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Delvig [45]
3 years ago
11

Logging is a cause of nonpoint source pollution how does the removal of trees affect our fresh water supply

Chemistry
2 answers:
satela [25.4K]3 years ago
8 0
Logging may cause the soil to be less compact and the loose dirt will enter and contaminate any water source.


Have a nice day!
kenny6666 [7]3 years ago
7 0

Answer Choices :

A: The removal of trees does not affect our fresh water supply.

B: Tree roots actually help absorb some chemicals, which prevents them from entering our fresh water supply.

C: Fewer trees increases absorption of water and other chemicals into the groundwater supply.

D: Fewer trees increases erosion, which adds more sediment to our fresh water supply.

Now <u>Mr.Josh-Ray</u> Says<em> "Logging may cause the soil to be less compact and the loose dirt will enter and contaminate any water source."</em>

<u><em>Meaning </em></u><em>- The Loose Dirt Contains Particles Are Contaminating Clean Water Sources.</em>

<u><em>D</em></u> - Fewer trees increases erosion, which adds more sediment to our fresh water supply.

Therefore <em>Mr.Josh</em> Is <u>Correct</u>

<em>"</em><u><em>D</em></u><em>" IS CORRECT ON </em><u><em>PLATO</em></u><em>.</em>

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1 mole of any gas under STP  ----- 22.4 L

18.65 L*1 mol/22.4 L ≈ 0.8326 mol N2
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Which best describes the current atomic theory?
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Atoms are composed of electrons in a cloud around a positive nucleus.
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The second-order rate constants for the reaction of oxygen atoms witharomatic hydrocarbons have been measured (R. Atkinson and J
Pepsi [2]

Answer:

A = 1,13x10¹⁰

Ea = 16,7 kJ/mol

Explanation:

Using Arrhenius law:

ln k = -Ea/R × 1/T + ln(A)

You can graph ln rate constant in x vs 1/T in y to obtain slope: -Ea/R and intercept is ln(A).

Using the values you will obtain:

y = -2006,9 x +23,147

As R = 8,314472x10⁻³ kJ/molK:

-Ea/8,314472x10⁻³ kJ/molK = -2006,9 K⁻¹

<em>Ea = 16,7 kJ/mol</em>

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ln A = 23,147

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6 0
3 years ago
 
Mashutka [201]

sodium cloride is salt created from sodium Na and chlorine Ci

Na-sodium Ca- calcium

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Ca- calcium Br-bromine

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6 0
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A 2.350×10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then b
sveta [45]

Answer:

  • Part A: m = 0.02356 mol/kg = 0.02356 m
  • Part B: Xsolute = 4.243×10⁻⁴
  • Part C: % m/m = 0.1376%
  • Part D: ppm = 1,376 ppm

Explanation:

<u>1. Data:</u>

a) M = 2.350×10⁻² M

b) V sol = 1.000 L

c) V H₂O = 994.4 mL = 0.9944 L

d) d H₂O = 0.9982 g/mL

<u>2. Formulae</u>

  • M = n solute / V sol (L)
  • m = n solute / Kg solvent
  • X solute = n solute / N total
  • % m/m = (mass of solute / mass of solution) × 100
  • ppm = (mass of solute / mass of solution) × 1,000,000
  • density = mass in grams / volume in mL

<u>3. Solution</u>

<u>Part A: Calculate the molality of the salt solution. </u>

<u />

            m = n solute / Kg solvent

i) M = n solute / V sol (L) ⇒ n solute = M × V sol (L)

⇒ n solute = M = 2.350×10⁻² M × 1.000 L = M = 2.350×10⁻² mol

ii) density H₂O = mass H₂O / volume H₂O

⇒ mass H₂O = density H₂O × volume H₂O

⇒ mass H₂O = 0.9982 g/mL × 999.4 mL = 997.6 g

iii) kg  H₂O = 997.6 g / (1,000 g/Kg) = 0.9976 kg

iv) m = 2.350×10⁻² mol / 0.9976 kg = 0.02356 mol/kg = 0.02356 m

<u>Part B: Calculate the mole fraction of salt in this solution</u>.

          X solute = n solute / N total

i) n solute =  2.350×10⁻² mol

ii) n solvent = n H₂O = mass H₂O in grams/ molar mass H₂O

⇒ 997.6 g / 18.015 g/mol = 55.38 mol

iii) X solute = 2.350×10⁻² mol / 55.38 mol = 4.243×10⁻⁴

<u>Part C: Calculate the concentration of the salt solution in percent by mass</u>.

         % m/m = (mass of solute / mass of solution) × 100

i) molar mass = mass in grams / molar mass

⇒ mass of solute = mass of NaCl = n solute × molar mass NaCl

⇒ mass of solute = 2.350×10⁻² mol × 58.44 g/mol = 1.373 g

ii) % m/m = (1.373 g / 997.6 g) × 100 = 0.1376%

Part D: Calculate the concentration of the salt solution in parts per million.

       ppm = (mass of solute / mass of solution) × 1,000,000

i) ppm = ( (1.373 g / 997.6 g) × 1,000,000 = 1,376 ppm

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3 years ago
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