4. hcl is a corrosive colourless gas that dissolves readily in water. aqueous hcl reacts with naoh to form…

4. hcl is a corrosive colourless gas that dissolves readily in water. aqueous hcl reacts with naoh to form water and nacl. in a simple calorimeter, a 100.00 ml sample of 0.355 mol/l hcl(aq) is mixed with 50.00 ml of excess naoh(aq). during the reaction, there is a rise in temperature by 4.200 °c. calculate the molar enthalpy change for the above reaction. show all your work.

4. hcl is a corrosive colourless gas that dissolves readily in water. aqueous hcl reacts with naoh to form water and nacl. in a simple calorimeter, a 100.00 ml sample of 0.355 mol/l hcl(aq) is mixed with 50.00 ml of excess naoh(aq). during the reaction, there is a rise in temperature by 4.200 °c. calculate the molar enthalpy change for the above reaction. show all your work.

Answer

Explanation:

Step1: Calculate the moles of HCl

The formula for moles (n = c\times V), where (c) is the concentration and (V) is the volume. Given (c = 0.355\space mol/L) and (V=100.00\space mL=0.10000\space L) (n_{HCl}=0.355\space mol/L\times0.10000\space L = 0.0355\space mol)

Step2: Calculate the mass of the solution

Assume the density of the solution is (1\space g/mL). The total volume of the solution (V_{total}=100.00 + 50.00=150.00\space mL) The mass (m=\rho\times V), with (\rho = 1\space g/mL) and (V = 150.00\space mL) (m = 150.00\space g)

Step3: Calculate the heat absorbed by the solution

The formula for heat (q = mc\Delta T), where (c = 4.18\space J/(g\cdot^{\circ}C)) (specific - heat capacity of water) and (\Delta T=4.200^{\circ}C) (q=(150.00\space g)\times(4.18\space J/(g\cdot^{\circ}C))\times(4.200^{\circ}C)) (q = 150\times4.18\times4.200\space J=2633.4\space J = 2.6334\space kJ)

Step4: Calculate the molar enthalpy change

The molar enthalpy change (\Delta H=\frac{q}{n}) Since the reaction is exothermic ((q) is released by the reaction), (\Delta H=-\frac{2.6334\space kJ}{0.0355\space mol}) (\Delta H=- 74.2\space kJ/mol)

Answer:

The molar enthalpy change for the reaction is (-74.2\space kJ/mol)