I’m assuming the top ruler has more measurement points, like more specific numbers. This would mean the top ruler is more reliable because you can be more specific with your measurements
Answer:
23.46 mmHg is the vapor pressure for the solution
Explanation:
To solve this problem we need to apply a colligative property, which is the lowering vapor pressure.
The formula for this is: P°- P' = P° . Xm
where P' is vapor pressure for solution and P°, vapor pressure for pure solvent.
Let's determine the Xm (mole fraction for solute)
We calculate the moles of the solute and the solvent and we sum each other:
Moles of solute: 60 g /342 g/mol = 0.175 moles of sucrose
Moles of solvent: 250 g / 18 g/mol = 13.8 moles of water
Total moles: 13.8 moles + 0.175 moles = 13.975 moles
Xm for solute: 0.175 moles / 13.975 moles = 0.0125
Let's replace data in the formula: 23.76 mmHg - P' = 23.76 mmHg . 0.0125
P' = - (23.76 mmHg . 0.0125 - 23.76 mmHg) → 23.46 mmHg
Answer
is: the molar mass of a covalent compound is 90.4 g/mol.
<span>
m(compound) = 0.486 g.
m(water) = 25 mL </span>· 1 g/mL = 25 g ÷ 1000 g/kg = 0.025 kg.<span>
ΔT = 0°C - (-0.40°C) = 0.40°C.</span>
Kf(H₂O) = 1.86°C/m.
M(compound) = Kf · m(compound<span>) /
m(water) · ΔT.
M</span>(compound)<span>= 1.86°C/m · 0.486 g /
(0.025 kg · 0.4°C).
M</span>(compound) = 90.4 g/mol.
The answer is 975S because u add all ofthem
