Answer:
The ideal gas equation
Explanation:
The ideal gas equation is derived from the combination of three gas laws:
The ideal gas law is expressed mathematically as: PV=nRT where:
P is pressure
V is volume
n is the number of moles
R is the ideal gas law
T is temperature.
To obtain the combined gas law, we assume that n=1 and this gives:
= R
Therefore:
=
<u>Answer:</u>
<u>For 1:</u> The value of for above reaction is 36.83
<u>For 2:</u> The value of for above reaction is 36.83
<u>For 3:</u> The equilibrium partial pressure of Indium is 0.126 atm
<u>For 4:</u> The equilibrium partial pressure of hydrogen gas is 0.094 atm
<u>For 5:</u> The equilibrium partial pressure of Indium dihydrogen is 0.018 atm
<u>Explanation:</u>
We are given:
Partial pressure of Indium gas = 0.0650 atm
Partial pressure of hydrogen gas = 0.0330 atm
Partial pressure of Indium dihydride = 0.0790 atm
The given chemical equation follows:
<u>Initial:</u> 0.065 0.033 0.079
<u>At eqllm:</u> 0.065-x 0.033-x 0.079+x
The expression of for above reaction follows:
Putting values in above equation, we get:
Hence, the value of for above reaction is 36.83
We are given:
of the reaction = 1.48
There are 3 conditions:
As, for the given reaction, the reaction is reactant favored.
Hence, the reaction proceed in the backward direction to attain equilibrium
The expression of for above reaction follows:
Putting values in above equation, we get:
Neglecting the value of x = 0.835 because the reaction is going backwards. So, by taking this value, the pressure of the reactants will decrease
So, equilibrium partial pressure of Indium = (0.065 - x) = [0.065 - (-0.061)] = 0.126 atm
The equilibrium partial pressure of hydrogen gas = (0.033 - x) = [0.033 - (-0.061)] = 0.094 atm
The equilibrium partial pressure of Indium dihydrogen = (0.079 + x) = [0.079 + (-0.061)] = 0.018 atm