When the speed of the particle is close to that of light, it's observed mass would be infinitely large.
To answer the question, we need to know what observed mass is.
<h3>What is observed mass in relativity?</h3>
This is the mass the body of an object in relativistic motion appears to have.
So, observed mass, m' = m/√(1 - β²) where
- m = rest mass and
- β = relative velocity of isotope to light.
Now, since the speed of the particle is close to that of light, β ≅ 1.
So, m' = m/√(1 - β²)
m' = m/√(1 - 1²)
m' = m/√(1 - 1)
m' = m/√0
m' = m/0
m' = ∞
So, when the speed of the particle is close to that of light, it's observed mass would be infinitely large.
Learn more about observed mass here:
brainly.com/question/14553472
Answer:
False.
Explanation:
The given statement is false because for hot vacuum filtration, the filter paper should be wet rather than dry when pouring the hot solution into the Buchner funnel. This is because The possible explanation the filter paper needs to be wetted is not only to allow it to adhere to the funnel, but also to promote the solute to filter down readily across its pores of the paper without wetting it (this is true for organic and aqueous solvents).
Answer:
why did you post a link to brainly when we are on brainly already??????
Explanation:
Answer:
Conditions are optimal for upwelling along the coast when winds blow along the shore. Winds blowing across the ocean surface push water away. Water then rises up from beneath the surface to replace the water that was pushed away. This process is known as “upwelling.”
Explanation:
Answer:
2.4 g
Explanation:
Step 1: Given data
- Initial pressure (P₁): 755 torr
- Final pressure (P₂): 1.87 atm
Step 2: Convert "P₁" to atm
We will use the conversion factor 1 atm = 760 torr.
755 torr × 1 atm/760 torr = 0.993 atm
Step 3: Convert "T" to K
We will use the following expression.
K = °C + 273.15
K = 25°C + 273.15 = 298 K
Step 4: Calculate the initial number of moles of He
We will use the ideal gas equation.
P₁ × V = n₁ × R × T
n₁ = P₁ × V/R × T
n₁ = 0.993 atm × 16.8 L/(0.0821 atm.L/mol.K) × 298 K
n₁ = 0.682 mol
Step 5: Calculate the final number of moles of He
We will use the ideal gas equation.
P₂ × V = n₂ × R × T
n₂ = P₂ × V/R × T
n₂ = 1.87 atm × 16.8 L/(0.0821 atm.L/mol.K) × 298 K
n₂ = 1.28 mol
Step 6: Calculate the moles of He added
n = n₂ - n₁
n = 1.28 mol - 0.682 mol
n = 0.60 mol
Step 7: Convert "n" to mass
The molar mass of He is 4.00 g/mol
0.60 mol × 4.00 g/mol = 2.4 g
