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d1i1m1o1n [39]
3 years ago
7

An important reaction sequence in the industrial production of nitric acid is the following: N2(g) + 3H2(g) → 2NH3(g) 4NH3(g) +

5O2(g) → 4NO(g) + 6H2O(l) Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?
Chemistry
1 answer:
frutty [35]3 years ago
3 0

Answer:

The answer to your question is 50 moles of O₂

Explanation:

Balanced Chemical reactions

1.-                 N₂(g)  +  3H₂ (g)   ⇒   2NH₃ (g)

2.-                4NH₃ (g) + 5O₂(g)  ⇒  4NO (g)  +  6H₂O (l)

moles of N₂(g) = 20 moles

moles of O₂(g) = ?

Process

1.- Calculate the moles of NH₃

                     1 mol of N₂ ------------- 2 moles of NH₃

                   20 moles of N₂ ---------  x

                     x = (20 x 2) / 1

                     x = 40 moles of NH₃

2.- Calculate the moles of O₂

                4 moles of NH₃ -------------- 5 O₂

               40 moles of NH₃ ------------  x

                    x = (40 x 5) / 4

                    x = 200 / 4

                    x = 50 moles of O₂

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Calculate the change in pH when 71.0 mL of a 0.760 M solution of NaOH is added to 1.00 L of a solution that is 1.0O M in sodium
Eddi Din [679]

Explanation:

It is known that pK_{a} value of acetic acid is 4.74. And, relation between pH and pK_{a} is as follows.

                    pH = pK_{a} + log \frac{[CH_{3}COOH]}{[CH_{3}COONa]}

                          = 4.74 + log \frac{1.00}{1.00}

So, number of moles of NaOH = Volume × Molarity

                                                   = 71.0 ml × 0.760 M

                                                    = 0.05396 mol

Also, moles of  CH_{3}COOH = moles of CH_{3}COONa

                                          = Molarity × Volume

                                          = 1.00 M × 1.00 L

                                          = 1.00 mol

Hence, addition of sodium acetate in NaOH will lead to the formation of acetic acid as follows.

            CH_{3}COONa + NaOH \rightarrow CH_{3}COOH

Initial :    1.00 mol                                  1.00 mol

NaoH addition:               0.05396 mol

Equilibrium : (1 - 0.05396 mol)    0           (1.00 + 0.05396 mol)

                    = 0.94604 mol                       = 1.05396 mol

As, pH = pK_{a} + log \frac{[CH_{3}COONa]}{[CH_{3}COOH]}

               = 4.74 +  log \frac{0.94604}{1.05396}

               = 4.69

Therefore, change in pH will be calculated as follows.

                         pH = 4.74 - 4.69

                               = 0.05

Thus, we can conclude that change in pH of the given solution is 0.05.

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