Some species of hares are brown most of the year, but change color to white in the winter. This allows them to blend in
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Answer:
The yield of the product in gram is
Explanation:
Given that:
the molecular mass weight of the product = 96.2 g/mol
the molecular mass of the reagent (3S)-2,2,-dibromo-3,4-dimethylpentane is 257.997 g
given that the millimoles of the reagent = 2,7 millimoles =
We know that:
Number of moles = mass/molar mass
Then:
mass = 0.697
Theoretical yield = (number of moles of the product/ number of moles of reactant) × 100
i.e
Theoretical yield =
where;
and
Theoretical yield =
Given that the theoretical yield = 100%
Then:
where,
= derived weight of the product
the molecular mass of the derived product
the molecular mass of the reagent
= weight in a gram of the reagent
Answer:
1. The pressure will be 32 atm, twice the initial pressure.
2. The pressure will be 1.83 atm, one third of the initial pressure.
Explanation:
Boyle's law is one of the gas laws that relates the volume and pressure of a certain quantity of gas kept at a constant temperature.
This law says that "The volume occupied by a given gaseous mass at constant temperature is inversely proportional to pressure." This means that if the pressure increases, the volume decreases, while if the pressure decreases, the volume increases.
Boyle's law is expressed mathematically as:
Pressure * Volume = constant
or P * V = k
Ahora es posible suponer que tienes un cierto volumen de gas V1 que se encuentra a una presión P1 al comienzo del experimento. Si varias el volumen de gas hasta un nuevo valor V2, entonces la presión cambiará a P2, y se cumplirá:
P1*V1=P2*V2
1. In this case:
- P1= 16 atm
- V1
- P2= ?
- V2= V1÷2=
because the volume is halved.
So:
16 atm*V1= P2*
Solving:
=P2
16 atm*2= P2
32 atm= P2
<u><em>The pressure will be 32 atm, twice the initial pressure.</em></u>
2. Now
- P1= 5.5 atm
- V1
- P2= ?
- V2= V1*3 because the volume is tripled.
So:
5.5 atm*V1= P2* V1*3
Solving:
=P2
= P2
1.83 atm= P2
<u><em>The pressure will be 1.83 atm, one third of the initial pressure.</em></u>