Please help with these questions. Thanks
Consider the reaction
C12H22O11(s)+ 12O2(g)-->12CO2(g)+11H2O(l)
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in which 10.0 g of sucrose,C12H22O11 , was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/ degrees celsius. The temperature increase was found to be 22.0 degrees celsius. Calculate the change in internal energy, E, for this reaction per mole of sucrose.
Express your answer numerically in kilojoules per mole.
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okay but i don't know where to star i would like an explanation if no one minds or a good link relating to this information.
Here is a good site to start you. Repost here with specific questions.
What the good site?
Sorry about that.
http://www.chem.ufl.edu/~itl/2045/lectures/lec_9.html
To calculate the change in internal energy (ΔE) per mole of sucrose, we need to first calculate the heat released by the reaction.
The heat released can be determined using the equation:
q = C × ΔT
where q is the heat released, C is the heat capacity of the calorimeter, and ΔT is the temperature increase.
In this case, the heat capacity (C) is given as 7.50 kJ/°C, and the temperature increase (ΔT) is 22.0 °C. Plugging in these values, we can calculate the heat released:
q = (7.50 kJ/°C) × (22.0 °C)
q = 165 kJ
Since the reaction is the combustion of one mole of sucrose, the heat released is per mole of sucrose. Therefore, the ΔE per mole of sucrose is equal to the heat released, which is 165 kJ.
Thus, the change in internal energy (ΔE) for this reaction per mole of sucrose is 165 kJ/mol.