Question

in a calorimetry experiment 21.00g of magnesium is reacted with 50mL of 1.1 mol/L hydrochloric acid with an initial temp of 21.4 degrees celsius the final temp was 23.9 degrees Celsius 1) calculate the enthalpy for the reaction

Answer 1

Sure! To calculate the enthalpy (ΔH) for the reaction, we can use the equation:

ΔH = q / n

Where:
- ΔH is the enthalpy change
- q is the heat transferred during the reaction
- n is the number of moles of the limiting reactant

First, let's calculate the heat transferred (q) during the reaction. We can use the equation:

q = m * c * ΔT

Where:
- q is the heat transferred
- m is the mass of the solution (in grams)
- c is the specific heat capacity of the solution (assumed to be 4.18 J/g°C)
- ΔT is the change in temperature (final temperature - initial temperature)

Given:
- Mass of magnesium (m) = 21.00 g
- Specific heat capacity of the solution (c) = 4.18 J/g°C
- Change in temperature (ΔT) = 23.9°C - 21.4°C

Now, let's calculate the number of moles of the limiting reactant (n). Since magnesium (Mg) is the limiting reactant in this case, we can use its molar mass:

Molar mass of Mg = 24.31 g/mol

Number of moles of Mg = Mass of Mg / Molar mass of Mg

Finally, we can substitute the values into the equation to calculate the enthalpy change (ΔH).

I hope this helps! Let me know if you have any other questions or need further assistance with the calculations.