A dilute aqueous solution with a mass of 43.8031 g has a temperature increase of 10.2 ^\circ
∘
C. Calculate the enthalpy change in kilojoules.
q = delta H = mass H2O x specific heat H2O x delta T
Plug and chug. Post your work if you get stuck.
To calculate the enthalpy change, we can use the formula:
q = m * c * ΔT
Where:
q is the heat energy transferred (enthalpy change)
m is the mass of the solution
c is the specific heat capacity of the solution
ΔT is the change in temperature
First, let's calculate the specific heat capacity (c) of the solution. The specific heat capacity of water is commonly used for aqueous solutions, so we'll use that value.
c = 4.18 J/g·°C
Next, convert the mass of the solution from grams to kilograms:
mass = 43.8031 g = 0.0438031 kg
Substituting the given values into the formula, we get:
q = (0.0438031 kg) * (4.18 J/g·°C) * (10.2 °C)
Now, let's convert the heat energy from joules to kilojoules:
q = (0.0438031 kg) * (4.18 J/g·°C) * (10.2 °C) / 1000
Calculating this, we find:
q ≈ 0.001825 kJ
Therefore, the enthalpy change in kilojoules is approximately 0.001825 kJ.
To calculate the enthalpy change, we can use the equation:
ΔH = q / n
where:
ΔH = enthalpy change (in kilojoules)
q = heat absorbed or released (in joules)
n = number of moles
First, let's find the value of q:
q = m * c * ΔT
where:
m = mass of the solution (in grams)
c = specific heat capacity (in joules per gram-degree Celsius)
ΔT = change in temperature (in degrees Celsius)
Given:
m = 43.8031 g
ΔT = 10.2 °C
To find c, we need to know the specific heat capacity of the solution. Assuming it is water, the value for c is approximately 4.18 J/g°C.
Now we can calculate q:
q = (43.8031 g) * (4.18 J/g°C) * (10.2 °C)
Next, we need to convert q from joules to kilojoules. Since 1 kJ = 1000 J, we divide q by 1000:
q_kJ = q / 1000
Finally, we can substitute the value of q_kJ into the enthalpy change equation to calculate ΔH:
ΔH = q_kJ / n
Note: We need the number of moles (n) of the substance involved in the reaction to calculate the enthalpy change accurately. Unfortunately, it's not provided in the question.