7.00g of compound x with molecular formula c5h10 are burned in a constant-pressure calorimeter containing 35.00kg of water at 25°c. the temperature of the water is observed to rise by 2.113°c. (you may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) calculate the standard heat of formation of compound x at 25°c. be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. [could you show a step by step way to solve this]

The standard heat of formation of Compound X at 25°C is -3095.75 kJ/mol.

Explanation:

Mass of compound X = 7.00 g

Moles of compound X =

Mass of water in calorimeter ,m= 35.00 kg = 35000 g

Change in temperature of the water in calorimeter = ΔT

ΔT = 2.113°C

Specific heat capacity of water ,c= 4.186 J/g °C

Q =  m × c × ΔT

Heat gained by 35 kg of water is equal to the heat released on burning of 0.100 moles of compound X.

Heat of formation of Compound X at 25°C:

= -3095.75 kJ/mol

answer

i think the answer is a) as air pressure in an area increases, the density of the gas particles in that area decreases.

hope it