The reaction for the metabolism of sucrose, C12H22O11, is the same as for its combustion in oxygen to yield CO2(g) and H2O(l). The standard heat of formation of sucrose is -2230 kJ mol^(-1). Use the data in the table below to compute the amount of energy (in kJ) released by metabolizing 2.04 oz (57.7 g) of sucrose.
[
egin{array}{|c|c|c|}
hline
ext{Substance} & ext{Standard Heat of Formation (kJ/mol)} \
hline
ext{C(s) (graphite)} & 0 \
ext{H2O(g)} & -241.8 \
ext{CO(g)} & -110.5 \
ext{H2O(l)} & -285.9 \
ext{CO2(g)} & -393.5 \
ext{CH4(g)} & -74.848 \
ext{HBr(g)} & -36 \
ext{CH3Cl(g)} & -82.0 \
ext{HCl(g)} & -92.30 \
ext{CH3I(g)} & 14.2 \
ext{HI(g)} & 26.6 \
ext{CH3OH(l)} & -238.6 \
ext{HNO3(l)} & -173.2 \
ext{CO(NH2)2(s) (urea)} & -333.19 \
ext{H2SO4(l)} & -811.32 \
ext{CO(NH2)2(aq)} & -391.2 \
ext{HC2H3O2(l)} & -487.0 \
ext{C2H2(g)} & 226.75 \
ext{O2(g)} & 0 \
ext{C2H4(g)} & 52.284 \
ext{Pb(s)} & 0 \
ext{C2H6(g)} & -84.667 \
ext{PbO(s)} & -219.2 \
ext{C2H5OH(l)} & -277.63 \
ext{S(s)} & 0 \
ext{H2(g)} & 0 \
ext{SO2(g)} & -296.9 \
ext{SO3(g)} & -395.2 \
hline
end{array}
]
Question 2
Numeric Fill in the Blank with Units
Question 3
Numeric Fill in the Blank with Units
Question 4
CW: graphite, CO(g), H2O(g), H2O(l), HBr(g), HCl(g), HI(g), HNO3(l), H2SO4(l), HC2H3O2(l)
Question 5
Numeric Fill in the Blank with Units: CH4(g), CH3Cl(g), C2H2(g), C2H4(g), C2H6(g), C2H5OH(l)
Question 6
Multipart
Question 7
True or False: 5O2(g)
Question 8
Multiple Choice: kJ
Question 9
Numeric Fill in the Blank
