What are the products in this chemical reaction?
1 answer:
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Answer:the pH is 12
Explanation:
First We need to understand the structure of trimethylamine
Due to the grades of the bond in the nitrogen with a hybridization sp3 is 108° approximately, then is generated a dipole magnetic at the upper side of the nitrogen, this dipole magnetic going to attract a hydrogen molecule of the water making the water more alkaline
C3H9N+ H2O --> C3H9NH + OH-
Then:
The concentration of the trimethylamine is 0.3 and the concentration of the ion C3H9NH is equal to the OH- relying on the stoichiometric equation. We could find the concentration of the OH- ion with the square root of the multiplication between k and the concentration of trimethylamine
[OH-]=
[OH-]=0.01
pH=14-(-log[OH-])
pH=12
Answer:
a) HCl is the limiting reagent.
b) Mass of NH₄Cl formed = 6.68 g
c) Pressure of the gas remaining in the flask = 1.742 atm
Explanation:
The complete Question is presented in the attached image to this solution.
To solve this question, we first need to obtain the limiting regaent for this reaction.
The limiting reagent is the reagent that is in short supply in the reaction and is used up in the reaction. It determines the amount of products that will be formed and the amount of other reactants that will be required for the reaction.
NH₃ (g) + HCl (g) ⟶ NH₄Cl (s)
1 mole of NH₃ reacts with 1 mole of HCl
we first convert the masses of the gases available to number of moles.
Number of moles = (Mass/Molar Mass)
Molar mass of NH₃ = 17.031 g/mol, Molar mass of HCl = 36.46 g/mol
Number of moles of NH₃ = (4.55/17.031) = 0.2672 mole
Number of moles of HCl = (4.55/36.46) = 0.1248 mole
Since 1 mole of NH₃ reacts with 1 mole of HCl
It is evident that HCl is in short supply and is the limiting reagent.
NH₃ is in excess.
So, to calculate the amount of NH₄Cl formed,
1 mole of HCl gives 1 mole of NH₄Cl
0.1248 mole of HCl will also gove 0.1248 mole of NH₄Cl
Mass (Number of moles) × (Molar Mass)
Molar mass of NH₄Cl = 53.491 g/mol
Mass of NH₄Cl formed = 0.1248 × 53.491 = 6.68 g
c) The gas remaining in the flask is NH₃
0.1248 mole of NH₃ is used up for the reaction, but 0.2672 mole was initially available for reaction,
The amount of NH₃ left in the reacting flask is then
0.2672 - 0.1248 = 0.1424 mole.
Using the ideal gas Equation, PV = nRT
We can obtain the rrequired pressure of the remaining gas in the flask
P = Pressure = ?
V = Volume = 2.00 L
n = number of moles = 0.1424 mole
R = molar gas constant = 0.08205 L.atm/mol.K
T = absolute temperature in Kelvin = 25 + 273.15 = 298.15 K
P = (nRT/V)
P = (0.1424×0.08205×298.15/2) = 1.742 atm
Hope this Helps!!!
