Object A at 40 degrees C and object B at 80 degrees C are placed in contact with each other. The heat flow will flow from the Object B to the object A because of temperature difference. To attain equilibrium, the heat flow must flow form a higher temperature to a lower temperature.
b) phosphorus
c) aluminum
d) boron
6
5
3
2
(2) H−Cl
(3) I−Br
(4) I−Cl
Among the presented bonds, the most polar is H-Cl.
Polarity is a separation of electric charge leading to a molecule or its chemical groups having an electric dipole moment.
The higher the difference in electronegativity, the more polar the bond.
We will calculate the difference in electronegativity for each bond.
ΔEN = |EN(H)-EN(Br)| = |2.2-3.0| = 0.8
ΔEN = |EN(H)-EN(Cl)| = |2.2-3.2| = 1.0
ΔEN = |EN(I)-EN(Br)| = |2.7-3.0| = 0.3
ΔEN = |EN(I)-EN(Cl)| = |2.7-3.2| = 0.5
Among the presented bonds, the most polar is H-Cl.
Learn more about polarity here: brainly.com/question/8857494
Answer:
The partial pressure of nitrogen is 0.402 atm.
Explanation:
Given data:
Number of moles of helium = 1 mol
Number of moles of nitrogen = 2 mol
Total pressure of mixture = 0.60 atm
Partial pressure of nitrogen = ?
Solution:
First of all we will calculate the mole fraction of nitrogen.
mole fraction of nitrogen = moles of nitrogen / total number of moles
mole fraction of nitrogen = 2 mol / 3 mol = 0.67
Partial pressure of nitrogen:
P₁ = [ n₁ /n(t)] × Pt
P₁ = 0.67 × 0.60 atm
P₁ = 0.402 atm
To find the partial pressure of nitrogen in a mixture, calculate the mole fraction of nitrogen and multiply it by the total pressure of the mixture. In this case, the partial pressure of nitrogen is 0.40 atm.
The question is about determining the partial pressure of nitrogen in a mixture of helium and nitrogen based on Dalton's Law of Partial Pressures. First, we find the mole fraction of nitrogen, which is the ratio of moles of nitrogen to the total moles in the mixture. In this scenario, the mole fraction (XN2) is 2 moles of nitrogen divided by the total moles (1 mole of helium + 2 moles of nitrogen), which equals 2/3.
Then we use Dalton's Law, which states that the partial pressure of nitrogen (PN2) can be found by multiplying the mole fraction by the total pressure of the mixture. Therefore, the partial pressure of nitrogen is 0.60 atm (total pressure) multiplied by 2/3 (mole fraction of nitrogen), yielding a partial pressure for nitrogen of 0.40 atm.
#SPJ3
b. external diffraction.
c. total internal reflection.
d. interference
Answer:
(C) Total internal reflection
Explanation:
Total internal reflection :
So the option (c) is the correct option
B. The average energy increases.
C. The average velocity of the particles increases by a factor of sqrt 2 .
D. The average energy remains constant but the velocity of some particles increases
When the temperature of a gas rises, the average energy of the particles increases. According to the Kinetic Molecular Theory, kinetic energy is proportional to its temperature. However, a rise in temperature doesn't directly double the energy.
The behavior of particles in a gas is very much affected by temperature changes. When the temperature of a gas increases, so too does the energy that the gas's particles have. This is defined by the Kinetic Molecular Theory, which states that the kinetic energy of a gas is proportional to its temperature. Therefore, when the temperature of a gas rises from 23°C to 46°C, the average energy of the particles increases. However, it doesn't double as an increase in temperature is not responsible for directly doubling the energy. Additionally, this increase in energy results in an increase in the velocity of the particles, but not necessarily by a factor of sqrt(2).
#SPJ2