Answer:
I think C option ✔️ ✔️ correct
Mass of KNO₃ : = 40.643 g
<h3>Further explanation</h3>
Given
28.5 g of K₃PO₄
Required
Mass of KNO₃
Solution
Reaction(Balanced equation) :
2K₃PO₄ + 3 Ca(NO₃)₂ = Ca₃(PO₄)₂ + 6 KNO₃
mol K₃PO₄(MW=212,27 g/mol) :
= mass : MW
= 28.5 : 212,27 g/mol
= 0.134
Mol ratio of K₃PO₄ : KNO₃ = 2 : 6, so mol KNO₃ :
= 6/2 x mol K₃PO₄
= 6/2 x 0.134
= 0.402
Mass of KNO₃ :
= mol x MW KNO₃
= 0.402 x 101,1032 g/mol
= 40.643 g
Answer:
See explanation
Explanation:
Anode;
Sn(s) ------> Sn^2+(aq) + 2e
Cathode;
Mn^2+(aq) + 2e ------> Mn(s)
The minimum voltage required to drive the reaction is the cell voltage. The cell voltage is obtained from;
E°cell= E°cathode - E°anode
E°cell= -1.19 - (-0.14)
E°cell= -1.05 V
Answer:
A)Boiling point constant of benzene = 2.63°C/m
B) 242.77 g/mol is the molar mass of the solute.
Explanation:
where,
=Elevation in boiling point
= boiling point constant od solvent= 3.63 °C/m
1 - van't Hoff factor
m = molality
A) Mas of solvent = 500 g = 0.500 kg
T = 80.1°C , =82.73°C
= 82.73°C - 80.1°C = 2.63°C
Boiling point constant of benzene = 2.63°C/m
B) Mass of solute = 1.2 g
Molar mas of solute = M
Mass of solvent = 50 g= 0.050 kg
i = 1
T = 80.1°C , =80.36°C
=80.36°C - 80.1°C = 0.26°C
M = 242.77 g/mol
242.77 g/mol is the molar mass of the solute.