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3 years ago

Name at least three types of energy associated with a microwave

1 answer:

3 0

I'm pretty sure what you are trying to ask for is radiative energy, light energy, and electronic energy.
Radiative since the microwave is releasing radiation,
Light since there is light inside the microwave,
Electronic since it is plugged in and uses electricity.
You can also use sound, but I don't think every microwave makes sound.

You might be interested in

Calculate the change in entropy when 10.0 g of CO2 isothermally expands from a volume of 6.15 L to 11.5 L. Assume that the gas b

USPshnik [31]

Answer:

The change in entropy of the carbon dioxide is $1.183\times 10^{-3}$ kilojoules per Kelvin.

Explanation:

By assuming that carbon dioxide behaves ideally, the change in entropy ( $\Delta S$ ), measured in kilojoules per Kelvin, is defined by the following expression:

$\Delta S = m\cdot \bar c_{v}\cdot \ln \frac{T_{f}}{T_{o}}+m\cdot \frac{R_{u}}{M}\cdot \ln \frac{V_{f}}{V_{o}}$ (1)

Where:

$m$ - Mass of the gas, measured in kilograms.

$\bar c_{v}$ - Isochoric specific heat of the gas, measured in kilojoules per kilogram-Kelvin.

$T_{o}$ , $T_{f}$ - Initial and final temperatures of the gas, measured in Kelvin.

$V_{o}$ , $V_{f}$ - Initial and final volumes of the gas, measured in liters.

$R_{u}$ - Ideal gas constant, measured in kilopascal-cubic meter per kilomole-Kelvin.

$M$ - Molar mass, measured in kilograms per kilomole.

If we know that $T_{o} = T_{f}$ , $m = 0.010\,kg$ , $R_{u} = 8.315\,\frac{kPa\cdot m^{3}}{kmol\cdot K}$ , $M = 44.010\,\frac{kg}{kmol}$ , $V_{o} = 6.15\,L$ and $V_{f} = 11.5\,L$ , then the change in entropy of the carbon dioxide is:

$\Delta S = \left[\frac{ (0.010\,kg)\cdot \left(8.315\,\frac{kPa\cdot m^{3}}{kmol\cdot K} \right)}{44.010\,\frac{kg}{kmol} } \right]\cdot \ln \left(\frac{11.5\,L}{6.15\,L}\right)$

$\Delta S = 1.183\times 10^{-3}\,\frac{kJ}{K}$

The change in entropy of the carbon dioxide is $1.183\times 10^{-3}$ kilojoules per Kelvin.

4 0

3 years ago

While you are doing your homework, a friend looks over your shoulder and sees electron configurations on your paper. "Whats That

zzz [600]

Answer:

The energy of atomic orbitals increases as the principal quantum number, n, increases. In any atom with two or more electrons, the repulsion between the electrons makes energies of subshells with different values of l differ so that the energy of the orbitals increases within a shell in the order s < p < d < f.

Explanation:

7 0

3 years ago

Using the phase diagram for CO2, what phase is carbon dioxide in at -20°C

djyliett [7]

Answer:

A. It is in the gas phase.

Explanation:

it was correct on ap3x :)

5 0

3 years ago

Methanol, ethanol, and n−propanol are three common alcohols. When 1.00 g of each of these alcohols is burned in air, heat is lib

Sergeeva-Olga [200]

Answer:

a) Heat of combustion of 1 g of methanol = -22.6 kJ = (-2.26 × 10) kJ

b) Heat of combustion of 1 g of ethanol = -29.7 kJ = (-2.97 × 10) kJ

c) Heat of combustion of 1 g of propanol = -33.5 kJ = (-3.35 × 10) kJ

Explanation:

a) The equation for the combustion of methanol is given as

CH₃OH + (3/2)O₂ → CO₂ + 2H₂O

The standard heat of combustion of methanol is given as -726 kJ/mol from literature.

But, 1 g of methanol will have the heat of combustion of the number of moles of methanol contained in 1 g of methanol.

Number of moles = (mass)/(molar mass)

Molar mass of (CH₃OH) = 32.04 g/mol

Number of moles = (1/32.04) = 0.03121 moles

1 mole of methanol has a heat of combustion of -726 kJ

0.03121 mole of methanol will have a heat of combustion of (0.03121 × -726) = -22.6 kJ

b) The equation for the combustion of ethanol is given as

C₂H₅OH + 3O₂ → 2CO₂ + 3H₂O

The standard heat of combustion of ethanol is given as -1367.6 kJ/mol from literature.

But, 1 g of ethanol will have the heat of combustion of the number of moles of ethanol contained in 1 g of ethanol.

Number of moles = (mass)/(molar mass)

Molar mass of (C₂H₅OH) = 46.07 g/mol

Number of moles = (1/46.07) = 0.0217 moles

1 mole of ethanol has a heat of combustion of -1367.6 kJ

0.0217 mole of ethanol will have a heat of combustion of (0.03121 × -1367.6) = -29.7 kJ

c) The equation for the combustion of propanol is given as

C₃H₇OH + (9/2)O₂ → 3CO₂ + 4H₂O

The standard heat of combustion of propanol is given as -2020 kJ/mol from literature.

But, 1 g of propanol will have the heat of combustion of the number of moles of propanol contained in 1 g of propanol.

Number of moles = (mass)/(molar mass)

Molar mass of (C₃H₇OH) = 60.09 g/mol

Number of moles = (1/60.09) = 0.0166 moles

1 mole of propanol has a heat of combustion of -2020 kJ

0.0166 mole of propanol will have a heat of combustion of (0.0166 × -2020) = -33.5 kJ

Hope this Helps!!!

5 0

3 years ago

how is substitution reaction in alkanes different from dehydrogenation reaction since both involve removing a hydrogen atom from

Ilia_Sergeevich [38]

Answer:

See Explanation

Explanation:

A substitution reaction means the replacement of one or more hydrogen atoms in an alkane by another atom or group. It does not introduce a double bond into the product. The product retains single bonds between the species present.

For instance;

CH4 + Cl2 -------> CH3Cl +HCl

is a substitution reaction

Dehydrogenation is the process of removing two hydrogen atoms from a saturated compound compound thereby yielding an unsaturated product.

E.g

C2H6 --------->C2H4 + H2

The key difference is that substitution reaction yields a saturated product while dehydrogenation yields an unsaturated product.

8 0

3 years ago