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.
Answer:
Anabolism builds complex molecules from simpler ones, while catabolism breaks large molecules into smaller ones.
Explanation:
Answer: Total pressure inside of a vessel is 0.908 atm
Explanation:
According to Dalton's law, the total pressure is the sum of individual partial pressures. exerted by each gas alone.
= partial pressure of nitrogen = 0.256 atm
= partial pressure of helium = 203 mm Hg = 0.267 atm (760mmHg=1atm)
= partial pressure of hydrogen =39.0 kPa = 0.385 atm (1kPa=0.00987 atm)
Thus 
=0.256atm+0.267atm+0.385atm =0.908atm
Thus total pressure (in atm) inside of a vessel is 0.908
Metals are the most abundant
Answer:
mass of acetone added:
w acetone = 21.676 g
Explanation:
decrease in vapor pressure:
∴ ΔP = - 1.576 KPa = Pa - P*a
∴ a: water (solvent)
∴ b: C3H6O (solute)
∴ P*a (65°C) = 25.022 KPa
⇒ ΔP/(- P*a) = Xb,l
⇒ Xb.l = - 1.576 KPa/(- 25.022 KPa) = 0.063
∴ Xb = nb/nt = nb/(na + nb) = (wb/Mb)/[(wa/Ma) + (wb/Mb)]
∴ Mb = 58.08 g/mol (molar mass acetone)
∴ Ma = 18.015 g/mol (molar mass water)
∴ wa = 100 g
⇒ 0.063 = (wb/58.08)/[(100/18.015) + (wb/58.08)]
⇒ (0.063)[(5.55 + (wb/58.08)] = wb/58.08
⇒ 0.3497 + 1.085 E-3wb = wb/58.08
⇒ 20.3106 + 0.063wb = wb
⇒ 20.3106 = wb - 0.063wb
⇒ 20.3106 = 0.937wb
⇒ 20.3106/0.937 = wb
⇒ 21.676 g = wb
