Answer: 0.0007 moles of 
are released when the temperature rises.
Explanation:
To determine the moles, we utilize the ideal gas law, as follows:
where,
P = gas pressure = 1.01 bar
V = gas volume = 1L
R = gas constant = 
- Calculated moles at T = 20° C
The gas temperature = 20° C = (273 + 20)K = 293K
Substituting values into the equation gives:
- Calculated moles at T = 25° C
The gas temperature = 25° C = (273 + 25)K = 298K
Substituting values into the equation gives:
- Released moles =
Therefore, 0.0007 moles of are released when the temperature increases from 20° C to 25° C.
To tackle this problem, one must first determine the specific heat of water, which is the energy required to raise the temperature of 1 g of water by 1 degree C. The relationship is given by the formula q = c X m X delta T, where q indicates the specific heat of water, m signifies the mass, and delta T denotes the temperature change. The specific heat of water is 4.184 J/(g X degree C). The temperature of the water increased by 20 degrees, therefore: 4.184 x 713 x 20.0 = 59700 J, rounded to 3 significant digits, equals 59.7 kJ. This value indicates the energy required to produce B2O3 from 1 gram of boron. To convert this to kJ/mole, additional calculations are required. The gram atomic mass of Boron is 10.811, so dividing 1 gram of boron by 10.811 results in.0925 moles of boron. Given that 2 moles of boron are needed for the formation of 1 mole of B2O3, dividing the moles of boron by two yields.0925/2 =.0462 moles. Consequently, dividing the energy in KJ by the number of moles provides KJ/mole: 59.7/.0462 = 1290 KJ/mole.
