When 0. 485 g of compound x is burned completely in a bomb calorimeter containing 3000 g of water, a temperature rise of 0. 285°c is observed. What is δu of the reaction for the combustion of compound x? the hardware component of the calorimeter has a heat capacity of 3. 81 kj/°c. The specific heat of water is 4. 184 j/g·°c, and the mw of x is 56. 0 g/mol.

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AnnuG AnnuG · Answer 1 · 2022-11-19T15:02:01+01:00

ΔU of the reaction the combustion of compound x is -538 kJ/mol

Combustion is a reaction in which a substance reacts with oxygen gas and releasing energy in the form of light and heat

Here given data is

Mass of compound x = 0.485gram

Mass of water = 3000gram

Temprature rise = 0. 285°C

Heat capacity of the calorimeter = 3. 81 kJ/°C

Specific heat of water = 4. 184 J/g·°C

MW of x = 56. 0 g/mol

Then calculate q

ΔU = ΔH -PΔV

The bomb calorimeter has a constant volume ΔV = 0

ΔU = ΔH

q reaction = q(water + q(bomb)

q(bomb) = 3810J/°C×0.285 = 1085.85J

q(water) = 3000g × 4. 184 J/g·°C×0.285°C = 3577.32 J

q reaction = q(water) + q(bomb)

q reaction = 4663.17 J = 4.66kJ means this is an exothermic

Then calculate moles of compound

Moles = mass/molar mass

Moles = 0.485 g/56.0g/mol

Moles = 0.00866 moles

Then calculate ΔU

ΔU = 4663.17 J/0.00866 moles = 538472 j/mol = 538.5kJ/mol means the reaction is exothermic

ΔU = -538kJ/mol

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