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mezya [45]
4 years ago
6

A 1.0 liter container is filled with 0.300 M of

Chemistry
1 answer:
grandymaker [24]4 years ago
8 0
If there is 1.0 liters of 0.300 M at the beginning, that means there was 0.300 moles (because 1 L times 0.300 moles/L = 0.300 mol).  It says that, at equilibrium, there is 0.200 mol PCL5.  That means 0.100 mol PCl5 reacted.  Therefore, 0.100 mol each was created of PCl3 and Cl2.

Equilibrium constant Kc can be found with this:
K_c= \frac{concentration\ of\ the\ products}{concentration\ of\ the\ reactants}\\K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}=\frac{(0.100)(0.100)}{(0.200)}=0.0500

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Decide which of the following statements are true and which are false, concerning the kinetic molecular theory.
ElenaW [278]

Answer:

1. A. True

2. A. True

3. B. False

4. A. True

5. B. False

Explanation:

1. The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas. A. True. The pressure of an ideal gas is higher than the one that would exert a real gas.

2. The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other. A. True. The intermolecular forces are negligible.

3. The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be about 1 mL. B. False. The volume of the gas particles is negligible.

4. The molecules in a real gas have finite volumes and do exert forces on each other, thus real gases do not conform to some of the assumptions of an ideal gas as stated by the kinetic molecular theory. A. True. We cannot apply ideal gas laws to real gases.

5. The average kinetic energy of a collection of gas particles is assumed to be inversely proportional to the Kelvin temperature of the gas. B. False. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.

8 0
3 years ago
How many kilograms of a fertilizer are made of pure P2O5 would be required to supply 1.69 kilogram of phosphorus to the soil?
Alekssandra [29.7K]

Answer:

3.89 kg P2O5 must be used to supply 1.69 kg Phosphorus to the soil.

Explanation:

The molecular mass of P2O5 is

P2 = 2* 31 =           62

O5 = 5 *<u> 16 =         80</u>

Molecular Mass = 142

Set up a Proportion

142 grams P2O5 supplies 62 grams of phosphorus

x    kg P2O5        supplies 1.69 kg of phosphorus

Though this might be a bit anti intuitive, you don't have to convert the units for this question. The ratio is all that is important.

142/x = 62/1.69            Cross multiply

142 * 1.69 = 62x           combine the left

239.98 = 62x               Divide by 62

239.98/62 = x

3.89 kg of P2O5 must be used.

3 0
3 years ago
Round off or add zero to the following calculated answers to give a final answer with three significant figures: 3.528x10exponen
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352.8
with this all you have to do is move the decimal point to the right 2 times.
5 0
4 years ago
Find the density of an object that has mass of 5kg and a volume of 50cm3
wel

Answer:

100g/cm^3

Explanation:

density=mass/volume

convert mass in kg to g

1kg=1000g

5kg=5000g

therefore, density=5000g/50cm^3

=100g/cm^3

4 0
3 years ago
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