Answer:
2
Explanation:
In two reactions energy is released.
1) C₆H₁₂O₆ + 6O₂ → 6H₂O + 6CO₂ + heat
It is cellular respiration reaction.It involves the breakdown of glucose molecule in the presence of oxygen to yield large amount of energy. Water and carbon dioxide are also produced as a byproduct.
Glucose + oxygen → carbon dioxide + water + 38ATP
2) 2H₂ + O₂ → 2H₂O ΔH = -486 kj/mol
The given reaction is formation of water. In this reaction oxygen and hydrogen react to form water and 486 kj/mol is also released.
The reaction in which heat is released is called 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
Endothermic reactions:
The type of reactions in which energy is absorbed are called endothermic reactions.
In this type of reaction energy needed to break the bond are higher than the energy released during bond formation.
For example:
C + H₂O → CO + H₂
ΔH = +131 kj/mol
it can be written as,
C + H₂O + 131 kj/mol → CO + H₂
<u>Answer:</u> The number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg
<u>Explanation:</u>
To calculate the amount of nitrogen gas, we use the equation given by ideal gas which follows:

where,
P = pressure of the gas = 755 mmHg
V = Volume of the gas = 2.55 L
T = Temperature of the gas = ![23^oC=[23+273]K=296K](https://tex.z-dn.net/?f=23%5EoC%3D%5B23%2B273%5DK%3D296K)
R = Gas constant = 
n = number of moles of nitrogen gas = ?
Putting values in above equation, we get:

To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law.
The equation follows:

where,
are the initial pressure, volume and temperature of the gas
are the final pressure, volume and temperature of the gas
We are given:
![P_1=755mmHg\\V_1=2.55mL\\T_1=23^oC=[23+273]K=296K\\P_2=?\\V_2=4.10L\\T_2=18^oC=[18+273]K=291K](https://tex.z-dn.net/?f=P_1%3D755mmHg%5C%5CV_1%3D2.55mL%5C%5CT_1%3D23%5EoC%3D%5B23%2B273%5DK%3D296K%5C%5CP_2%3D%3F%5C%5CV_2%3D4.10L%5C%5CT_2%3D18%5EoC%3D%5B18%2B273%5DK%3D291K)
Putting values in above equation, we get:

Hence, the number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg
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