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4 years ago

How does carbon enter soil?

2 answers:

6 0

Animals and plants get rid of carbon<span> dioxide gas through a process called respiration. </span>Carbon<span> moves from fossil fuels to the atmosphere when fuels are burned. When humans burn fossil fuels to power factories, power plants, cars and trucks, most of the </span>carbon<span> quickly </span>enters<span> the atmosphere as </span>carbon<span> dioxide gas. I hope this works!

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svet-max [94.6K]4 years ago

5 0

When something carbon based is in the soil. For example when you bury a cat or a body, it slowly decomposes, that carbon that was in the body gets absorbed by the soil. It goes back to the earth. That soil with "new" carbon is soil rich in nutrients etc. hope this helps

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An unknown triprotic acid (H3A) is titrated with NaOH. After the titration Ka1 is determined to be 0.0053 and Ka2 is determined

Savatey [412]

Answer:

Ka3 for the triprotic acid is 7.69*10^-11

Explanation:

Step 1: Data given

Ka1 = 0.0053

Ka2 = 1.5 * 10^-7

pH at the second equivalence point = 8.469

Step 2: Calculate Ka3

pKa = -log (Ka2) = 6.824

The pH at the second equivalence point (8.469) will be the average of pKa2 and pKa3. So,

8.469 = (6.824 + pKa3) / 2

pKa3 = 10.114

Ka3 = 10^-10.114 = 7.69*10^-11

Ka3 for the triprotic acid is 7.69*10^-11

6 0

3 years ago

If a chlor-alkali cell used a current of 3X10⁴A, how many pounds of Cl₂ would be produced in a typical 8-h operating day?

vova2212 [387]

7 × 10² pounds of Cl₂ would be produced in a typical 8-h operating day.

<h3>What is Stoichiometry ?</h3>

Stoichiometry helps us use the balanced chemical equation to measures quantitative relationships and it is to calculate the amount of products and reactants that are given in a reaction.

<h3>What is Balanced chemical equation ?</h3>

The balanced chemical equation is the equation in which the number of atoms on the reactants side is equal to the number of atoms on the product side in an equation.

2Cl⁻ (aq) → Cl (g) + 2e⁻

According to stoichiometry, moles of Cl₂

$= (3 \times 10^4\ A) \left (\frac{\frac{C}{s}}{A} \right ) \left (\frac{3600\ s}{h} \right ) (8h) \left (\frac{1\ \text{mol}\ e^{-}}{9.65 \times 10^4\ C} \right ) \left (\frac{1\ \text{mol}\ Cl_2}{2\ \text{mol}\ e^-} \right )$

= 4477 moles

Pounds Cl₂

$= (4477\ \text{moles}\ Cl_2) \left (\frac{70.90\ g\ Cl_2}{\text{mol}} \right ) \left (\frac{1\ kg}{1000\ g} \right ) \left (\frac{2.205\ lb}{1\ kg} \right )$

= 7 × 10² lb

Thus from the above conclusion we can say that 7 × 10² pounds of Cl₂ would be produced in a typical 8-h operating day.

Learn more about Stoichiometry here: brainly.com/question/14935523

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5 0

1 year ago

Assuming all the nh3 dissolves and that the volume of the solution remains at 0.300 l , calculate the ph of the resulting soluti

barxatty [35]

<span>Assume p=735 Torr V= 7.6L R=62.4 T= 295 PV-nRT (735 Torr)(7.60L)= n (62.4Torr-Litres/mole-K)(295K) 0.30346 moles of NH3 Find moles 0.300L solution of 0.300 M HCL = 0.120 moles of HCL 0.30346 moles of NH3 reacts with 0.120 moles of HCL producing 0.120 moles of NH4+ ION, and leaving 0.18346 mole sof NH3 behind Find molarity 0.120 moles of NH4+/0.300L = 0.400 M NH4+ 0.18346 moles of NH3/0.300L = 0.6115 M NH3 NH4OH --> NH4 & OH- Kb = [NH4+][OH]/[NH4OH] 1.8 e-5=[0.300][OH-]/[0.6115] [OH-]=1.6e-5 pOH= 4.79 PH=9.21 .</span>

3 0

3 years ago

What mass of H2 is needed to react with 8.5 g of O2 according to the following equation G plus O2 (G)plus H2 ( G)?

Rzqust [24]

The correct answer is number 1

5 0

3 years ago

How many moles of copper are needed to react with sulfur to produce 0.25 moles Ol

Tems11 [23]

Answer:

0.50 moles of Cu

Explanation:

The balanced chemical equation for given synthetic reaction is,

2 Cu + S → Cu₂S

According to balance chemical equation,

1 mole of Cu₂S is produced by = 2 moles of Cu

So,

0.25 moles of Cu₂S will be produced by = X moles of Cu

Solving for X,

X = 0.25 mol × 2 mol / 1 mol

X = 0.50 moles of Cu

Hence, as the molar ratio of Cu to Cu₂S is 2:1 hence, to produce 0.25 moles of Cu₂S we will need 0.50 moles of Cu.

6 0

3 years ago