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3 years ago

In a longitudinal wave moving along a spring, what are areas where the coils are farthest apart called?

Chemistry

2 answers:

Sholpan [36]3 years ago

7 0

Areas of rarefaction

Deffense [45]3 years ago

4 0

<h3>Answer;</h3>

Rarefactions

In a longitudinal wave moving along a spring, what are areas where the coils are farthest apart called Rarefactions.

<h3>Explanation;</h3>

A wave is a transmission of a disturbance from one point to another. It involves the transmission of energy from a source to other points.
Waves may classified as longitudinal waves or transverse waves depending on the vibration of particles relative to the wave motion.
Longitudinal waves are waves in which the vibration of particles is parallel to the direction of the wave motion, while transverse wave are types of waves in which the vibration of particles is perpendicular to the wave motion.
Longitudinal waves creates regions where particles are close together called compressions and regions where particles are farthest apart called rarefactions, while transverse waves creates regions of maximum displacement called crests and troughs.

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Name four main Homologous series in organic chemistry...... plz hlp me

Akimi4 [234]

I believe the four series you are looking for are straight-chain alkanes, alkenes, and alkynes, and cycloalkanes. These all have the same repeating of CH2 as the base group, while alkenes have a double bond somewhere in the molecule, and alkynes a triple somewhere.

8 0

3 years ago

How much energy is evolved during the reaction of 51.2 g of al, according to the reaction below? assume that there is excess fe2

sesenic [268]

Answer : The amount of energy evolved during the reaction is, $-807.696KJ$ .

Solution : Given,

$\Delta H=-852KJ$

Mass of Al = 51.2 g

Molar mass of Al = 27 g/mole

First we have to calculate the moles of Al.

$\text{ Moles of Al}=\frac{\text{ Mass of Al}}{\text{ Molar mass of Al}}=\frac{51.2g}{27g/mole}=1.896moles$

The balanced combustion reaction is,

$Fe_2O_3+2Al\rightarrow Al_2O_3+2Fe$

From the given reaction, we conclude that

As, 2 moles of Al evolved energy = $-852KJ$

So, 1.896 moles of Al evolved energy = $\frac{-852KJ}{2moles}\times 1.896moles=-807.696KJ$

Therefore, the amount of energy evolved during the reaction is, $-807.696KJ$ .

8 0

3 years ago

Calculate the vapor pressure (in torr) at 298 K in a solution prepared by dissolving 46.8 g of the non-volatile non-electrolye g

Rainbow [258]

Answer: The total partial pressure of the solution is 131.37 torr.

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

For glucose:

Given mass of glucose = 46.8 g

Molar mass of glucose = 180 g/mol

Plugging values in equation 1:

$\text{Moles of glucose}=\frac{46.8g}{180g/mol}=0.26 mol$

For methanol:

Given mass of methanol = 117 g

Molar mass of methanol = 32 g/mol

Plugging values in equation 1:

$\text{Moles of methanol}=\frac{117g}{32g/mol}=3.66 mol$

Mole fraction is defined as the moles of a component present in the total moles of a solution. It is given by the equation:

$\chi_A=\frac{n_A}{n_A+n_B}$ .....(2)

where n is the number of moles

Putting values in equation 2:

$\chi_{methanol}=\frac{3.66}{0.26+3.66}=0.934$

Raoult's law is the law used to calculate the partial pressure of the individual gases present in the mixture. The equation for Raoult's law follows:

$p_A=\chi_A\times p_T$ .....(3)

where $p_A$ is the partial pressure of component A in the mixture and $p_T$ is the total partial pressure of the mixture

We are given:

$p_{methanol}=122.7torr\\\chi_{methanol}=0.934$

Putting values in equation 3, we get:

$122.7torr=0.066\times p_T\\\\p_T=\frac{122.7torr}{0.934}=131.37torr$

Hence, the total partial pressure of the solution is 131.37 torr.

3 0

3 years ago

Why does liquids rate of evaporation increase when the liquid is heated

ivann1987 [24]

Boiling liquids that want to escape gas

4 0

3 years ago

Hydrogengasand oxygengas react to form water vapor. Suppose you have of and of in a reactor. Calculate the largest amount of tha

bezimeni [28]

The question is incomplete. The complete question is :

Hydrogen $(H_2)$ gas and oxygen $(O_2)$ gas react to form water vapor $(H_2O)$ . Suppose you have 11.0 mol of $H_2$ and 13.0 mol of $O_2$ in a reactor. Calculate the largest amount of $H_2O$ that could be produced. Round your answer to the nearest 0.1 mol .

Solution :

The balanced reaction for reaction is :

$2H_2(g) \ \ \ \ + \ \ \ \ \ O_2(g)\ \ \ \rightarrow \ \ \ \ 2H_2O(g)$

11.0 13.0

11/2 13/1 (dividing by the co-efficient)

6.5 mol 13 mol (minimum is limiting reagent as it is completely consumed during the reaction)

Therefore, $H_2$ is limiting reagent. It's stoichiometry decides the product formation amount from equation above it is clear that number of moles for $H_2O$ will be produced = number of moles of $H_2$

= 11.0 mol

3 0

3 years ago