1) D = 13.6 g / mL
2)ethyl alcohol weighs 158g
3)ρ
_copper = 8.9 g
Explanation:
1)
D = m / V
=306.0 g / 22.5 mL
D= 13.6 g / mL
2)
density = mass / volume
mass = density × volume
=0.789g /ml × 200.0 ml
M=158g
Ethyl alcohol weighs 158g
3)
ρ (density) = Mass / Volume
ρ _copper = 1896 g / 8.4cm × 5.5cm × 4.6cm
= 1896g / 212.5
ρ
_copper=8.9 g
Answer: At equilibrium , there are 0.274 moles of
Explanation:
Moles of = 0.682 mole
Moles of = 0.440 mole
Volume of solution = 2.00 L
Initial concentration of =
Initial concentration of =
Equilibrium concentration of =
The given balanced equilibrium reaction is,
Initial conc. 0.341 M 0.220 M 0 M
At eqm. conc. (0.341-x) M (0.220-x) M (2x) M
Given : (0.341-x) M = 0.258 M
x= 0.083 M
Thus equilibrium concentartion of = (0.220-0.083) M = 0.137 M
Thus moles of at equilibrium =
At equilibrium , there are 0.274 moles of