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alex41 [277]
3 years ago
9

A food processing plant discharges 40 cfs (cubic feet per second) of process water containing an ultimate BOD (L0) of 25 mg/L an

d a DO concentration of 1.8 mg/L into a river that has a flow rate of 260 cfs and a velocity of 1.1 ft/s. Just upstream of the release point, the river has an ultimate BOD of 3.6 mg/L and a DO of 7.6 mg/L. The saturation value of DO in the river is 8.5 mg/L. The deoxygenation coefficient in the river (kd) is 0.61/day and the reaeration coefficient for the river (kr) is 0.76/day. Assume complete and instantaneous mixing of the process water and the river water.
Required:
a. What are the initial oxygen deficit and ultimate BOD concentration just downstream of the outfall?
b. What are the time and distance downstream to the minimum DO concentration?
c. What DO concentration could be expected 10 miles downstream?
Chemistry
1 answer:
Feliz [49]3 years ago
8 0

Answer:

The right solution according to the question is provided below.

Explanation:

According to the question,

(a)

The initial conditions will be:

DO = \frac{(40\times 1.8)+(260\times 7.6)}{40+260}

      = \frac{2048}{300}

      = 6.826 \ mg/L

The initial oxygen defict will be:

Do = 8.5-6.826

     = 1.674 \ mg/L

The initial BOD will be:

Lo = \frac{(40\times 25)+(260\times 3.6)}{40+260}

    = \frac{1936}{300}

    = 6.453 \ mg/L

(b)

The time reach minimum DO:

tc = \frac{1}{(kr-kd)} ln{(\frac{0.76}{0.61} )[1-\frac{1.674(0.76-0.61)}{0.61\times 6.453} ]}

   = \frac{1}{0.15}\times ln \ 1.158

By putting the values of log, we get

   = 0.973 \ days

The distance to reach minimum DO will be:

Xc = \frac{1.1\times 3600\times 24}{5280}\times 0.973 \ days

    = 18\times 0.973

    = 17.5 \ miles

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Come up with a three-step plan for your household to reduce its effect on water pollution. Your plan should include a way to edu
Marina86 [1]

Answer:

1 tell your family difrent ways to safe water

2 dont leave the water running when you brush your teeth

3 dont dump cups of water out for no reason

Explanation:

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In the Alkali metals what element is the same "Period" as the element Neon
Slav-nsk [51]

Answer:

Lithium

Explanation:

The answer is Lithium because the Alkali metals family is in the group 1A and the element neon is in the second period. If you look at the periodic table group 1A and the second period connects at the element Lithium.

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4 years ago
Using the following reaction (depicted using molecular models), large quantities of ammonia are burned in the presence of a plat
Mila [183]

Answer:

17.65 grams of O2 are needed for a complete reaction.

Explanation:

You know the reaction:

4 NH₃ + 5 O₂ --------> 4 NO + 6 H₂O

First you must know the mass that reacts by stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction). For that you must first know the reacting mass of each compound. You know the values ​​of the atomic mass of each element that form the compounds:

  • N: 14 g/mol
  • H: 1 g/mol
  • O: 16 g/mol

So, the molar mass of the compounds in the reaction is:

  • NH₃: 14 g/mol + 3*1 g/mol= 17 g/mol
  • O₂: 2*16 g/mol= 32 g/mol
  • NO: 14 g/mol + 16 g/mol= 30 g/mol
  • H₂O: 2*1 g/mol + 16 g/mol= 18 g/mol

By stoichiometry, they react and occur in moles:

  • NH₃: 4 moles
  • O₂: 5 moles
  • NO: 4 moles
  • H₂O: 6 moles

Then in mass, by stoichiomatry they react and occur:

  • NH₃: 4 moles*17 g/mol= 68 g
  • O₂: 5 moles*32 g/mol= 160 g
  • NO: 4 moles*30 g/mol= 120 g
  • H₂O: 6 moles*18 g/mol= 108 g

Now to calculate the necessary mass of O₂ for a complete reaction, the rule of three is applied as follows: if by stoichiometry 68 g of NH₃ react with 160 g of O₂, 7.5 g of NH₃ with how many grams of O₂ will it react?

mass of O_{2} =\frac{7.5 g of NH_{3} * 160 g of O_{2} }{68 g of NH_{3} }

mass of O₂≅17.65 g

<u><em>17.65 grams of O2 are needed for a complete reaction.</em></u>

3 0
3 years ago
19) What is the molarity of a KOH solution if 200 ml of the solution contains 0.6 moles KOH?
zloy xaker [14]

Answer: 3M

Explanation: Molarity : It is defined as the number of moles of solute present in one liter of solution.

