ZN(s) + 2H+(aq) produces ZN2+(aq) +H2(g)
A sample of Zinc is placed in the ice calorimeter. if 0.0657g of Zinc causes a decrease of 0.109ML in the ice/water volume of the calorimeter, what is the enthalpy change, per mole of Zinc, for the above reaction per mole of zinc.
PLEASE HELP! DUE TOMORROW. I DON'T KNOW WHAT TO DO. It looks like there is not enough information given to find enthalpy change.
H2O(s) ==> H2O(l)
The density of liquid H2O = 1.00 g/mL.
The density of ice is 0.917 g/mL.
Suppose we start with 1 mol (18 g) H2O(s) and it melts to the liquid.
As a liquid it will occupy 18g/1.00 = 18 mL.
As a solid it will occupy 18/0.917 = 19.63 mL.
19.63-18.0 = 1.63 mL diffeence.
The heat fusion of ice is 6.01 kJ/mol; therefore, 6.01/1.63 = about 3.69 kJ for each mL difference.
In this experiment we have a difference of 0.109 mL; then 3.69 kJ/mL x 0.109 mL = ? kJ for 0.0657 g Zn. You want per mol Zn and you have 0.0657/65.39 = about 0.001 mol Zn so
?kJ/0.001 = ? kJ/mol Zn.
To find the enthalpy change per mole of zinc for the given reaction, we need more information such as the initial and final temperatures of the system or the heat capacity of the ice/water mixture in the calorimeter. Without this information, we cannot directly calculate the enthalpy change.
However, we can still make some general observations. In the given reaction, 0.0657g of zinc causes a decrease in volume of the ice/water mixture, indicating an exothermic reaction where heat is released. This means that the enthalpy change is negative.
If you have the initial and final temperatures of the system along with the mass of the ice/water mixture or the heat capacity of the calorimeter, you can calculate the enthalpy change using the following equation:
ΔH = -(q / n)
where ΔH is the enthalpy change, q is the heat absorbed or released by the system, and n is the number of moles of zinc involved in the reaction.
To calculate q, you can use the equation:
q = m × C × ΔT
where m is the mass of the water/ice mixture, C is the specific heat capacity of the mixture, and ΔT is the change in temperature.
If you have the initial and final temperatures, the mass of the ice/water mixture, and the specific heat capacity of the mixture, you can proceed with the calculations. Otherwise, you will need to provide additional information to solve the problem accurately.