The number of moles left = 0.0067 moles
<h3>Further explanation</h3>
Given
0.28 g CO
2 x 10²¹ molecules removed
Required
Number of moles left
Solution
Initial mol of CO(MW=28 g/mol) :
mol = 0.28 : 28
mol = 0.01
The number of molecules in 0.01 mol :
= 0.01 x 6.02 x 10²³
= 6.02 x 10²¹
2 x 10²¹ molecules removed, so molecules left :
= 6.02 x 10²¹ - 2 x 10²¹
= 4.02 x 10²¹
moles of 4.02 x 10²¹ :
= 4.02 x 10²¹ : 6.02 x 10²³
= 0.0067 moles
There are 1739218 atoms in 2.5 mole of wolframite
Answer:
Mass = 255 g
Explanation:
Given data:
Number of moles of nitrogen = 7.5 mol
Mass of ammonia formed = ?
Solution:
Chemical equation:
3H₂ + N₂ → 2NH₃
Now we will compare the moles of nitrogen and ammonia.
N₂ : NH₃
1 : 2
7.5 : 2/1×7.5 = 15
Mass of ammonia:
Mass = number of moles × molar mass
Mass = 15 mol × 17 g/mol
Mass = 255 g
Answer:
If a sample of 2 moles of nitric oxide gas was reacted with excess oxygen, 2 moles of nitrogen dioxide would be produced.
Explanation:
The balanced reaction is:
2 NO + O₂ → 2 NO₂
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:
-
NO: 2 moles
- O₂: 1 mole
- NO₂: 2 moles
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop. By reaction stoichiometry, <u><em>
if a sample of 2 moles of nitric oxide gas was reacted with excess oxygen, 2 moles of nitrogen dioxide would be produced.
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