Answer:
The correct option is: a chemical reaction between carbohydrates and oxygen to produce carbon dioxide, water, and heat energy
Explanation:
Respiration refers to the catabolic reactions in the cells that produce energy in the form of adenosine triphosphate (ATP) from various nutrients.
An aerobic respiration, is a spontaneous process that involves the use of <u>molecular oxygen (O₂) to produce energy (ATP). In this process, molecular oxygen oxidizes nutrients such as carbohydrates, fats, and proteins; to give carbon dioxide, water and heat energy</u>.
Answer:
d. directly proportional to the number of moles of the gas.
Explanation:
The formula for the partial pressure of a gas is written as -
P = n * P ( total )
P = partial pressure of the gas ,
n = mole fraction of the gas ,
P ( total ) = Total pressure of the mixture of gas .
Hence , from the above equation ,
the partial pressure is directly proportional to the mole fraction , i.e. , on increasing the number of moles of gas , the partial pressure increases .
Answer:
1700 kj
Explanation:
The given reaction is exothermic reaction.
Exothermic reaction:
The type of reactions in which energy is released are called exothermic reactions.
In this type of reaction energy needed to break the bonds are less than the energy released during the bond formation.
For example:
Chemical equation:
C + O₂ → CO₂
ΔH = -393 Kj/mol
it can be written as,
C + O₂ → CO₂ + 393 Kj/mol
Chemical equation:
2Al + Fe₂O₃ → Al₂O₃ + 2Fe + 850 Kj
when one mole of Fe₂O₃ react 850 kj energy is produced.
when 2 moles react,
2 × 850 kj = 1700 kj
Answer:
153.6771 amu
Explanation:
From the question given above, the following data were:
Isotope A:
Mass of A = 114.3789 amu
Abundance (A%) = 64.23%
Isotope B:
Mass of B =.?
Abundance (B%) = 100 – A%
Abundance (B%) = 100 – 64.23
Abundance (B%) = 35.77%
average atomic mass of Element Y = 128.4359 amu
The mass of the 2nd isotope (i.e isotope B) can be obtained as follow:
Average atomic mass = [(Mass of A × A%)/100] + [(Mass of B × B%)/100]
128.4359 = [(114.3789 × 64.23)/100] + [(Mass of B × 35.77) /100]
128.4359 = 73.4656 + (Mass of B × 0.3577)
Collect like terms
128.4359 – 73.4656 = Mass of B × 0.3577
54.9703 = Mass of B × 0.3577
Divide both side by 0.3577
Mass of B = 54.9703 / 0.3577
Mass of B = 153.6771 amu
Therefore, the mass of the 2nd isotope is 153.6771 amu