Hey! Let me help you!
C)
<span>What
additional volume of 10.0 M HCl would be needed to exhaust the
remaining capacity of the buffer after the reaction described in Part B?
In other words, how much more of this HCl solution is required to
consume the remaining Tris in the buffer?
let x = how much more solution needed
x = 1.8 mL <=========
Your answer is 1.8 mL as it is needed for more of this HCI solution is requires to consume the remaining Tris in the buffer!
Have an awesome day! :D
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R in the equation is a gas constant. It is .0821 liters x ATM over Moles x degrees kelvin.
Answer:
The equilibrium constant Kp = 29.68
Explanation:
2SO3(g) ⇄ 2SO2(g) + O2(g)
Kp = (pSO2)²(pO2)/(pSO3)²
We can use ideal gas formula to find pressure of each: PV = nRT thus P=nRT/V,
with n=moles at equilibrium; R=0.082057L.atm.mol⁻¹.K⁻¹ (gas constant); T=1.30*10^3K; V=13.2L
After substituting each values:
P(SO3) = 0.873 atm
P(SO2) = 3.15 atm
P(O2) = 2.28 atm
Kp = (3.15²×2.28)/(0.873)² = 29.68
Answer:
what is ionic? Is it iron
Explanation:
<span>Of all the sub-shells shown ( 1s ,2s ,2p ,3s ,3p ,4s ,3d ,4p ,5s ,4d ,5p ,6s ,4f ,5d) the ones that act as core orbital of HF (Hydrogen Fluoride) is 6s and 5d</span>