1.02 moles of the gas is present in the sample.
The conditions in which the gases deviate from ideal behavior is high pressure and low temperatures.
Correct option is 2.
Explanation:
Data given:
volume of the gas = 31.2 litres
temperature of the gas = 28 degrees or 301.15 K
pressure of the gas = 82.6 kPa or 0.815 atm
R (Gas constant) = 0.0820 Latm/moles K
number of moles =?
From the ideal gas law, we have
PV = nRT
rearranging the equation:
n = 
n = 
n = 1.02 moles
At high pressure and low temperature an ideal gas deviates from ideal behaviour. Under high pressure the gas molecules get closer to each other and intermolecular force acts on them as molecules attract each other while in ideal case gas has no attractions in its molecules.
Answer:
v2 = 100 Ml OR 0.1 Liters
Explanation:
(400 Ml) (10 atm) = (v2) (40 atm)
4000 = 40v2
100 Ml = v2
Liters = ml / 1000
Liters = 100 / 1000
Liters = 0.1
Answer:
0.3023 M
Explanation:
Let Picric acid = 
So,
+
⇄
+ 
The ICE table can be given as:
+
⇄
+ 
Initial: 0.52 0 0
Change: - x + x + x
Equilibrium: 0.52 - x + x + x
Given that;
acid dissociation constant (
) = 0.42
![K_a = \frac{[H_3O^+][Picric^-]}{H_{picric}}](https://tex.z-dn.net/?f=K_a%20%3D%20%5Cfrac%7B%5BH_3O%5E%2B%5D%5BPicric%5E-%5D%7D%7BH_%7Bpicric%7D%7D)
![0.42 = \frac{[x][x]}{0.52-x}}](https://tex.z-dn.net/?f=0.42%20%3D%20%5Cfrac%7B%5Bx%5D%5Bx%5D%7D%7B0.52-x%7D%7D)
![0.42 = \frac{[x]^2}{0.52-x}}](https://tex.z-dn.net/?f=0.42%20%3D%20%5Cfrac%7B%5Bx%5D%5E2%7D%7B0.52-x%7D%7D)
0.42(0.52-x) = x²
0.2184 - 0.42x = x²
x² + 0.42x - 0.2184 = 0 -------------------- (quadratic equation)
Using the quadratic formula;
; ( where +/- represent ± )
= 
= 
=
OR 
=
OR 
=
OR 
= 0.30225 OR - 0.72225
So, we go by the +ve integer that says:
x = 0.30225
x = [
] = [
] = 0.3023 M
∴ the value of [H3O+] for an 0.52 M solution of picric acid = 0.3023 M (to 4 decimal places).
PH scale is from 1 to 14 and indicates how acidic or basic a solution is. To find pH or pOH we need to know the H⁺ ion concentration or OH⁻ concentration.
pH can be calculated using the following equation;
pH = -log[H⁺]
the H⁺ concentration of the given acid is 1.0 x 10⁻⁴ M. substituting this we can find the pH
pH = -log[1x10⁻⁴]
pH = 4
answer is 1) 4