Answer:
Final temperature attained by water = 34.6°C
Explanation:
The reaction of CaO and H₂O is an <em>exothermic reaction</em>. The equation of reaction is given below:
CaO + H₂O ----> Ca(OH)₂
The quantity of heat given off, ΔH°rxn = 64.8KJ/mol = 64800J/mol
Number of moles of CaO = mass/molar mass, where molar mass of Ca0 = 56g/mol, mass of CaO = 10.1g
Number of moles of CaO = 10.1g/56g/mol =0.179moles
Quantity of heat given off by 0.179 moles = 64800 *0.179 = 11599.2J/mol
Using the formula, <em>Quantity of heat, q = mass * specific heat capacity * temperature rise.</em>
mass of mixture = (10.1 + 157)g = 167.1g, Initial temperature = 18.0°C
Final temperature(T₂) - Initial temperature(T₁) = Temperature rise
11599.2J/mol = 167.1g * 4.18J/g·°C * ( T₂ - 18.0°C)
11599.2 = 698.478T₂ - 12572.604
11599.2 + 12572.604 = 698.478T₂
698.478T₂ = 24171.804
T₂ = 34.6°C
Therefore, final temperature attained by water = 34.6°C
![-pOH= log [ OH^{-}]](https://tex.z-dn.net/?f=-pOH%3D%20log%20%5B%20OH%5E%7B-%7D%5D%20)
![[ OH^{-}]= 10^{-pOH}](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%3D%2010%5E%7B-pOH%7D%20%20)
![[ OH^{-}] = 10^{-6.48}](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%20%3D%2010%5E%7B-6.48%7D%20)
![[ OH^{-}]=3.31* 10^{-7} M](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%3D3.31%2A%2010%5E%7B-7%7D%20M%20%20)