An empty erlenmeyer flask weighs 241.3 g. when filled with water (d = 1.00 g/cm3), the flask and its contents weigh 489.1 g. wha
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0.164 g/L is the density of a sample of 1.00 mole of at 793mmhg and -9.00 degrees celcius.
Density is the mass of a unit volume of a material substance. The formula for density is d = , where d is density, M is mass, and V is volume.
Given data:
n = 1.00 mole
P=793 mm hg =1.04342 atm
T=-9.00 degree celcius = -9.00 + 273= 264 K
V=?
Using Ideal Gas Law equation:
PV = n R T
R = gas constant = 0.082057 L-atm/(mol-K)
(1.04342 atm)(V) = 5 X 0.082057 L-atm/(mol-K) X 264 K
V = 103.67 Liters
Now calculate density:
Mole weight of = 1.00 mole
So, the mass of = 17.031 g
Density =
Density =
= 0.164 g/L
Hence, 0.164 g/L is the density of a sample of 1.00 mole of at 793mmhg and -9.00 degrees celcius.
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Answer:
76.0%
Explanation:
Let's consider the following reaction.
CaCO₃(s) ⇄ CaO(s) + CO₂(g)
At equilibrium, the equilibrium constant Kp is:
Kp = 1.16 = pCO₂ ⇒ pCO₂ = 1.16 atm
We can calculate the moles of CO₂ at equilibrium using the ideal gas equation.
From the balanced equation, we know that 1 mole of CO₂ is produced by 1 mole of CaCO₃. Taking into account that the molar mass of CaCO₃ is 100.09 g/mol, the mass of CaCO₃ that reacted is:
The percentage by mass of the CaCO₃ that reacted to reach equilibrium is: