A mixture of 0.750 mol H2 and 0.750 mol I2 was placed in a 1.00 L...

A mixture of 0.750 mol H₂ and 0.750 mol I₂ was placed in a 1.00 L flask at 430°C. The equilibrium constant K_c for the reaction is 54.3 at this temperature. Calculate the concentration of H₂, I₂, and HI at equilibrium.

H₂ + I₂ ⇌ 2 HI

Solutions

Expert Solution

queen_honey_blossom answered 2 weeks ago

Next > < Previous

Related Solutions

A.) Initially, 1.0 mol of H2 and 2.0 mol of I2 are placed into a 10.0...

A.) Initially, 1.0 mol of H2 and 2.0 mol of I2 are placed into a 10.0 L reaction flask. When equilibrium was established, the [HI] was 0.080 mol/L. Find the equilibrium concentrations of H2 and I2 and evaluate Kc for the following reaction: H2 (g)+ I2 (g) <--> 2HI (g) B.) The equilibrium constant for the reaction above is 45.0 at 490 C. What is the equilibrium concentration of each species if 1.0 mol of HI were put in a...

1.00 mol of A and 1.00 mol of B are placed in a 4.00-L container. After...

1.00 mol of A and 1.00 mol of B are placed in a 4.00-L container. After equilibrium is established, 0.400 mol of D is present in the container. Calculate the equilibrium constant for the reaction: A(g) + 3 B(g) <---> C(g) + 2 D(g)

In the reaction below, 4.24 atm each of H2 and I2 were placed into a 1.00...

In the reaction below, 4.24 atm each of H2 and I2 were placed into a 1.00 L flask and allowed to react: H2(g) + I2(g) <=> 2 HI(g) Given that Kp = 33.9, calculate the equilibrium pressure of I2 to 2 decimal places.

A 4.10 −g sample of a mixture of CaO and BaO is placed in a 1.00-L...

A 4.10 −g sample of a mixture of CaO and BaO is placed in a 1.00-L vessel containing CO2 gas at a pressure of 735 torr and a temperature of 26 ∘C. The CO2 reacts with the CaO and BaO, forming CaCO3 and BaCO3. When the reaction is complete, the pressure of the remaining CO2 is 155 torr . Calculate the number of moles of CO2 that have reacted. Calculate the mass percentage of CaO in the mixture.

If 1.00 mol of argon is placed in a 0.500-L container at 19.0 ∘C , what...

If 1.00 mol of argon is placed in a 0.500-L container at 19.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.

When 0.127 mol of NO and 17.80 g of bromine are placed in a 1.00-L reaction...

When 0.127 mol of NO and 17.80 g of bromine are placed in a 1.00-L reaction vessel and sealed, the mixture is heated to 350 K and the following equilibrium is established: 2NO(g) + Br2(g) ------> 2NOBr(g) If the equilibrium concentration of nitrosyl bromide is 8.63X10^-2 M, what is Kc ?

4.60 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose...

4.60 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.10 M, where it remained constant. A(s) <===> B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain?

a mixture of 0.2 mol of NO, 0.1 mol of H2 and 0.2 mol of H2O...

a mixture of 0.2 mol of NO, 0.1 mol of H2 and 0.2 mol of H2O is placed in 2.0 L at 300 K. At equal [NO] = 0.062. Calculate K

A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O...

A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0 L vessel at 300 K. At equilibrium [NO] = 0.062 M. 2 NO(g) + 2H2 ⇌ N2(g) + 2 H2O(g) a. What is the Kc at 300 K? b. What is the Kc of the halved reaction, given, at 300 K? NO(g) + H2 ⇌ ½ N2(g) + H2O(g) c. What is the Kp of part (a) at 300...

A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O...

A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: 2NO(g)+2H2(g)←−→N2(g)+2H2O(g) At equilibrium [NO]=0.062M. Calculate the equilibrium concentration of H2. Calculate the equilibrium concentration of N2. Calculate the equilibrium concentration of H2O. Calculate Kc

Subjects