Answer:
a. [HI]² / [I₂] . [H₂]
b. Kc = 46.9
c. This is an homogeneous reaction
Explanation:
The equilibrium is this:
H₂ (g) + I₂ (g) ⇄ 2HI (g)
Eq. 0.102M 0.00183M 0.0963M
The expression for Kc will be:
Kc = [HI]² / [I₂] . [H₂]
Kc = 0.0963² / 0.00183 . 0.102
Kc = 46.9
The reaction is homegeneous, because all the reactants and the product are at the same phase. In this case, as the reaction is homogeneous, the speed of reaction is not affected by the exposed surface area.
If it was an heteregeneous reaction, it would depend on the area of the surface exposed to the mixture of reaction. The heterogeneous reaction are in a different phase, for example a catalyst in a different phase as the reactants.
According to Gases law, we know,
PV/T = Constant
So, P₁V₁/T₁ = P₂V₂/T₂
Here, P₁ = 108 kPa
V₁ = 592.2 mL
T₁ = 10+273 = 283 K
P₂ = ?
V₂ = 750 mL
T₂ = 28.9+273 = 301.9
Substitute their values,
108 * 592.2 / 283 = P₂ * 750 / 301.9
P₂ = 63957.6 * 301.9 / 283 * 750
P₂ = 19308799.44 / 212250
P₂ = 90.97 kPa
In short, Your Final Answer would be: 90.97 kPa
Hope this helps!
Answer:
Whenever you are doing calculations with gases and temperature, you must convert the temperature from C into Kelvin. Then, just plug in your values and do the calculation. So, for the first one,
32C + 273 = 305 K
63C + 273 = 336 K
Then, P1/T1 = P2/T2
575 torr / 305 K = P2 / 336 K
P2 = 633 torr
For the second one:
P1/T1 = P2/T2
575/305 = 5750 / T2
T2 = 3050 K
Answer:
b. is always a weak electrolyte.
Explanation:
Such compounds of low solubility dissociates partly and hence cannot be strong electrolytes
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