At a temperature of 30 deg C, the vapour pressure of water
H2O is about 32 mm Hg. Therefore at a total pressure f 734 mm Hg, the partial
pressure of the Hydrogen gas collected is:
<span>P Hydrogen = 734 mm Hg – 32 mm Hg = 702 mm Hg</span>
Answer:
-68.4 kJ
Explanation:
<u>The standard enthalpy of vaporization = 23.3 kJ/mol</u>
<u>which means the energy required to vaporize 1 mole of ammonia at its boiling point (-33 °C).</u>
To calculate heat released when 50.0 g of ammonia is condensed at -33 °C.
This is the opposite of enthalpy of vaporization which means that same magnitude of heat is released.
<u>Thus, Q = -23.3 kJ/mol</u>
<u>Where negative sign signifies release of heat</u>
Given: mass of 50.0 g
Molar mass of ammonia = 17.034 g/mol
Moles of ammonia = 50.0 /17.034 moles = 2.9353 moles
Also,
1 mole of ammonia when condenses at -33 °C releases 23.3 kJ
2.9412 moles of ammonia when condenses at -33 °C releases 23.3×2.9353 kJ
<u>Thus, amount of heat released when 50 g of ammonia condensed at -33 °C= -68.4 kJ, where negative sign signifies release of heat.</u>
Answer:
Keq: [SO3][NO] /[SO2]NO2]
Explanation:
Answer: precipitation of 
from 
and 
ions in solution
Explanation:
Entropy is the measure of randomness or disorder of a system. If a system moves from an ordered arrangement to a disordered arrangement, the entropy is said to decrease and vice versa.
is positive when randomness increases and is negative when randomness decreases.
a) precipitation of from and ions in solution : As ions are getting solidified, entropy decreases.
b) dissolution of 
in water: The compounds dissociates into ions, entropy increases.
c) melting solid gold into liquid gold: The randomness increases, entropy increases.
d) evaporation of Hg(l) to form Hg(g) : The randomness increases, entropy increases.
e) mixing of two gases into one container : The randomness increases, entropy increases.
