Answer:
The <u>equilibrium constant</u> is:
Explanation:
The correct equation is:
Thus, with the equilibrium concentrations you can calculate the equilibrium constant, Kc.
The equation for the equilibrium constant is:
![k_c=\dfrac{[NH_3]^2}{[N_2]\cdot [H_2]^3}](https://tex.z-dn.net/?f=k_c%3D%5Cdfrac%7B%5BNH_3%5D%5E2%7D%7B%5BN_2%5D%5Ccdot%20%5BH_2%5D%5E3%7D)
Substituting:
Answer:
Final temperature = 
Explanation:
Given that,
Heat added, Q = 250 J
Mass, m = 30 g
Initial temperature, T₁ = 22°C
The Specific heat of Cu= 0.387 J/g °C
We know that, heat added due to the change in temperature is given by :
Put all the values,
So, the final temperature is equal to .
Answer:
It's the last option.
Explanation:
H3PO4 + 5HCl → PCl5 + 4H2O
Answer:
0.54g of Cr
Explanation:
Current (I) = 10A
Time (t) = 100s
Molecular mass of Cr = 51.996 amu
Faraday's first law of electrolysis states that
The mass of the substance (m) of a given substance deposited at an electrode is directly proportional to the quantity of electricity or charge (Q) passed
m = nQ
M = mass of the substance
n = electrochemical constant
Q = charge passed through it
Q = IT
Q = (10 * 100) = 1000C
1 moles = molarmass = Faraday's constant (96500C)
Molar mass = Faraday's constant (96500C)
51.996 g = 96500C
How many grams will be liberated with 1000C
51.996g = 96500C
Xg = 1000C
X = (1000 * 51.996) / 96500
X = 51996 / 96500
X = 0.5388g = 0.54 g of Cr will be deposited
