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3 years ago

The Law of Superposition is most relevant when studying which type of rock?

Chemistry

2 answers:

bagirrra123 [75]3 years ago

8 0

Answer:

igneous or metamorphic

Explanation:

Those two are sorta relvant

igomit [66]3 years ago

8 0

Answer:

Sedimentary

Explanation:

Sedimentary rock is formed when pieces of eroded earth are deposited in layers. These layers are piled upon one another, slowly pressed down into the earth, and pressurized to become rock. The Law of Superposition states that, of these layers, the younger are found on top of the older.

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During a period of discharge of a lead-acid battery, 405 g of Pb from the anode is converted into PbSO4 (s).

Alexus [3.1K]

Answer:

The answers to the question are as follows

First part

The mass of PbO2 (s) reduced at the cathode during the period is = 467.55_g

Second part

The electrical charge are transferred from Pb to PbO2 is 377186.86_C or 3.909 F

Explanation:

To solve this, we write the equation for the discharge of the lead acid battery as

H₂SO₄ → H⁺ + HSO₄⁻

Pb (s) + HSO⁻₄ → PbSO₄ + H⁺ + 2e⁻

at the cathode we have

PbO₂ + 3H⁺ + HSO⁻₄ + 2e⁻ → PbSO₄ + 2H₂O

Summing the two equation or the total equation for discharge is

Pb (s) + PbO₂ + 2H₂SO₄ → 2PbSO₄ + 2H₂O

From the above one mole of lead and one mole of PbO₂ are consumed simultaneously hence

Number of moles of lead contained in 405 g of Pb with molar mass = 207.2 g/mole = (405 g)/ (207.2 g/mole) = 1.95 mole of Pb

Hence number of moles of PbO₂ reduced at the cathode = 1.95 mole

mass of PbO₂ reduced at the cathode = (number of moles)×(molar mass)

= 1.95 mole × 239.2 g/mol = 467.55 g of Lead (IV) Oxide is reduced at the cathode

Part B

Each mole of Pb transfers 2e⁻ or 2 electrons, therefore 1.95 moles of Pb will transfer 2 × 1.95 = 3.909 moles of electrons transferred

Each electron carries a charge equal to -1.602 × 10⁻¹⁹ C or one mole of electrons carry a charge equal to 96,485.33 coulombs

hence 3.909 moles carries a charge = 3.909 × 96,485.33 coulombs =377186.86 Coulombs of electrical charge

or transferred electrical charge = 377186.86 C or 3.909 Faraday

6 0

3 years ago

What is the difference between an atom and a compound?

puteri [66]

An atom cannot be broken down any smaller whereas a compound is made up of atoms and can be broken down into smaller pieces (the individual atoms that make it up)
Hope this helps!

6 0

4 years ago

Read 2 more answers

a 9.84 ounces ingot of unknown metal is heated from 73.2 degrees fahrenheit - 191.2 degrees fahrenheit this requires 3.912 calor

Gekata [30.6K]

The SI unit of specific heat is J per gram per degree Celsius. Thus it follows that specific heat could be calculated in this way:

Specific Heat = Energy / (mass x change in temperature)

Thus,

Specific Heat = 3.912 cal / (9.84 oz x (191.2 ˚F – 73.2 ˚F))

Specific Heat = 3.369 x 10^-3 cal/oz-˚F

6 0

4 years ago

What types of reactions are these 3 chemical equations?-

IceJOKER [234]

Answer:

*2Kl+Pb(NO3)2=PbI2+2KNO3: double replacement.

*2Al+3CuSO4=Al2(SO4)3+3Cu: single replacement.

*C2H5OH+3O2=2CO2+3H2O: combustion.

Explanation:

Hello there!

In this case, according to the required, it turns out necessary for us to recall the five types of reactions, combination, decomposition, single and double replacement and combustion as shown on the attached figure.

In such a way, since the first reaction follows the pattern AB+CD-->AD+CB we infer it is double replacement; the second reaction follows the patter A+BC-->AC+B and therefore it is single replacement; and the last one follows the pattern of combustion reaction due to the presence of CO2 and H2O on the products side.

Regards!

3 0

3 years ago

can someone explain in detail how molar mass, Avogadro's number, and volume are all connected through moles? Im so confused :(

sashaice [31]

Answer:

See Explanation

Explanation:

By definition, 1 mole is the mass of substance (or, formula mass in grams) containing 1 Avogadro's Number (N₀ = 6.02 x 10²³) of particles. That is ...

1 mole of hydrogen atoms (H) = 1.00794 grams

1 mole of molecular hydrogen (H₂) = 2.01588 grams

1 mole of any substance = 1 formula weight in grams

1 mole = 1 Avogadro's Number (N₀) = 1 formula weight in grams

In the concept of 'gas laws' 1 mole of any (all) gas at STP conditions ( => 0°C & 1 atmosphere pressure) occupies 22.4 Liters & is known as the 'molar volume' of a gas at STP. If the temperature &/or pressure change the volume will not be 22.4 Liters.

For reactions whose coefficients are balanced to the lowest whole number values (i.e., no fractional coefficients) the equation is known as the 'standard reaction' and conditions are assumed to be STP and the coefficients of gas phase components indicate molar volumes. Example ...

Given N₂(g) + 3H₂(g) => 2NH₃(g) is assumed to be at 0°C; 1 Atm pressure.

Molecular Nitrogen = 1 molar volume = 22.4 Liters of N₂(g)

Molecular Hydrogen = 3 molar volumes = 3 x 22.4 Liters of H₂(g) = 67.2 Liters of H₂(g)

Molecular Ammonia = 2 molar volumes = 2 x 22.4 Liters of NH₃(g) = 44.8 Liters of NH₃

8 0

3 years ago