P * V = n R T
<span>1 * 2.50 = n * 0.082 * 273 = 2. 50 / ( 0.082 * 273 ) = 0.11 mol </span>
<span>mass = mole number * molecular mass </span>
<span>mass = 0.11 * ( 16 * 2 ) = 3.52 g </span>
Answer: Option C. p-dichlorobenzene and 1,4-dichlorobenzene.
Explanation:
A line-angle formula with six vertices and a circle inscribed corresponds to the compound known as benzene.
Further, according to the IUPAC standards for naming benzene derivatives, you must first number the position of the substituent. In this case, the substituents (chloros) are located at the positions 1 and 4; also, for the benzene derivatives when they have 2 substituents and the positions are 1 and 4, this configuration is known as <em>para </em>or <em>p </em>configuration.
Additionally, this compound has 2 substituents (chloros) so you have to indicate this number (di).
Therefore, the correct answer is C. p-dichlorobenzene and 1,4-dichlorobenzene.
Patent - Not sure if this is much of a Chem question dou.
The answer is B 2. As it says Atom Number of Protons and Number of Neutrons, from my understanding it means that the first number after the letter is the number of protons and the second number is the number of neutrons.
Now, If there are 6 protons in a nucleus that means there are 6 electrons on the outside, so A and D are the same element. However, you may be confused because of the different number of neutrons (6 and 7 or 7 and 8) this only means that one is and isotope of the element.
*Isotopes are atoms with the same number of protons but different number of neutrons. (Basically, same element different mass)
Answer:
Mass released = 8.6 g
Explanation:
Given data:
Initial number of moles nitrogen= 0.950 mol
Initial volume = 25.5 L
Final mass of nitrogen released = ?
Final volume = 17.3 L
Solution:
Formula:
V₁/n₁ = V₂/n₂
25.5 L / 0.950 mol = 17.3 L/n₂
n₂ = 17.3 L× 0.950 mol/25.5 L
n₂ = 16.435 L.mol /25.5 L
n₂ = 0.644 mol
Initial mass of nitrogen:
Mass = number of moles × molar mass
Mass = 0.950 mol × 28 g/mol
Mass = 26.6 g
Final mass of nitrogen:
Mass = number of moles × molar mass
Mass = 0.644 mol × 28 g/mol
Mass = 18.0 g
Mass released = initial mass - final mass
Mass released = 26.6 g - 18.0 g
Mass released = 8.6 g
