At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature,...

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.500 mol of H2 and 0.500 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

At a certain temperature, the equilibrium constant Kc for this reaction is 53.3 H2 + I2...

At a certain temperature, the equilibrium constant Kc for this reaction is 53.3 H2 + I2 ---> 2HI <--- at this temperature, 0.500 mol of H2 AND 0.500 mol of I2 were placed in 1.00L container to react. What concentration of HI is present at equilibrium? [HI]= ?M

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?

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?

The equilibrium constant Kc for the reaction below is 0.00427 at a certain temperature. Br2(g) ⇌...

The equilibrium constant Kc for the reaction below is 0.00427 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0844 M and [Br] = 0.0763 M, calculate the concentrations of these species at equilibrium.

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature,...

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌...

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

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

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ↔...

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask? At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are...

a) Give the mathematical equilibrium constant expression Kc and Kp (not the value!) for the reaction...

a) Give the mathematical equilibrium constant expression Kc and Kp (not the value!) for the reaction 2N2O5(g) ↔ 4NO2 (g) + O2(g) b) At 250oC the concentrations of N2O5, NO2 and O2 are 0.100 mol/L, 0.0283 mol/L and 0.0105 mol/L. Calculate the values for Kc and Kp

Subjects