Answer:
Mass = 114.26 g
Explanation:
Given data:
Number of gold atoms = 3.47×10²³ atoms
Mass in gram = ?
Solution:
The given problem will solve by using Avogadro number.
It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance. The number 6.022 × 10²³ is called Avogadro number.
1 mole = 6.022 × 10²³ atoms
3.47×10²³ atoms × 1 mol /6.022 × 10²³ atoms
0.58 mol
Mass of gold:
Mass = number of moles × molar mass
Mass = 0.58 mol × 197 g/mol
Mass = 114.26 g
Answer:
It may be too late, but you got lost in all that info. All they want is for you to show how many moles in 3.00 grams of Tin metal.
Explanation: I cannot print the dimensional analysis that is asked for, but we can do this.
Let’s use water instead of Tin, then you can figure it out. 1 mole of water is 2 H x 1 amu. 1 O at 16 amu. Forget the amu, just add the 16 + 2= 18 grams of Water In 1 mole. So 9 grams would be how many moles of water? 9 is 1/2 of 18 isn’t it? So it is 0.5 Moles.
1.Electrons can be transferred from one atom to another.
2.Electrons can be shared between neighbouring atoms.
3.Electrons can be shared with all atoms in a material.
Answer:
S + 4 Cl2
Explanation:
Sulphur - S
1 mol of Sulphur = S
Chlorine = Cl2
4 moles of Chlorine = 4Cl2
4S + 2Cl2
Incorrect option
S + 4 Cl2
Correct option
S + 2Cl2
Incorrect option
S + Cl2
Incorrect option
Answer: Electrons must be heated to emitted light. When heat was added to the elements,the electrons absorbs the energy and moves to its excited state. Once the electronstarts to fall back to a lower orbit, it emits energy in the form of light. Thedifferent lights being emitted, depends on their wavelength
Explanation: I did the Quantization of Energy Lab