Answer:
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The wavelengths of the light are 4.3 * 10^-12 m and 0.2 m respectively.
<h3>What is wavelength?</h3>
The term wavelength has to do with the horizontal distance that is covered by a wave. We know that a long wavelength implies that the wave is able to travel a long distance from one point to another.
Given that;
c = λf
c = speed of light
λ = wavelength of ight
f = frequency of light
Thus;
λ = 3 * 10^8/ 7.00 x 10^19
λ = 4.3 * 10^-12 m
λ = 3 * 10^8/1.50 x 10^9
λ = 2 * 10^-1 or 0.2 m
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Missing parts:
What are the wavelengths of electromagnetic wave in free space that have the following frequencies? (a) 7.00 x 10^19 Hz______ pm (b) 1.50 x 10^9 Hz__________ cm
Answer:
T = 20.84°C
Explanation:
From the law of conservation of energy:
Heat Lost by Copper Block = Heat Gained by Aluminum Calorimeter + Heat Gained by Water

where,
= mass of copper = 227 g
= mass of water = 844 g
= mass of aluminum = 155 g
= specific heat capacity of calorimeter = 385 J/kg.°C
= specific heat capacity of water = 4200 J/kg.°C
= specific heat capacity of aluminum = 890 J/kg.°C
= change in temperature of copper = 283°C - T
= change in temperature of water = T - 14.6°C
= change in temperature of aluminum = T - 14.6°C
T = equilibrium temperature = ?
Therefore,

<u>T = 20.84°C</u>
Answer:
563712.04903 Pa
Explanation:
m = Mass of material = 3.3 kg
r = Radius of sphere = 1.25 m
v = Volume of balloon = 
M = Molar mass of helium = 
= Density of surrounding air = 
R = Gas constant = 8.314 J/mol K
T = Temperature = 345 K
Weight of balloon + Weight of helium = Weight of air displaced

Mass of helium is 6.4356 kg
Moles of helium

Ideal gas law

The absolute pressure of the Helium gas is 563712.04903 Pa
The temperature of the oxygen gas is 243.75 K.
Using ideal gas law to explain the answer, the absolute temperature of the gas will decrease if the number of moles of the gas increases and it will increase if the volume and/or pressure of the gas increases.
The reaction of the given elements;

volume of the collected oxygen gas, V = 10 L
pressure of the gas, P = 1 atm
number of moles of the gas, n = 0.5
Using ideal law the temperature of the oxygen gas is calculated as follows;

Thus, the temperature of the gas is 243.75 K.
Using ideal gas law to explain the answer. The absolute temperature of the oxygen gas is directly proportional to the product of its pressure and volume and inversely proportional to its number of moles. That is the absolute temperature of the gas will decrease if the number of moles of the gas increases and it will increase if the volume and/or pressure increases.
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