1. The equilibrium constant, Kp, for the following reaction is 1.04 x 10^-2 at 5

Question

1. The equilibrium constant, Kp, for the following reaction is 1.04 x 10^-2 at 548 K NH4Cl <------>NH3 + HCl
If an equilibrium mixture of three compounds in a 4.06 L container at 548 K contains 2.64 mol of NH4Cl and 0.222 mol of NH3, the partial pressure of HCl is ______ atm
2. The equilibrium constant, Kp, for the following reaction is 1.80 x 10^-2 at 698 K 2HI <------>H2 + I2
If an equilibrium mixture of three gases in a 10.1 L container at 698 K contains HI at a pressure of 1.56 arm and H2 at a pressure of 0.635 atm, the equilibrium partial pressure of I2 is ____ atm.
3. A student ran the following reaction in the laboratory at 672 K: 2 NH3 <------> N2 + 3H2
When she introduced NH3 at a pressure of 0.761 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of H2 to be 1.13 atm.
Kp=______
4. A student ran the following reaction in the laboratory at 301 K: 2NOBr <------> 2NO + Br2
When she introduced NOBr at a pressure of 0.201 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of NOBr to be 7.58 x 10^-2 atm.
Kp=______

1. The equilibrium constant, Kp, for the following reaction is 1.04 x 10^-2 at 548 K NH4Cl <------>NH3 + HCl
If an equilibrium mixture of three compounds in a 4.06 L container at 548 K contains 2.64 mol of NH4Cl and 0.222 mol of NH3, the partial pressure of HCl is ______ atm
2. The equilibrium constant, Kp, for the following reaction is 1.80 x 10^-2 at 698 K 2HI <------>H2 + I2
If an equilibrium mixture of three gases in a 10.1 L container at 698 K contains HI at a pressure of 1.56 arm and H2 at a pressure of 0.635 atm, the equilibrium partial pressure of I2 is ____ atm.
3. A student ran the following reaction in the laboratory at 672 K: 2 NH3 <------> N2 + 3H2
When she introduced NH3 at a pressure of 0.761 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of H2 to be 1.13 atm.
Kp=______
4. A student ran the following reaction in the laboratory at 301 K: 2NOBr <------> 2NO + Br2
When she introduced NOBr at a pressure of 0.201 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of NOBr to be 7.58 x 10^-2 atm.
Kp=______

NH4Cl <------>NH3 + HCl
If an equilibrium mixture of three compounds in a 4.06 L container at 548 K contains 2.64 mol of NH4Cl and 0.222 mol of NH3, the partial pressure of HCl is ______ atm
2. The equilibrium constant, Kp, for the following reaction is 1.80 x 10^-2 at 698 K 2HI <------>H2 + I2
If an equilibrium mixture of three gases in a 10.1 L container at 698 K contains HI at a pressure of 1.56 arm and H2 at a pressure of 0.635 atm, the equilibrium partial pressure of I2 is ____ atm.
3. A student ran the following reaction in the laboratory at 672 K: 2 NH3 <------> N2 + 3H2
When she introduced NH3 at a pressure of 0.761 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of H2 to be 1.13 atm.
Kp=______
4. A student ran the following reaction in the laboratory at 301 K: 2NOBr <------> 2NO + Br2
When she introduced NOBr at a pressure of 0.201 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of NOBr to be 7.58 x 10^-2 atm.
Kp=______

Explanation / Answer

1)partial pressure of NH4Cl be x and that of NH3 be y.so,

using the ideal gas law,

PV=nRT,

or x*4.06=2.64*(1/12)*584

or x=31.64 atm

also, y*4.06=0.222*(1/12)*584

or y=2.66 atm

Hence,

1.04*10^-2=P*2.66/31.64

or P=0.1237 atm

2)Kp=Ph2*Pi2/(Phi)^2

or 1.8*10^-2=x*0.635/1.56^2

or x=0.0689 atm

3)Kp=Pn2*(Ph2)^3/(Pnh3)^2

since 1.13 atm of H2 is formed, the the partial pressure of N2 will be 1/3 of it and the partial pressure of NH3 used up will be 2/3 of it. So,

Kp=(1.13)^3*(1.13/3)/((0.761-1.13*2/3))

=70.89

4)Pnobr=7.58*10^-2

Pno=0.201-7.58*10^-2

Pbr2=0.5*(0.201-7.58*10^-2)

so, Kp=Pno^2*Pbr2/Pnobr^2

=(0.201-7.58*10^-2)^2*0.5*(0.201-7.58*10^-2)/(7.58*10^-2)^2

=0.1707

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