A total of 2.00 mol of a compound is allowed to react in a foam coffee cup that contains 167 g of water. The reaction caused the temperature of the water to rise from 21.0 to 24.7 degrees C. What is the enthalpy?
heat=167*c*(3.7)
Normally, one wants enthalpy on a per mole basis, if so, divide by 2.
To determine the enthalpy change (ΔH) of a reaction using the temperature change of a substance, you can use the equation:
ΔH = q / n
Where:
ΔH is the enthalpy change (in J/mol)
q is the heat absorbed or released by the reaction (in J)
n is the number of moles of the substance involved in the reaction
In this case, we need to calculate the heat absorbed or released (q) by the water. The heat equation for water can be given by:
q = m * C * ΔT
Where:
q is the heat absorbed or released (in J)
m is the mass of the water (in g)
C is the specific heat capacity of water (4.184 J/g°C)
ΔT is the change in temperature (in °C)
Let's calculate the heat (q) absorbed by the water.
Given:
Mass of water (m): 167 g
Specific heat capacity of water (C): 4.184 J/g°C
Change in temperature (ΔT): 24.7°C - 21.0°C = 3.7°C
Substituting the values into the equation, we get:
q = 167 g * 4.184 J/g°C * 3.7°C
Now, we can calculate q.
q = 2676.068 J
Next, we need to calculate the number of moles (n) of the compound involved in the reaction. Given that there are 2.00 mol of the compound, n = 2.00 mol.
Now, we can calculate the enthalpy change (ΔH) using the formula:
ΔH = q / n
Substituting the values, we get:
ΔH = 2676.068 J / 2.00 mol
Calculating this expression gives the enthalpy change (ΔH) for the reaction.