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3 years ago

The middle ear converts sound from what into vibrations that can be sent through what?

Chemistry

1 answer:

Katarina [22]3 years ago

5 0

Answer:

Explanation:

Eardrum or tympanic membrane changes sound to vibration and pass through malleus, incus and stapes.

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which pair shares the same empirical formula. c2h2 and c6h6, c2h2 and c2h4, ch2 and c6h6, ch and c2h4

olasank [31]

Answer:

Answer: CH₃ and C₂H₆ have same empirical formula.

Explanation:

it just compares in that it its the same

7 0

3 years ago

What is the limiting reactant if 12 moles of p4 react with 15 moles of o2?.

brilliants [131]

Answer:

see explanation

Explanation:

To determine limiting reactant divide mole quantities of reactants by the respective coefficient in the balanced equation. The smaller value is the limiting reactant.

P₄ + 5O₂ => 2P₂O₅

12/1 = 12 15/5 = 3

O₂ is the limiting reactant. P₄ will be in excess when rxn stops.

4 0

2 years ago

How many mL of a stock solution of 2.00 M KNO3 are needed to prepare 100.0 mL of 0.15M KNO3? with work plz

Tatiana [17]

Using the law of dilution :

Mi x Vi = Mf x Vf

2.00 x Vi = 0.15 x 100.0

2.00 x Vi = 15

Vi = 15 / 2.00

Vi = 7.5 mL

hope this helps!

3 0

3 years ago

When calculating the equilibrium constant, aqueous solutes must be expressed in moles per liter (M), and gases must be expressed

alukav5142 [94]

Answer:

B. They are dimensionless ratios of the actual concentration or pressure divided by standard state concentration, which is 1 M for solutions and 1 bar for gases.

Explanation:

Activity of a substance is defined as the ratio of an effective concentration or an effective pressure to a standard state pressure or a standard state pressure. It is usually a unit less ratio.

Concentrations in an equilibrium constant are really dimensionless ratios of actual concentrations divided by standard state concentrations. Since standard states are 1 M for solutes, 1 bar for gases, and pure substances for solids and liquids, these are the units to be used.

Hence, activity is a fudge factor to ideal solutions that correct the true concentration. Activity of a gas and solute concentration is a ratio with no unit.

3 0

3 years ago

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring

Lady_Fox [76]

Answer:

The standard cell potential is 1.40 V. The correct option is the option D (+1.40 V)

Explanation:

Oxide-reduction reactions, also called redox, involve the transfer or transfer of electrons between two or more chemical species. In these reactions two substances interact: the reducing agent and the oxidizing agent.

An oxidizing element or oxidizing agent is one that reaches a stable energy state as a result of which the oxidant is reduced and gains electrons. The oxidizing agent causes oxidation of the reducing agent generating the loss of electrons of the substance and, therefore, oxidizes in the process.

In other words, the oxidizing agent is that chemical species that in a redox process accepts electrons released by the reducing agent and, therefore, is reduced in said process. The oxidizing agent is reduced because, upon receiving electrons from the reducing agent, a decrease in the value of the charge or oxidation number of one of the atoms of the oxidizing agent is induced .

Electrochemical cells, galvanic cells or batteries are called devices that are capable of transforming chemical energy originated in a spontaneous redox process into electrical energy.

The cellular potential is generally in standard conditions, that is, 1 M with respect to solute concentrations in solution and 1 atm for gases.

In this case you have the reaction:

3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq)

In this case the following half-reactions occur:

Semi-reaction of oxidation ( an atom or group of atoms loses electrons, or increases its positive charges): Fe³⁺(aq) + 3 e- -->Fe(s); E⁰ = -0.04 V

Semi-reaction of reduction (an atom or group of atoms gains electrons, increasing its negative charges): Cl₂(g) + 2 e- --> 2 Cl-(aq); E⁰=1.36 V

In an electrochemical cell at 25°C the potentials of the semi-reactions are usually measured in the sense of reduction and generally the standard potential between both electrochemical cells will be:

$E^{0} =E^{0} _{reduction} -E^{0} _{oxidation}$

E⁰=1.36 V - (-0.04 V)

E⁰=1.36 V + 0.04 V

E⁰=1.40 V

The standard cell potential is 1.40 V. The correct option is the option D (+1.40 V)

7 0

3 years ago