Answer: 18.97 L
Explanation:
This can be solved by the Ideal Gas equation:
Where:
is the pressure of the gas
is the volume of the gas
the number of moles of gas
is the gas constant
is the absolute temperature of the gas in Kelvin
Finding :
Therefore:
The volume occupied by 1.5 mole of gas at 35°C and 2.0 atmosphere of pressure is <u>18.97</u> liters
If by classical you mean formula name it is CrPO4<span>.</span>
Answer:
Livermorium is a radioactive, artificially produced element about which little is known. It is expected to be a solid and classified as a metal. It is a member of the chalcogen group. Livermorium has four isotopes with known half-lives, all of which decay through alpha decay
Answer:
V = 0.2714 mL
Explanation:
Henry's Law:
∴ Kh CO2 = 0.034 M/atm ....The Henry's constant
∴ Partial pressure: P CO2 = 3.7 atm
⇒ <em>C</em> CO2 = P CO2 / Kh
⇒ <em>C</em> CO2 = 3.7 atm / 0.034 M/atm = 108.823 M (mol/L)
∴ molar mass CO2 = 44.01 g/mol
⇒ mol CO2 = (1.3 E3 mg)(g/1000 mg)(mol/44.01 g) = 0.03 mol CO2
volumen solution:
⇒ V sln = (0.03 mol)(L/108.823 mol) = 2.714 E-4 L
⇒ V sln = 0.2714 mL
Calorimetry-the science or act of measuring changes in state variables of a body for the purpose of deriving heat transfer associated with changes of its due date.