Formula used :

Molarity=\frac{n\times 1000}{V_s}

where,

n = moles of solute KOH = 0.6 moles

V_s = volume of solution in ml= 200 ml

Now put all the given values in the formula of molarity, we get

Molarity=\frac{0.6moles\times 1000}{200ml}=3mole/L

Therefore, the molarity of solution will be 3M.

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3 years ago
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Iron and vanadium both have the BCC crystal structure and V forms a substitutional solid solution in Fe for concentrations up to
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Answer:

Explanation:

To find the concentration; let's first compute the average density and the average atomic weight.

For the average density \rho_{avg}; we have:

\rho_{avg} = \dfrac{100}{ \dfrac{C_{Fe} }{\rho_{Fe}} + \dfrac{C_v}{\rho_v} }

The average atomic weight is:

A_{avg} = \dfrac{100}{ \dfrac{C_{Fe} }{A_{Fe}} + \dfrac{C_v}{A_v} }

So; in terms of vanadium, the Concentration of iron is:

C_{Fe} = 100 - C_v

From a unit cell volume V_c

V_c = \dfrac{n A_{avc}}{\rho_{avc} N_A}

where;

N_A = number of Avogadro constant.

SO; replacing V_c with a^3 ; \rho_{avg} with \dfrac{100}{ \dfrac{C_{Fe} }{\rho_{Fe}} + \dfrac{C_v}{\rho_v} } ; A_{avg} with \dfrac{100}{ \dfrac{C_{Fe} }{A_{Fe}} + \dfrac{C_v}{A_v} } and

C_{Fe} with 100-C_v

Then:

a^3 = \dfrac   { n \Big (\dfrac{100}{[(100-C_v)/A_{Fe} ] + [C_v/A_v]} \Big) }    {N_A\Big (\dfrac{100}{[(100-C_v)/\rho_{Fe} ] + [C_v/\rho_v]} \Big)  }

a^3 = \dfrac   { n \Big (\dfrac{100 \times A_{Fe} \times A_v}{[(100-C_v)A_{v} ] + [C_v/A_Fe]} \Big) }    {N_A  \Big (\dfrac{100 \times \rho_{Fe} \times  \rho_v }{[(100-C_v)/\rho_{v} ] + [C_v \rho_{Fe}]} \Big)  }

a^3 = \dfrac   { n \Big (\dfrac{100 \times A_{Fe} \times A_v}{[(100A_{v}-C_vA_{v}) ] + [C_vA_Fe]} \Big) }    {N_A  \Big (\dfrac{100 \times \rho_{Fe} \times  \rho_v }{[(100\rho_{v} - C_v \rho_{v}) ] + [C_v \rho_{Fe}]} \Big)  }

Replacing the values; we have:

(0.289 \times 10^{-7} \ cm)^3 = \dfrac{2 \ atoms/unit \ cell}{6.023 \times 10^{23}} \dfrac{ \dfrac{100 (50.94 \g/mol) (55.84(g/mol)} { 100(50.94 \ g/mol) - C_v(50.94 \ g/mol) + C_v (55.84 \ g/mol)   }   }{ \dfrac{100 (7.84 \ g/cm^3) (6.0 \ g/cm^3 } { 100(6.0 \ g/cm^3) - C_v(6.0 \ g/cm^3) + C_v (7.84 \ g/cm^3)   } }

2.41 \times 10^{-23} = \dfrac{2}{6.023 \times 10^{23} }  \dfrac{ \dfrac{100 *50*55.84}{100*50.94 -50.94 C_v +55.84 C_v} }{\dfrac{100 * 7.84 *6}{600-6C_v +7.84 C_v} }

2.41 \times 10^{-23} (\dfrac{4704}{600+1.84 C_v})=3.2 \times 10^{-24} ( \dfrac{284448.96}{5094 +4.9 C_v})

\mathbf{C_v = 9.1 \ wt\%}

4 0
3 years ago
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