Answer:
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Answer:
30 g of magnesium would be combined with 20 g of oxygen. The law used solving this problem is the Lavoisier Law of conservation of mass.
Explanation:
If 60 g of magnesium combines with 40 g of oxygen to make 100 g of magnesium oxide, then 30 g of magnesium will combine with 20 g of oxygen to make 50 g of magnesium oxide.
This happens because in a chemical reaction there is no creation or descruction of atoms, only a rearrangement. Therefore, the mass of reactants should be equal to the mass of products.
The following equation represents the proportions of the substances:
Mg + 1/2O₂ → MgO
Answer:
Explanation:
Moles of
= 1 mole
Moles of
= 1 mole
Volume of solution = 1 L
Initial concentration of
= 1 M
Initial concentration of
= 1 M
The given balanced equilibrium reaction is,

Initial conc. 1 M 0M 1 M
At eqm. conc. (1-2x) M (2x) M (1+x) M
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{[NO]^2[Cl_2]}{[NOCl]^2}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BNO%5D%5E2%5BCl_2%5D%7D%7B%5BNOCl%5D%5E2%7D)
The
= 
Now put all the given values in this expression, we get :

By solving the term 'x', we get :

Concentration of
at equilibrium= (2x) M =
Answer:
The volume for the ideal gas is: 4647.5 Liters
Explanation:
Formula for the Ideal Gases Law must be applied to solve this question:
P . V = n . R . T
We convert the T° to K → 100°C + 273 = 373 K
We convert pressure value from kPa to atm.
2 kPa . 1atm/101.3 kPa = 0.0197 atm
We replace data in the formula.
V = ( n . R . T) / P → (3 mol . 0.082 . 373K) / 0.0197 atm =
The volume for the ideal gas is: 4647.5 Liters