In a constant‑pressure calorimeter, 70.0 mL of 0.350 M Ba(OH)2 was added to 70.0 mL of 0.700 M HCl. The reaction caused the temperature of the solution to rise from 23.97 ∘C to 28.74 ∘C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ).

The amount of heat absorbed by the solution is 2.795 kJ

Explanation:

To calculate the mass of water, we use the equation:

Density of water = 1 g/mL

Volume of water = [70 + 70] = 140 mL

Putting values in above equation, we get:

To calculate the heat absorbed, we use the equation:

where,

q = heat absorbed

m = mass of water = 140 g

c = heat capacity of water = 4.186 J/g°C

= change in temperature =

Putting values in above equation, we get:

Hence, the amount of heat absorbed by the solution is 2.795 kJ

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !