cytoplasm
chlorophyll
nuclei
changes from 53.0 atm to 35.2
atm, the temperature changes
from
°C to 12.0°C.
Please help I will give brainliest
Answer:
To determine the relationship between pressure and temperature in this scenario, we can use the ideal gas law.
The ideal gas law states that PV = nRT, where P represents pressure, V represents volume, n represents the number of moles of gas, R is the ideal gas constant, and T represents temperature in Kelvin.
Since we only have the initial and final pressures and temperatures, we can compare them using the ideal gas law equation by setting up the following ratio:
(P₁T₁) / (P₂T₂) = (V₁n₁R) / (V₂n₂R)
Since the volume, number of moles, and gas constant remain constant, we can simplify the equation:
(P₁T₁) / (P₂T₂) = 1
Now, we can substitute the given values into the equation:
(53.0 atm * T₁) / (35.2 atm * 12.0°C) = 1
To solve for T₁, we need to convert 12.0°C to Kelvin by adding 273.15:
(53.0 atm * T₁) / (35.2 atm * (12.0 + 273.15) K) = 1
Simplifying the equation further:
(53.0 atm * T₁) / (35.2 atm * 285.15 K) = 1
Now, we can solve for T₁:
(53.0 atm * T₁) = (35.2 atm) * (285.15 K)
Dividing both sides of the equation by 53.0 atm:
T₁ = (35.2 atm * 285.15 K) / 53.0 atm
Calculating the numerical value:
T₁ ≈ 189.5 K
Therefore, when the pressure changes from 53.0 atm to 35.2 atm, the temperature changes from approximately 12.0°C to 189.5 K.
Ans: A)
HBrO and HBrO₃ are oxyacids where the acidic strength increases with the increase in the number of atoms attached to the central atom.
In both acids, oxygen is the most electronegative atom. In HBrO, the B atom is linked to only one O atom. In contrast, there are 3 electronegative O atoms surrounding the central B atom in HBrO₃ which would make the OH bond more polar and easily accessible. Thus, HBrO₃ tends to lose a proton readily than HBrO making the former more acidic.
HBrO is a weaker acid than HBrO3 because the H-O bond in HBrO is less polar than the H-O bond in HBrO3. In a series of oxyacids with similar formulas, the higher the electronegativity of the central atom, the stronger is the attraction of the central atom for the electrons of the oxygen(s), making the acid stronger.
The acid strength of HBrO is weaker than HBrO3 because the H-O bond in HBrO is less polar than the H-O bond in HBrO3 (Option A). In a series of oxyacids with similar formulas, the higher the electronegativity of the central atom, the stronger is the attraction of the central atom for the electrons of the oxygen(s). This stronger attraction of oxygen for the electrons in the O-H bond makes the hydrogen more easily released, resulting in a stronger acid (Option E). Therefore, HBrO3 is a stronger acid than HBrO.
Learn more about Oxyacids here:
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(1) the first shell
(2) the second shell
(3) the third shell
(4) the fourth shell
The valence electrons in an atom of phosphorus in the ground state are all found in IN THE THIRD SHELL.
Phosphorus has an atomic number of 15, therefore its electronic configuration is 2, 8, 5. This configuration implies that, phosphorus electrons are distributed in three different shells and the number of electrons in the outermost shell, which is the third shell, is 5. The ground state refers to a state, where the atoms of phosphorus are not excited. Electrons move away from their ground states when they are excited.