2. Solved Papers
  3. AMU Medical

AMU Medical AMU Solved Paper-2014

  • question_answer
    A person inhales 640 g of \[{{O}_{2}}\] per day. If all \[{{O}_{2}}\]is used for converting sugar into \[C{{O}_{2}}\] and\[{{H}_{2}}O\], how much sucrose \[({{C}_{12}}{{H}_{22}}{{O}_{11}})\] is consumed in the body in one day and what is the heat evolved? \[\Delta H\] for combustion of sucrose \[=-5645\,kJ\,mo{{l}^{-1}}\]

    A)  530 g, 9403.34 kJ

    B)  570 g, 9408.34 kJ

    C)  500 g, 9402.27 kJ

    D)  520 g, 9435.21 kJ

    Correct Answer: B

    Solution :

                    \[{{C}_{12}}{{H}_{22}}{{O}_{11}}\,\,\,+12\,\,{{O}_{2}}\xrightarrow{{}}12C{{O}_{2}}+11\,{{H}_{2}}O;\] \[12\times 12+1\times 22\,\,\,12\times 16\times 2\,\,\,\,{{\Delta }_{C}}H=-5645\,\,kJ\]\[mo{{l}^{-1}}\] \[+11\times 16=342=384\] \[\because \] 384 g of \[{{O}_{2}}\] converts = 342 g of sugar \[\therefore \]640 g of \[{{O}_{2}}\] will convert \[=\frac{342\times 640}{384}\]                                                 = 570 g of sugar. Again, \[\because \,342\,g\]of sucrose evolves heat = 5645 kJ \[\therefore \,570\,g\] of sucrose will evolve heat                 \[=\frac{5645\times 570}{342}\]                 = 9408.33 kJ


You need to login to perform this action.
You will be redirected in 3 sec spinner