The initial temperature of the water in a constant-pressure calorimeter is 24°c. a reaction takes place in the calorimeter, and the temperature rises to 87°c. the calorimeter contains 367 g of water, which has a specific heat of 4.18 j/(g·°c). calculate the enthalpy change (δh) during this reaction.

4739.86 J/mol.

Explanation:

The amount of heat released to water = Q = m.c.ΔT.

where, m is the mass of water (m = 367.0 g).

c is the specific heat capacity of water = 4.18 J/g°C.

ΔT is the temperature difference = (final T - initial T = 87.0°C - 24.0°C = 63.0°C).

∴ The amount of heat absorbed by released to water = Q = m.c.ΔT = (367.0 g)(4.18 J/g°C)(63.0°C) = 96645.78 J.

ΔH = Q/n.

n = mass/molar mass = 367 g/18 g/mol = 20.39 mol.

∴ ΔH = Q/n = - (96645.78 J)/(20.39 mol) = 4739.86 J/mol.

the leaf is an organ of a typical plant, and the main functions are to complete photosynthesis and allow the plant to exchange gas, just like how we have the respiratory system. leaves have the stomata, which collects maintains co2 and o2 levels. this is necessary for cell metabolism. the leaf also collects sunlight using chloroplasts. succinctly, leaves own a pivotal role in sustaining plant life.