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kicyunya [14]
2 years ago
11

How many moles in 200 grams of Br

Chemistry
1 answer:
saveliy_v [14]2 years ago
6 0
2.5030036043252 moles.
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(1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.233 M aqueous acetylsalicylic acid (aspiri
AveGali [126]

Complete Question

The complete question is shown on the first uploaded image

Answer:

 1)  The ionic equation is  

HC_9H_7O_4 + (C_2 H_5)_3 N -----> C_9H_7O_4^- + (C_2 H_5)_3 NH^-

2

  At equilibrium The  aniline will be  favored

3

The pH  of the solution is   pH  = 7.12

Explanation:

  From the question we are told that

      The concentration of aspirin is  C_A = 0.233M

      The acid dissociation  constant for aspirin is  K_a = 3.0*10^{-4}

       The base  dissociation constant for aniline is  K_b = 7.4 *10^{-10}

The molecular formula for aspirin  is  HC_9H_7O_4

The molecular formula for aniline  is   (C_2 H_5)_3 N

So the net ionic reaction is  

     HC_9H_7O_4 + (C_2 H_5)_3 N -----> C_9H_7O_4^- + (C_2 H_5)_3 NH^-

Generally pKa is mathematically evaluated as

                  pKa = -log(3.0*10^{-4})

                           = 3.52

Generally pKb is mathematically represented as

                  pKa = -log(7.4*10^{-10 })

                           = 9.13

Generally

                    pKa + pKb = 14

So for the triethylammonium salt  produced the pKa is

                  pK_a__{s}} = 14 - 3.28

                            = 10.72          

 As a result of the   pKa  of  aspirin being lower that that of  triethylammonium salt at equilibrium it implies that  aniline would be favored

The pH of the solution is mathematically represented as

           Since they are of equal mole

     pH  =  \frac{1}{2}  (pKa + pKb + pKw)

Where pKw is the pKw of water which has a value of 14

pH   =  0.5(14 + 3.52 + 3.28)

    pH  = 7.12

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Which half-reaction is most easily oxidized?
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From the ones that you are showing me <span>the more positive the potential the more likely: </span>

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If 8.500 g CH is burned and the heat produced from the burning is added to 5691 g of water at 21 °C, what is the final
mojhsa [17]

The final temperature = 36 °C

<h3>Further explanation</h3>

The balanced combustion reaction for C₆H₆

2C₆H₆(l)+15O₂(g)⇒ 12CO₂(g)+6H₂O(l)  +6542 kJ

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mol C₆H₆ :

\tt \dfrac{8.5}{78.11}=0.109

Heat released for 2 mol C₆H₆ =6542 kJ, so for 1 mol

\tt \dfrac{0.109}{2}\times 6542=356.539~kJ/mol

Heat transferred to water :

Q=m.c.ΔT

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If the ball rolls down the hill, potential energy decreases while kinetic increases.

simple example
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