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enot [183]
3 years ago
6

Identify the benefits and limitations of models

Chemistry
1 answer:
Leona [35]3 years ago
8 0

Answer:

benefits

1. easier to use

2. save to use

3. saves money

4. helps you picture things in your mind

limitations

1. cannot include all the details

2. models do not behave exactly like the things they represent

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For the following systems at equilibrium
inna [77]

Answer:

1. CaCO3(s) <=> CaO(s) +CO2 (g) Delta H = +178 kJ/mol

Since Delta H is positive, it means the reaction is endothermic

a. An increase in temperature will will shift the equilibrium position to the right, thus forming more products

b. A decrease in the temperature will shift the equilibrium position to the left, thus forming more reactants

2. PCl3(g) + Cl2(g) <-> PCl5 (g) Delta H= -88 kJ/mol

From the above, Delta H is negative which implies exothermic reaction.

c. Increasing the temperature will shift the equilibrium position to the left, thus forming more reactants.

d. Decreasing the temperature will shift the equilibrium position to the right, thus forming more products

7 0
4 years ago
HELP ASAP, PLEASE!
algol13
A) James Cook.
B) He put his sailors on a strict diet to see if they would get scurvy.
C) Sauerkraut.
D) He told others of this diet and that none of his sailors died of scurvy.
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7 0
3 years ago
A sample of glucose ( C6H12O6 ) of mass 8.44 grams is dissolved in 2.11 kg water. What is the freezing point of this solution? T
zhuklara [117]

Answer:

- 0.0413°C ≅ - 0.041°C (nearest thousands).

Explanation:

  • Adding solute to water causes the depression of the freezing point.

  • We have the relation:

<em>ΔTf = Kf.m,</em>

Where,

ΔTf is the change in the freezing point.

Kf is the freezing point depression constant (Kf = 1.86 °C/m).

m is the molality of the solution.

<em>Molality is the no. of moles of solute per kg of the solution.</em>

  • <em>no. of moles of solute (glucose) = mass/molar mass</em> = (8.44 g)/(180.156 g/mol) = <em>0.04685 mol.</em>

<em>∴ molality (m) = no. of moles of solute/kg of solvent</em> = (0.04685 mol)/(2.11 kg) = <em>0.0222 m.</em>

∴ ΔTf = Kf.m = (1.86 °C/m)(0.0222 m) = 0.0413°C.

<em>∴ The freezing point of the solution = the freezing point of water - ΔTf </em>= 0.0°C - 0.0413°C = <em>- 0.0413°C ≅ - 0.041°C (nearest thousands).</em>

4 0
3 years ago
Lily took 57 seconds to walk from classroom to library. If the distance between the classroom and library was 38 m, at what aver
slamgirl [31]
1.5 sorry if I’m wrong!
4 0
3 years ago
A solution of methanol and water has a mole fraction of water of 0.312 and a total vapor pressure of 211 torr at 39.9 ºC. The va
r-ruslan [8.4K]

Answer:

The solution is not ideal.

The relative strengths of the solute-solvent interactions are greater  compared to the solute-solute and solvent-solvent interactions

Explanation:

The total vapor pressure is the sum of the partial pressures of  water and methanol, and they are calculated by the Raoult´s law equation:

Pₐ = Xₐ Pºₐ, where  Pₐ is the partial pressure of component A

                              Xₐ is the molar fraction of A

                              P⁰ₐ is the pressure of pure A

So lets calculate the partial pressures of methanol and water and compare them with the given total vapor pressure of solution:

X H2O = 0.312 ⇒ X CH3OH = 1 - 0.312 = 0.688

PH2O = 0.312 x 55.3 torr =  17.3 torr

PCH3OH = 0.688 x 256 torr = 176.1 torr

Ptotal = PH2O  + PCH3OH  = 17.3 torr + 176.1 torr = 193.4 torr

This pressure is less than the experimental value of 211 torr. So the solution is not ideal. The relative strength of the solute-solvent interactions are greater than the solute-solute and solvent-solvent interactions.

The reason for this is the presence of hydrogen bonding between methanol and water.

6 0
4 years ago
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