Respuesta :
Answer: The final temperature of the mixture is 51.49°C
Explanation:
When two samples of water are mixed, the heat released by the water at high temperature will be equal to the amount of heat absorbed by water at low temperature
[tex]Heat_{\text{absorbed}}=Heat_{\text{released}}[/tex]
The equation used to calculate heat released or absorbed follows:
[tex]Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})[/tex]
[tex]m_1\times c\times (T_{final}-T_1)=-[m_2\times c_2\times (T_{final}-T_2)][/tex] ......(1)
where,
q = heat absorbed or released
[tex]m_1[/tex] = mass of water at high temperature = 140 g (Density of water = 1.00 g/mL)
[tex]m_2[/tex] = mass of water at low temperature = 230 g
[tex]T_{final}[/tex] = final temperature = ?°C
[tex]T_1[/tex] = initial temperature of water at high temperature = 95.00°C
[tex]T_2[/tex] = initial temperature of water at low temperature = 25.00°C
c = specific heat of water= 4.186 J/g°C
Putting values in equation 1, we get:
[tex]140\times 4.186\times (T_{final}-95)=-[230\times 4.186\times (T_{final}-25)][/tex]
[tex]T_{final}=51.49^oC[/tex]
Hence, the final temperature of the mixture is 51.49°C
