What is the heat liberated when 10g of citric acid is combusted at 298k?

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To calculate the heat liberated from the combustion of 10g of citric acid at 298K, first convert the mass into moles using the molar mass of citric acid. The heat of combustion is given as ΔH = -1986 kJ/mol, which indicates the energy released per mole of citric acid combusted. Since combustion reactions typically occur at constant pressure, this is the relevant condition for the calculation, and specifying pressure is unnecessary as it is assumed in standard conditions. By multiplying the number of moles of citric acid by the heat of combustion, the total heat liberated can be determined. This approach provides a clear method for calculating the energy released during the combustion process.
rcs
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I am confused on how to find out the heat of combustion of solid citric acid to water and carbondioxide that is deltaH 296 -1986 kJ/mol. I need to figure out the heat liberated when 10g of citric acid is totally combusted at 298k? *a) At constant pressure?? at constant volume?? and why is it not necessary to specify the pressure in part a?
 
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hello can one give me some input
 
rcs said:
I am confused on how to find out the heat of combustion of solid citric acid to water and carbondioxide that is deltaH 296 -1986 kJ/mol. I need to figure out the heat liberated when 10g of citric acid is totally combusted at 298k? *a) At constant pressure?? at constant volume?? and why is it not necessary to specify the pressure in part a?

HINT: Think about converting your mass into moles. (what units is \Delta H given as)?
 
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