When 0.969 g of CaO is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 397C is observed.
Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/gC.
(Note: Pay attention to significant figures. Do not round until the final answer.)
Hrxn , for the reaction of
CaO(s) + 2H+(aq) Ca2+(aq) + H2O(l)
is kJ/mol.
please help it is due at 5
To find the heat of the reaction (ΔHrxn), we can use the equation:
ΔHrxn = q / n
Where:
- ΔHrxn is the heat of the reaction in kJ/mol,
- q is the heat absorbed or released in Joules (J),
- n is the number of moles of the limiting reactant.
First, let's determine the number of moles of CaO used in the reaction.
Number of moles of CaO = mass of CaO / molar mass of CaO
Given that the mass of CaO is 0.969 g and the molar mass of CaO is 56.08 g/mol:
Number of moles of CaO = 0.969 g / 56.08 g/mol
Now, let's calculate the heat absorbed or released (q) using the equation:
q = mcΔT
Where:
- q is the heat absorbed or released in Joules (J),
- m is the mass of the solution in grams,
- c is the specific heat capacity of the solution in J/g°C,
- ΔT is the change in temperature in °C.
The mass of the solution can be calculated using the density and volume:
mass of solution = density of solution * volume of solution
Given that the density of the solution is 1.00 g/mL and the volume of the solution is 200.0 mL:
mass of solution = 1.00 g/mL * 200.0 mL
Now, substitute the mass of the solution and the specific heat capacity into the equation to find q:
q = (mass of solution) * (specific heat capacity) * ΔT
Finally, substitute the calculated values for q and the number of moles of CaO into the equation for ΔHrxn:
ΔHrxn = q / (number of moles of CaO).
Calculate each step using the given values and algebraically, ensuring you consider significant figures.