Answer:
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Answer:
Total pressure = 4.57 atm
Explanation:
Given data:
Partial pressure of nitrogen = 1.3 atm
Partial pressure of oxygen = 1824 mmHg
Partial pressure of carbon dioxide = 247 torr
Partial pressure of argon = 0.015 atm
Partial pressure of water vapor = 53.69 kpa
Total pressure = ?
Solution:
First of all we convert the units other into atm.
Partial pressure of oxygen = 1824 mmHg / 760 = 2.4 atm
Partial pressure of carbon dioxide = 247 torr / 760 = 0.325 atm
Partial pressure of water vapor = 53.69 kpa / 101 = 0.53 atm
Total pressure = Partial pressure of N + Partial pressure of O + Partial pressure of CO₂ + Partial pressure of Ar + Partial pressure of water vapor
Total pressure = 1.3 atm + 2.4 atm + 0.325 atm + 0.015 atm + 0.53 atm
Total pressure = 4.57 atm
Answer:
No
Explanation:
given that, enthalpy is a state function, that means it depends only on the initial and final states, there is no difference between the enthalpy of a phase transition versus the enthalpy of a heating or cooling process, when the cooling or heating process finish in a change of phase.
It does not matter which way we take to cool or heat the substances the Enthalpy of this process will be the same.
The lowest value of the henry's law for methane gas (CH₄) will be obtained with H₂O as the solvent and a temperature of 349 K.
The lowest value of the henry's law for methane gas (CH₄) will be obtained with H₂O as the solvent and a temperature of 349 K.
Henry's law: This law states that at a constant temperature, the amount of a gas dissolved in a given type and volume of liquid is directly proportional to the partial pressure of that gas that in equilibrium with that liquid.
Mathematically it can be written as:
So, for the methane gas , lowest value of the henry's law obtained at 349 K and with H₂O as the solvent.
Covalent bonds can be classified as nonpolar and polar covalent given the electronegativity difference between two atoms (ΔEN).
Nonpolar covalent bond electrons are shared equally between two atoms, polar covalent bond electrons are shared unequally, atoms have partial charges, ionic bond electrons are completely transferred to one atom, full charges present. Therefore, the greater the electronegativity difference, the greater the bond polarity. Let's determine the types of bonds present in the compounds and arrange the ones with polar covalent in order of increasing ΔEN. Sulfur and oxygen are both nonmetals so the substance is covalent. Sulfur has EN = 2.5 and oxygen has EN = 3.5. Since there is an electronegativity difference, the S−O bonds in the substance can be classified as polar covalent bonds.
Learn more about polar covalent bond here:
brainly.com/question/25150590
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