A solution can exist in three phases: solid, liquid and gas, depending on the temperature and pressure. The pH of the solution can also change based on the nature of ions present in it. Understanding the nature and properties of solutions is crucial for many chemical reaction processes.
A solution can exist in three phases depending on the temperature and pressure, which are: gas, liquid, and solid. These are depicted in a phase diagram (an illustrative depiction that shows the states of a substance under different conditions of temperature and pressure).Consider the phase diagrams for a pure solvent and a solution. When a nonvolatile solute is dissolved in a solvent, a solution is formed. These states coexist and are in a state of thermal equilibrium at specific combinations of pressures and temperatures.
In addition to the physical phase, the pH of the solution can also be considered as a 'phase.' The pH can decrease, increase, or even show a pattern of increase and then decrease depending on the nature of ions present in the solution.
Solutions are crucial to life-sustaining processes as well as other chemical reaction processes. It's important to know the nature of solutions and factors determining its formation and properties for understanding various biological, geological and industrial processes.
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B. Electrons have a negative charge.
C. An atom is made up of mostly empty space.
D. There is a dense area within an atom that has a negative charge.
Answer: C
Explanation:
Rutherford's Gold Foil Experiment
These were his conclusions.
Answer: Acid rain is caused by a chemical reaction that begins when compounds such as sulphur dioxide and oxides of nitrogen are released into the air. These substances can rise very high up into the atmosphere, where they mix and react with water, oxygen, and other chemicals to form more acidic pollutants called acid rain.
Explanation:
Answer: Option (c) is the correct answer.
Explanation:
According to Le Chatelier's principle, when a system is in equilibrium for a long time then it will change its concentration, temperature, volume or pressure to attain a new equilibrium that partly counteracts the applied change.
Since it is given that reaction is exothermic therefore, according to Le Chatelier's principle increase in temperature will be opposed so that reaction can proceed in the forward direction. Therefore, temperature has to be decreased to carry the reaction in forward direction.
Whereas pressure has to be increased so that reaction will shift to the forward side where there are less number of molecules.
Thus, we can conclude that to increase the yield of the products for the given reaction decrease the temperature and increase the pressure.