentrations of A, B, C at equilibrium?

Question 2 CH13 1) For the reaction 2A(g)+2B(g)⇌C(g) Kc = 68.4 at a temperature of 311...

Question 2 CH13 1) For the reaction 2A(g)+2B(g)⇌C(g) Kc = 68.4 at a temperature of 311 ∘C . Calculate the value of Kp. Express your answer numerically. 2) For the reaction X(g)+3Y(g)⇌2Z(g) Kp = 1.76×10−2 at a temperature of 255 ∘C . Calculate the value of Kc.

At 35 degrees C, Kc = 1.6x10^-5 for the reaction: 2NOCl(g),<--> 2NO(g) + Cl2(g) Calculate the...

At 35 degrees C, Kc = 1.6x10^-5 for the reaction: 2NOCl(g),<--> 2NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following origional mixtures. a. 1.00 mol NOCl in a 1.0 L container b. 1.00 mol NO and 0.50 mol Cl2 in a 1.0 L container c. 1.00 mol NO and 0.75 mol Cl2 in a 1.0 L container The answers are: a. [NOCl]= 1.0M, [NO]= 0.032M, [Cl2]= 0.016M; b. [NOCl]= 1.0M, [NO]= 0.032M, [Cl2]=...

The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.055. The reaction...

The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.055. The reaction mixture starts with only the product, [NO] = 0.0200 M, and no reactants. Part A Find the equilibrium concentrations of N2 at equilibrium. Part B Find the equilibrium concentrations of O2 at equilibrium. Part C Find the equilibrium concentrations of NO at equilibrium.

At a certain temperature, the equilibrium constant, Kc, for this reaction is 2.60 SO2(g) + NO2(g)...

At a certain temperature, the equilibrium constant, Kc, for this reaction is 2.60 SO2(g) + NO2(g) <--> SO3(g) + NO(g) At this temperature, calculate the number of moles of NO2(g) that must be added to 3.12 mol of SO2(g) in order to form 1.30 mol of SO3(g) equilibrium

Subjects