Answer:
0.75 moles
Explanation:
S2 + 2O2 = 2SO2
From the reaction above,
We see that number of moles attached to S2 is 1 and number of moles attached to SO2 is 2.
Since we want to find how many moles of S2 are needed to produce 1.50 moles of SO2 gas
The answer is gotten by proportion;
Number of moles = 1/2 × 1.5 = 0.75 moles
atomic mass=percentage of isotope a * mass of isotope a + percentage of isotope b * mass of isotope b+...+percentage of isotope n * mass of isotope n.
Data:
mass of isotope₁=267.8 u
percentage of isotope₁=90.3%
mass of isotope₂=270.9 u
percentage of isotope₂=9.7%
Therefore:
atomic mass=(0.903)(267.8 u)+(0.097)(270.9 u)=
=241.8234 u + 26.2773 u≈268.1 u
Answer: the mass atomic of this element would be 268.1 u
Answer:
4.56×10^-10
Explanation:
Co(OH)2(s)<------->Co^2+(aq) + 2OH^-(aq)
Co^2+(aq) + 6NH3(aq) ---------->[Co(NH3)6]^2+(aq)
Overall equation:
Co(OH)2(s)+ 6NH3(aq) ---------->[Co(NH3)6]^2+(aq) + 2OH^-(aq)
The increased solubility of the cobalt salt in the presence of ammonia is as a result of the formation of the hexammine cobalt II complex shown above.
Knet= Ksp×Kf
Ksp of Co(OH)2= 5.92 × 10^-15.
Kf= 7.7 x 10^4
Knet= 5.92 × 10^-15 × 7.7 x 10^4
Knet= 4.56×10^-10
Note Knet is the equilibrium constant of the overall reaction.
