Answer:
Kc = [H₂S]² . [CH₄] / [ H₂O]⁴ . [CS₂]
Explanation:
The equilibrium constant indicates the % of the yield reaction and can shows where the reaction is going to be equilibrated.
It works with molar concentrations on the equilibrium and it does not consider the solids compounds
Kc also can be modified by the time of the reaction.
This reaction is:
CS₂ (g) + 4 H₂O(g) ⇌ CH₄ (g) + 2H₂S (g)
Kc = [H₂S]² . [CH₄] / [ H₂O]⁴ . [CS₂]
71.8 g of iron (III) oxide (Fe₂O₃) were produced from 3 moles of magnesium oxide (MgO).
Explanation:
We have the following chemical reaction:
2 FeCl₃ + 3 MgO → Fe₂O₃ + 3 MgCl₂
We see from the chemical reaction that 3 moles of magnesium oxide (MgO) will produce 1 mole of iron (III) oxide (Fe₂O₃).
number of moles = mass / molar weight
mass = number of moles × molar weight
mass of Fe₂O₃ = 1 × 71.8 = 71.8 g
Learn more about:
number of moles
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Answer:
a) At a given temperature, C₂H₆ has a higher vapor pressure than C₄H₁₀.
Explanation:
<em>Which statement below is true?
</em>
<em>a) At a given temperature, C₂H₆ has a higher vapor pressure than C₄H₁₀. </em>TRUE. C₂H₆ has a lower molar mass than C₄H₁₀ and a higher vapor pressure at most temperatures.
<em>b) The strongest intermolecular attractive forces present in liquid CCl₄ are dipole-dipole forces.</em> FALSE. CCl₄ is nonpolar, so the strongest intermolecular forces are dispersion forces.
<em>c) HCl has a higher boiling point than LiCl.</em> FALSE. LiCl (ionic compound) has a higher boiling point than HCl (covalent compound).
<em>d) H₂O has a greater polarizability than H₂Se.</em> FALSE. Se has a larger atomic radius than O which is why H₂Se has a greater polarizability than H₂O.
<em>e) In general, the stronger the intermolecular attractive forces, the lower the ∆Hºvap.</em> FALSE. In general, the stronger the intermolecular attractive forces, the higher the ∆Hºvap.
Answer:
CuO + 2HCl = CuCl2(s) + H2O(l)
1 molecule of CuO reacts with 2 moles of HCl to form 1 mole of Copper II chloride and 1 mole of HCl
Here we have to get the correct molecular formula of the compound.
The molecular formula of the compound is C₆H₆O₆ i.e. option C.
Let assume, the empirical formula of the compound is 
.
The given molar mass of the compound is 176.124 g/mole.
The percent of carbon in the compound is 
×100 = 40.924.
The percent of hydrogen in the compound is 
×100 = 4.577.
The percent of oxygen in the compound is 
×100 = 54.498.
Now the ratio of the atomic number in the compound for carbon is 
= 3.410
Now the ratio of the atomic number in the compound for hydrogen is 
= 4.577
Now the ratio of the atomic number in the compound for oxygen is 
= 3.406
So, the C, H and O lowest ratio is 
= 1, 
= 1 and 
= 1
Thus the empirical formula of the compound is ![[CH_{1}O] _{n}](https://tex.z-dn.net/?f=%5BCH_%7B1%7DO%5D%20_%7Bn%7D)
(where n = integer.
12n + 1n + 16n = 176.24
29n = 176.24
n = 6 (approx)
Thus the molecular formula of the compound is C₆H₆O₆.
