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Question- The combustion of 3.010 g sucrose, in a bomb calorimeter, causes the temperature to rise from 24.92 to 78.33?C. The heat capacity of the calorimeter assembly is 4.90 kJ/?C.
a) What is the heat of combustion of sucrose, expressed in kJ/mol C12H22O11.
b) Verify the claim of sugar producers that one teaspoon of sugar (about 4.8g) contains only 19 calories.
I want to know how this is done please show all steps in detail
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Problem- Sucrose (table sugar) has the formula C12H22O11 (molar mass= 342.30) and a food value of 6.49 kj/g. Determine the calorimeter constant of the calorimeter in which the combustion of 2.040g of sucrose raises the temperature by 2.08 C
If the container has a pinhole leak, which describes the relationship between the partial pressures of the individual components in the containtainer after 3 hours? (A.) PSO2 > PCH4>PH2. (B.) PSO2 PH2. (D) PSO2= PCH4 = PH2.
The following equilibrium concentrations were measured at 800 K:[SO2]=3.0*10^-3M; [O2]=3.5*10^-3M; [SO3]=5.0*10^-2M. Calculate the equilibrium constant at 800K for each of the following reactions.
Gas particles are attracted to one another and therefore behave as grouped particles.
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Acetylsalicylic acid (aspirin), HC9H7O4, is the most widely used pain reliever and fever reducer in the world. Find the pH of 0.045 M aqueous aspirin at body temperature (Ka at 37°C = 3.6 10-4)
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