Answer:
Explanation:
For a chemical reaction, the enthalpy of reaction (ΔHrxn) is … ... to increase the temperature of 1 g of a substance by 1°C; its units are thus J/(g•°C). ... Both Equations 12.3.7 and 12.3.8 are under constant pressure (which ... The specific heat of water is 4.184 J/g °C (Table 12.3.1), so to heat 1 g of water by 1 ..
Answer : The enthalpy change during the reaction is 4.74 kJ/mole
Explanation :
First we have to calculate the heat released during the reaction.
[tex]q=m\times c\times (T_{final}-T_{initial})[/tex]
where,
q = heat released = ?
[tex]c[/tex] = specific heat of water = [tex]4.18J/g^oC[/tex]
m = mass of water = 367 g
[tex]T_{final}[/tex] = final temperature of water = [tex]87^oC[/tex]
[tex]T_{initial}[/tex] = initial temperature of metal = [tex]24^oC[/tex]
Now put all the given values in the above formula, we get:
[tex]q=367g\times 4.18J/g^oC\times (87-24)^oC[/tex]
[tex]q=96645.78J=96.6kJ[/tex]
Thus, the heat released during the reaction = 96.6 kJ
Now we have to calculate the enthalpy change during the reaction.
[tex]\Delta H=\frac{q}{n}[/tex]
where,
[tex]\Delta H[/tex] = enthalpy change = ?
q = heat released = 96.6 kJ
n = number of moles water = [tex]\frac{\text{Mass of water}}{\text{Molar mass of water}}=\frac{367g}{18g/mol}=20.4mole[/tex]
[tex]\Delta H=\frac{96.6kJ}{20.4mole}=4.74kJ/mole[/tex]
Therefore, the enthalpy change during the reaction is 4.74 kJ/mole
