Substance | Specific Heat |
A | \[0.60\,J{{g}^{-1}}{{\,}^{o}}{{C}^{-1}}\] |
B | \[0.40\,J{{g}^{-1}}{{\,}^{o}}{{C}^{-1}}\] |
C | \[0.20\,J{{g}^{-1}}{{\,}^{o}}{{C}^{-1}}\] |
A) \[{{T}_{C}}>{{T}_{B}}>{{T}_{A}}\]
B) \[{{T}_{B}}>{{T}_{A}}>{{T}_{C}}\]
C) \[{{T}_{A}}>{{T}_{B}}>{{T}_{C}}\]
D) \[{{T}_{A}}={{T}_{B}}={{T}_{C}}\]
Correct Answer: C
Solution :
Heat absorbed or evolved, \[\Delta Q=ms\Delta t.\] Where,\[m=\] mass of substance, s = specific heat\[\Delta t=\] temperature difference It means \[s\propto \frac{1}{\Delta t}.\] Higher the temperature of the given solution, lesser is the temperature difference. So higher is the specific heat. As, the specific heat order is A > B > C. So, the order of temperature of solution is A > B > C. Hence, the correct option is [c].You need to login to perform this action.
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