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3 years ago

What is the wavelength of electromagnetic radiation with a frequency of 5.00 x 10^12 Hz? S

Chemistry

1 answer:

Angelina_Jolie [31]3 years ago

8 0

Answer:

Infrared

Explanation:

To calculate the wavelength if the electromagnetic radiation, we must use the following formula:

c = f × λ

where c is the speed of the wave (in this case it's the speed of light, which is 3 × $10^{8}$ m/s) , f is the frequency and λ is the wavelength.

Using this formula, all we have to do is plug in our values and rearrange for the answer:

c = f × λ

3 × $10^{8}$ = 5.00 x $10^{12}$ Hz × λ

λ = 3 × $10^{8}$ /5.00 x $10^{12}$

λ = 6.00 × $10^{-5}$ m = 6.00 × $10^{4}$ nm

Now that we know the wavelength we can figure out which kind of electromagnetic radiation this is.

6.00 × $10^{4}$ nm falls in the range of infrared radiation. We know this either from memorizing the values of the wavelengths or looking up a reference.

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Compare and contrast aldehydes, ketones and alcohols in terms of structure, physical properties and chemical properties.

Ksivusya [100]

The functional group of aldehyde is -CHO

The functional group of ketone is -CO-

The functional group of alcohol is -OH

<h2>STRUCTURES</h2><h3>ALDEHYDE</h3>

The carbonyl group is bounded to at least one hydrogen atom

<h3>KETONE</h3>

The carbonyl group is bounded to two carbon atom

<h3>ALCOHOL</h3>

Organic molecules assembled from carbon, oxygen and hydrogen.

<h2>PHYSICAL PROPERTIES</h2><h3>COLOUR</h3>

Aldehyde. alcohols and ketone are colourless

<h3>ODOURS</h3>

Alcohols are sweet smell expect glycerol

Aldehyde have unpleasant odors

ketone have pleasant odors

<h3>BOILING POINT</h3>

Alcohol , Aldehyde and Ketone have High boiling point

<h3>STATE</h3>

Alcohol, Aldehyde and Ketone are in liquid state

<h2>CHEMICAL PORPERTIES</h2><h3>OXIDATION </h3>

Alcohol oxidized to form carboxylic acid

Aldehyde oxidized to form carboxylic acid

Ketone oxidized to form carboxylic acid

Learn more about alcohol, aldehyde and ketone on

https://brainly.ph/question/11006608

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7 0

2 years ago

How does molarity and molality affect the concentration of a solution<br>explain.

kolbaska11 [484]

Concentration of a solution can be expressed in terms of molarity and molality

Molarity is the number of moles of solute in a liter of a solution.

Molarity (M) = Moles of solute/Volume(litres) of solution

Molality is the number of moles of solute in one kg of the solution

Molality (m) = Moles of solute/Mass (kg) of solution

Therefore if the volume or the mass of the solution is changed this would affect the concentration.

In addition, volume is a quantity which depends on temperature. However, mass is independent of temperature. Therefore any changes in temperature, can also bring about a change in the molarity of the solution.

5 0

3 years ago

Methanol, CH3OH, is the simplest of the alcohols. It is synthesized by the reaction of hydrogen and carbon monoxide. Write chemi

Serhud [2]

Answer:

The limiting reactant is H₂

Explanation:

The reaction of hydrogen (H₂) and carbon monoxide (CO) to produce methanol (CH₃OH) is the following:

2H₂(g) + CO(g) → CH₃OH(g)

From the balanced chemical equation, we can see that 1 mol of CO reacts wIth 2 moles of H₂. So, the stoichiometric ratio is:

2 mol H₂/1 mol CO = 2.0

We have 500 mol of CO and 750 mol of H₂, so we calculate the ratio to establish a comparison:

750 mol H₂/500 mol CO = 1.5

Since 2.0 > 1.5, we have fewer moles of H₂ than are needed to completely react with 500 moles of CO. In fact, we need 1000 moles of H₂ and we have 750 moles. So, the limiting reactant is H₂.

