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2 years ago

Dead leaves on the forest floor become new soil through the actions of _____.

Chemistry

2 answers:

laila [671]2 years ago

5 0

I believe the answer is Decomposition. They become new soil through decomposers decomposing it, and making it soil.
~Silver

dmitriy555 [2]2 years ago

4 0

Decomposers break down different organic matter into the soil.

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1. Calculate the [H] in a solution that has a pH of 9.88.

Olenka [21]

The answer to the question is D.

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2 years ago

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What is the percent yield of O2 if 10.2 g of O2 is produced from the decomposition of 17.0 g of H2O?

yawa3891 [41]

The balanced chemical reaction will be:

2H2O = 2H2 + O2

We are given the amount of water used in the decomposition reaction. This will be our starting point.

17.0 g H2O (1 mol H2O/ 18.02 g H2O) (1 mol O2/2 mol H2O) ( 32.00 g O2/1mol O2) = 15.09 g O2

Percent yield = actual yield / theoretical yield x 100

Percent yield =10.2 g / 15.09 g x 100

Percent yield = 67.58%

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2 years ago

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What happens to these physical properties as the strength of intermolecular forces increases?Increase or decrease?a) melting poi

docker41 [41]

Boiling Point, Melting Point, Viscosity, Surface Tension. Decrease: Vapor Pressure.

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2 years ago

How many chlorine atoms are there in one molecule of PCI3

Darya [45]

Answer:

Chemical Formula:

For example- for every one mole of the compound PCl3 P C l 3 , it contains 3 moles of Chlorine atom and 1 mole of Phosphorus atom.

Explanation:

• Phosphorus trichloride (PCl3) contains three chlorine atoms and one phosphorus atoms.

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1 year ago

He molecular formula mass of this compound is 180 amu . what are the subscripts in the actual molecular formula?

mezya [45]

I can't actually answer this one if the empirical formula is not given. Luckily, I've found a similar problem from another website. The problem is shown in the picture attached. It shows that the empirical formula is CH₂O. Let's calculate the molar mass of the empirical formula.

Molar mass of E.F = 12 + 2(1) + 16 = 30 g/mol

Then, let's divide this to the molar mass of the molecular formula.
Molar mass of M.F/Molar mass of E.F = 180/30 = 6

Therefore, let's multiply 6 to each subscript in the empirical formula to determine the actual molecular formula.
Actual molecular formula = C₆H₁₂O₆

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2 years ago