Answer:
127.3° C, (This is not a choice)
Explanation:
This is about the colligative property of boiling point.
ΔT = Kb . m . i
Where:
ΔT = T° boling of solution - T° boiling of pure solvent
Kb = Boiling constant
m = molal (mol/kg)
i = Van't Hoff factor (number of particles dissolved in solution)
Water is not a ionic compound, but we assume that i = 2
H₂O → H⁺ + OH⁻
T° boling of solution - 118.1°C = 0.52°C . m . 2
Mass of solvent = Solvent volume / Solvent density
Mass of solvent = 500 mL / 1.049g/mL → 476.6 g
Mol of water are mass / molar mass
76 g / 18g/m = 4.22 moles
These moles are in 476.6 g
Mol / kg = molal → 4.22 m / 0.4766 kg = 8.85 m
T° boling of solution = 0.52°C . 8.85 m . 2 + 118.1°C = 127.3°C
Answer:
0.003088 moles of hydrogen gas were formed .
Explanation:
Pressure at which hydrogen gas is collected at 20°C = 768.0 Torr
Vapor pressure of water at 20°C = 17.5 Torr
Total pressure = Vapor pressure of water + Partial pressure of hydrogen gas
Partial pressure of hydrogen gas:
Total pressure - Vapor pressure of water
= 768.0 Torr - 17.5 Torr = 750.5 Torr = 0.987 atm
(1 Torr = 0.001315 atm)
Pressure of hydrogen gas =P = 0.986 atm
Temperature at which gas was collected ,T= 20°C = 293.15 K
Volume of the gas ,V= 75.3 mL = 0.0753 L
Moles of hydrogen gas = n
PV=nRT (An ideal gas equation)

0.003088 moles of hydrogen gas were formed .
Answer:
B
Explanation:
If someone was to call your picture calligraphy it mean beautiful graphics so theres your answer
M=43.2 g
v₁=63 ml
v₂=74 ml
p=m/v=m/(v₂-v₁)
p=43.2/(74-63)=3.927 g/ml
Yeast. Yeast causes the mixture with flour to become light and airy thus increasing size as temperature is applied.