8 0

3 years ago

Oxygen gas can be prepared by heating potassium chlorate according to the following equation:2KClO3(s)Arrow.gif2KCl(s) + 3O2(g)T

Eduardwww [97]

Answer:

Moles of potassium chlorate reacted = 0.2529 moles

The amount of oxygen gas collected will be 12.8675 g

Explanation:

(a)

We are given:

Vapor pressure of water = 17.5 mmHg

Total vapor pressure = 748 mmHg

Vapor pressure of Oxygen gas = Total vapor pressure - Vapor pressure of water = (748 - 17.5) mmHg = 730.5 mmHg

To calculate the amount of Oxygen gas collected, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 730.5 mmHg

V = Volume of the gas = 9.49 L

T = Temperature of the gas = $20^oC=[20+273]K=293K$

R = Gas constant = $62.3637\text{ L.mmHg }mol^{-1}K^{-1}$

n = number of moles of oxygen gas = ?

Putting values in above equation, we get:

$730.5mmHg\times 9.49L=n\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 293K\\\\n=\frac{730.5\times 9.49}{62.3637\times 293}=0.3794mol$

According to the reaction shown below as:-

$2KClO_3(s)\rightarrow 2KCl(s) +3O_2(g)$

3 moles of oxygen gas are produced when 2 moles of potassium chlorate undergoes reaction.

So,

0.3794 mol of oxygen gas are produced when $\frac{2}{3}\times 0.3794$ moles of potassium chlorate undergoes reaction.

<u>Moles of potassium chlorate reacted = 0.2529 moles</u>

(b)

We are given:

Vapor pressure of water = 17.5 mmHg

Total vapor pressure = 753 mmHg

Vapor pressure of Oxygen gas = Total vapor pressure - Vapor pressure of water = (753 - 17.5) mmHg = 735.5 mmHg

To calculate the amount of Oxygen gas collected, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 735.5 mmHg

V = Volume of the gas = 9.99 L

T = Temperature of the gas = $20^oC=[20+273]K=293K$

R = Gas constant = $62.3637\text{ L.mmHg }mol^{-1}K^{-1}$

n = number of moles of oxygen gas = ?

Putting values in above equation, we get:

$735.5mmHg\times 9.99L=n\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 293K\\\\n=\frac{735.5\times 9.99}{62.3637\times 293}=0.40211mol$

Moles of Oxygen gas = 0.40211 moles

Molar mass of Oxygen gas = 32 g/mol

Putting values in above equation, we get:

$0.037mol=\frac{\text{Mass of Oxygen gas}}{2g/mol}\\\\\text{Mass of Oxygen gas}=(0.40211mol\times 32g/mol)=12.8675g$

<u>Hence, the amount of oxygen gas collected will be 12.8675 g</u>

5 0

3 years ago

What is the quantity of heat (in kJ) associated with cooling 185.5 g of water from 25.60°C to ice at -10.70°C?Heat Capacity of S

Cerrena [4.2K]

Taking into account the definition of calorimetry, sensible heat and latent heat, the amount of heat required is 37.88 kJ.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

<h3>Sensible heat</h3>

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

<h3>Latent heat</h3>

Latent heat is defined as the energy required by a quantity of substance to change state.

When this change consists of changing from a solid to a liquid phase, it is called heat of fusion and when the change occurs from a liquid to a gaseous state, it is called heat of vaporization.

<u><em>25.60 °C to 0 °C</em></u>

First of all, you should know that the freezing point of water is 0°C. That is, at 0°C, water freezes and turns into ice.

So, you must lower the temperature from 25.60°C (in liquid state) to 0°C, in order to supply heat without changing state (sensible heat).

The amount of heat a body receives or transmits is determined by:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case, you know:

c= Heat Capacity of Liquid= 4.184 $\frac{J}{gC}$
m= 185.5 g
ΔT= Tfinal - Tinitial= 0 °C - 25.60 °C= - 25.6 °C

Replacing:

Q1= 4.184 $\frac{J}{gC}$ × 185.5 g× (- 25.6 °C)

Solving:

<u><em>Change of state</em></u>

The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to

Q = m×L

where L is called the latent heat of the substance and depends on the type of phase change.

In this case, you know:

n= 185.5 grams× $\frac{1mol}{18 grams}$ = 10.30 moles, where 18 $\frac{g}{mol}$ is the molar mass of water, that is, the amount of mass that a substance contains in one mole.