Answer:
Explanation:
They are the gases that conform to gas laws under all conditions of temperature and pressure. They are the gases that conform precisely to the assumptions of kinetic theory. ideal gases according to the kinetic theory assumptions could have no significant volume and there is no attractive or repulsive forces between its particles. there is no gas for which these assumptions are true; an ideal gas does not exist. However, under many coditions of temperature and pressure real gases behave much like ideal gases. Real gases have volume and there are attractions between their particles. Because of these attractions, real gases can be solidified or condensed when compressed or cooled e.g. water vapor when cooled below 100 degrees celsius at standard atmospheric pressure can be condensed into liquid. other real gases behave like that but sometimes more pressure and less temperature is required.
Assumptions of kinetic theory:
- the volume of a single particle in gas is small compared to the overall volume of the gas.
- under pressure, the particles are compressed and come closer together.
- there are no attractice or repulsive forces between its particles so it can move freely
- it expand to take the shape and size of the container
- the particles of the gas move in straight path until they collide with the wall of the container or with each other
- the motion of the particles is rapid, random and constant
- the distance between the particles of gas is more than that between solids and liquids
Answer:
0.007 g of deprenyl dose is required fro the patient with body mass of 70 kilograms.
Explanation:
The dose for treating Parkinson’s disease = 100 μg/kg body weight
Mass of patient's body = 70 kg
Amount of dose of deprenyl required = 100 μg/kg × 70 kg = 7,000 μg
1 μg = 0.00001 g
7,000 μg = 7,000 × 0.000001 g = 0.007 g
0.007 g of deprenyl dose is required fro the patient with body mass of 70 kilograms.
Reactants are the starting Ingredients in a chemical reaction products are the end result.
Answer:
A: The amount of CaCO₃ decreases.
B: The amount of CaCO₃ increases.
Explanation:
To know how the system will proceed to reach equilibrium, we need to calculate the reaction quotient (Q) and compare it with the equilibrium constant (Kc).
Part A 15.0 g CaCO₃, 15.0 g CaO, and 4.25g CO₂
CaCO₃ and CaO are solids and they do not take part in Q nor Kc, so we will just calculate the concentration of CO₂.
Then,
Q = [CO₂] = 9.66 x 10⁻³
Q < Kc (0.0108), so the reaction will proceed to the right to achieve equilibrium, thus decreasing the amount of CaCO₃.
Part B 2.50 g CaCO₃, 25.0 g CaO, and 5.66g CO₂
Then,
Q = [CO₂] = 0.0129
Q > Kc, so the reaction will proceed to the left to achieve equilibrium, thus increasing the amount of CaCO₃.