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.
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.
352.8
with this all you have to do is move the decimal point to the right 2 times.
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
![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](https://tex.z-dn.net/?f=K_c%3D%20%5Cfrac%7Bconcentration%5C%20of%5C%20the%5C%20products%7D%7Bconcentration%5C%20of%5C%20the%5C%20reactants%7D%5C%5CK_c%3D%5Cfrac%7B%5BPCl_3%5D%5BCl_2%5D%7D%7B%5BPCl_5%5D%7D%3D%5Cfrac%7B%280.100%29%280.100%29%7D%7B%280.200%29%7D%3D0.0500)