Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.64 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.64 L flask at a certain temperature initially contains 0.765 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.3 g HI. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. please round to two digits

Solutions

Expert Solution

Important points to remember:

1. Concentration = moles/total volume

2. Law of mole balance (not mass balance, be careful) applies according to the stoichiometry of the reaction.

3. Kc is defined for the concentration of the reactants and products in equilibrium. Only subsitute the equilibrium values of concentration.

4. MW of H2 = 2 g; MW of I2 = 253.8 g; MW of HI = 127.9

5. Amount of HI produced =1/2 x Amount of H2 or I2 consumed: You can see from the stoichiometry of the reaction.

milcah answered 1 year ago

Next > < Previous

Related Solutions

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain temperature initially contains 0.767 g H2 and 96.8 g I2. At equilibrium, the flask contains 90.2 g HI.calculate the equillibrium constant (Kc) for the reaction at this temperature. please show work

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.68 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.68 L flask at a certain temperature initially contains 0.767 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.4 g HI. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. Express your answer using two significant figures.

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain temperature initially contains 0.767 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.6 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Express your answer using two significant figures.

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain temperature initially contains 0.766 g H2 and 96.8 g I2. At equilibrium, the flask contains 90.2 g HI. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. Express your answer using two significant figures. Kc= nothing SubmitPrevious AnswersRequest Answer

Consider the following reaction: H2(g)+I2(g)?2HI(g) A reaction mixture in a 3.68 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)?2HI(g) A reaction mixture in a 3.68 L flask at a certain temperature initially contains 0.761 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.3 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature.

Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.65 L flask at a certain temperature...

Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.65 L flask at a certain temperature initially contains 0.764 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.5 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Kc = ?

Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture...

Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture at equilibrium contains pressures of H2 = 0.958 atm, I2 = 0.877 atm, and HI = 0.020 atm. At the same temperature, a second reaction mixture (not at equilibrium) contains pressures of H2 = 0.621 atm, I2 = 0.621 atm, and HI = 0.101 atm. What will be the partial pressure of HI when the second reaction mixture reaches equilibrium? a) 0.0144 atm b)...

For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an...

For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.057 g H2 and 4.39 g I2. Part A What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2:...

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2: 0.050M, and HI:0 Assume this reaction is not at equilibrium. When it does reach equilibrium, what will the concentrations be?

Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.15 −L flask at a certain...

Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.15 −L flask at a certain temperature contains 26.6 g CO and 2.36 g H2 . At equilibrium, the flask contains 8.67 g CH3OH . Calculate the equilibrium constant (Kc) for the reaction at this temperature.

Subjects