Answer: Hydrosphere, discontinuous layer of water at or near Earth's surface. It includes all liquid and frozen surface waters, groundwater held in soil and rock, and atmospheric water vapour. Earth's environmental spheresEarth's environment includes the atmosphere, the hydrosphere, the lithosphere, and the biosphere.
Explanation:
Answer:
<u>5 moles S x (36.02 g S/mole S) = 180.1 grams of S</u>
Explanation:
The periodic table has mass units for every element that can be correlated with the number of atoms of that element. The relationship is known as Avogadro's Number. This number, 6.02x
, is nicknamed the mole, which scientists found to be a lot more catchy, and easier to write than 6.02x. <u>The mole is correlated to the atomic mass of that element.</u> The atomic mass of sulfur, S, is 36.02 AMU, atomic mass units. <u>But it can also be read as 36.02 grams/mole.</u>
<u></u>
<u>This means that 36.02 grams of S contains 1 mole (6.02x</u><u>) of S atoms</u>.
<u></u>
This relationship holds for all the elements. Zinc, Zn, has an atomic mass of 65.38 AMU, so it has a "molar mass" of 65.38 grams/mole. ^5.38 grams of Zn contains 1 mole of Zn atoms.
And so on.
5.0 moles of Sulfur would therefore contain:
(5.0 moles S)*(36.02 grams/mole S) = <u>180.1 grams of S</u>
Note how the units cancel to leaves just grams. The units are extremely helpful in mole calculations to insure the correct mathematical operation is done. To find the number of moles in 70 g of S, for example, we would write:
(70g S)/(36.02 grams S/mole S) = 1.94 moles of S. [<u>Note how the units cancel to leave just moles</u>]
Answer:
is the symbol for an oxide ion
The following are the steps to complete and balnce the equation for the given reaction
<u>Explanation:</u>
We are given, NO2– is oxidized to NO3– and Ag is reduced to Ag
NO2– + Ag+ -----> NO3– + Ag(s)
Step 1) Assign the oxidation state to each element reaction
NO2– + Ag+ -----> NO3– + Ag(s)
N= +3 N = +5
O = -2 O = -2
Ag = +1 Ag = 0
NO2– -----> NO3– ………oxidation half reaction
Ag+ -----> Ag(s) ……….reduction half reaction
Step 2) Balance the element other than O and H
NO2– -----> NO3–
Ag+ -----> Ag(s)
Step 3) Balance the O by adding 1 H2O for 1 O
NO2– + H2O -----> NO3–
Ag+ -----> Ag(s)
Step 4) Balance the H by adding H+
NO2– + H2O -----> NO3– + 2H+
Ag+ -----> Ag(s)
Step 5) Balance the charge by adding electron
NO2– + H2O -----> NO3– + 2H+ + 2e-
Ag+ + 1e------> Ag(s)
Step 6) Balance the electron in both half reaction
NO2– + H2O -----> NO3– + 2H+ + 2e-
2 Ag+ + 2e------> 2 Ag(s)
Answer:
3.14
Explanation:
A student was comparing two samples with an equal number of carbon atoms. One sample contained only Carbon-12 atoms. One sample contained only Carbon-14 atoms, which contain two more neutrons than Carbon-12 atoms. The student measured the mass of each sample and testing the reactivity of each sample.
Required:
What would best describe the results of the investigation?
