An inhibitor, which slows down the reaction enough to measure the release of gas.
Answer:
Explanation:
1. Calculate the mass of each element
2. Calculate the moles of each element
3. Calculate the molar ratios
Divide all moles by the smallest number of moles.
4. Round the ratios to the nearest integer
C:H = 1:2
5. Write the empirical formula
The empirical formula is
When pressure in a chemical reaction increases, the equilibrium will shift towards the side of the reaction with fewer moles of gas. When there is a decrease in pressure, the equilibrium will shift towards the side of the reaction with more moles of gas.Therefore; in this case; increased the Equilibrium will shift to the left and favor the reverse reaction. This is because the side of products has more moles compared to the side of reactants, thus increased in pressure will aid conversion of products to reactants.
Answer:
Answer in the attached file
Answer:
pH = 9,32
Explanation:
The compound with 2 ionizable groups has the following equilibriums:
H₂M ⇄ HM⁻ + H⁺ pka = 6,2
HM⁻ ⇄ M²⁻ + H⁺ pka = 9,5
The reaction of M²⁻ with HCl is:
M²⁻ + HCl → HM⁻ + Cl⁻
The moles of M²⁻ are:
0,100L×1,0M = 0,1moles
And moles of HCl are:
0,060L×1,0M = 0,06moles
That means that moles of M²⁻ will be 0,1-0,06 = 0,04mol and moles of HM⁻ will be the same than HCl, 0,06mol
Using Henderson-Hasselbalch formula:
pH = pka + log₁₀ [M²⁻] / [HM⁻]
Replacing:
pH = 9,5 + log₁₀ [0,04] / [0,06]
<em>pH = 9,32</em>
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I hope it helps!
