Atoms are made up of protons , electrons and neutrons ..,, Atoms of the same element with different number of neutrons are called isotopes. Saying that substance “contains only one type of atom “ really means that it contains only atoms that all have the same number of protons .
Answer:
hi
Explanation:
The mass of the actual tin will remain constant; however I assume you are comparing the mass of the reactant, tin, with the mass of the products. The increase in mass stems from the oxides of tin present due to its reaction with oxygen in the air:
Sn(s) + O2(g) → SnO2(s)
By working out the atomic mass of the tin and the relative formula mass of tin oxide, you can see why there is a mass increase; 119:151. As you can see here, for every 119g of tin reacted, there will be 151g of tin oxide, hence why you think the mass of the tin increased (by 32g).
Hope this helped!
Answer:
It is composed of 57.17% S and 42.83% C and has a molar mass of 448.70 g/mol. Determine the empirical and molecular formulas of “sulflower.”
...
what is the molecular formula of the compound?
Empirical formula Molar mass (g/mol) Molecular formula
CHO 116.1
C8H16
Explanation:
Hope this helps
Answer:
71.372 g or 0.7 moles
Explanation:
We are given;
- Moles of Aluminium is 1.40 mol
- Moles of Oxygen 1.35 mol
We are required to determine the theoretical yield of Aluminium oxide
The equation for the reaction between Aluminium and Oxygen is given by;
4Al(s) + 3O₂(g) → 2Al₂O₃(s)
From the equation 4 moles Al reacts with 3 moles of oxygen to yield 2 moles of Aluminium oxide.
Therefore;
1.4 moles of Al will require 1.05 moles (1.4 × 3/4) of oxygen
1.35 moles of Oxygen will require 1.8 moles (1.35 × 4/3) of Aluminium
Therefore, Aluminium is the rate limiting reagent in the reaction while Oxygen is the excess reactant.
4 moles of aluminium reacts to generate 2 moles aluminium oxide.
Therefore;
Mole ratio Al : Al₂O₃ is 4 : 2
Thus;
Moles of Al₂O₃ = Moles of Al × 0.5
= 1.4 moles × 0.5
= 0.7 moles
But; 1 mole of Al₂O₃ = 101.96 g/mol
Thus;
Theoretical mass of Al₂O₃ = 0.7 moles × 101.96 g/mol
= 71.372 g
Answer:
used to complete the glicolisis process
Explanation:
A glucose molecule will generate the necessary energy to the body to compete their own metabolic processes.
At the begging of the process, the glucose change into 2 molecules of gliceraldehyde 3 - phosphate. In this first process the glucose molecule consume 2 molecules of ATP (the energetic molecule).
After this first process, the aldehyde turns into piruvate, during this process, there is produced 2 molecules of ATP, so it is producing chemical energy.
If during this process the cell need to enter into another metabolic process (pentose ways) then the gain of ATP deplets.
