<h3>
Answer:</h3>
Ba(NO₃)₂(aq) + CuSO₄(aq) ⟶ BaSO₄(s) + CU(NO₃)₂(aq)
2K₃PO₄(aq) + 3MgCl₂(aq) ⟶ 6KCl(aq) + Mg₃(PO₄)₂(s)
<h3>
Explanation:</h3>
- Precipitation reactions are types of reactions that involve a reaction between soluble salts to form an insoluble salt or a precipitate and a soluble salt.
- The equations given in the question are examples of precipitation reactions that lead to the formation of precipitates BaSO₄ and Mg₃(PO₄)₂
- The balanced equations are;
Ba(NO₃)₂(aq) + CuSO₄(aq) ⟶ BaSO₄(s) + CU(NO₃)₂(aq)
2K₃PO₄(aq) + 3MgCl₂(aq) ⟶ 6KCl(aq) + Mg₃(PO₄)₂(s)
- Based on solubility rules, all sulfates are soluble except CaSO₄, BaSO₄, PbSO₄ and silver sulfate. Therefore, BaSO₄ is a precipitate and will have a solid-state.
- All phosphates are insoluble except those of ammonium, potassium, and sodium. Therefore, Mg₃(PO₄)₂ is a precipitate and will have a soluble state.
Answer:
When the electrons hit the atoms in the chamber, they cause some of the electrons in the atoms to be stripped or knocked away. ... When one or more electrons is knocked off of an atom, it becomes positively charged. It is now an positive ion. A negative ion can be made by adding an electron to an atom.
Explanation:
C. They come from energy sources that never run out.
Carbon has four valence electrons. These electrons are associated for a specific atom and is responsible for forming a bond to different atoms. For carbon, in order to agree with the octet rule, it should have 4 more electrons. For an oxygen atom, there are 6 valence electrons present so it would need two more electrons. Thus, carbon atoms would share electrons with another two oxygen atoms wherein each oxygen atom would form double bonds with the carbon atom. So, the characteristics of these bonds would be that all of the four valence electrons of the carbon are being shared.
The student should set up an experiment in which he will require a crucible, a sample of hydrated copper sulfate (CuSO₄ <span>• 5H</span>₂O), a hot plate and a digital mass balance.
First, the student should check the mass of the empty crucible, then add the sample to the crucible and check the mass again. The difference is the mass of the sample.
Next, the student should place the crucible on a hot plate and begin heating the sample. After regular time intervals, such as two minutes, the students should measure the mass of the crucible and sample and note it down until it stops decreasing.
After a final mass of the sample has been obtained, the student may subtract this from the initial mass and find the mass of water evaporated.