Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.127 g of Zn(s) is combined with enough HCl to make 52.1 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.3 ∘C to 23.9 ∘C . a. Find ΔrH for this reaction as written. (Use 1.0 gmL−1 for the density of the solution and 4.184 Jg−1∘C−1 as the specific heat capacity.)

200.0 mL of 0.200 M HNO3 is added to 200.0 mL of 0.200 M KOH in a coffee cup calorimeter. The neutralization reaction that occurs can be described by the chemical equation- HNO3(aq) + KOH(aq) → KNO3(aq) + H₂O(l) Before the solutions are mixed they are both at 23.00 °C. After the mixing of the solutions the temperature increases until it remains constant at 24.39 °C. Assuming no heat lost to the surroundings, how much heat was lost in this reaction? (Assume the specific heats and densities of the solutions is the same as water.)

When a 4.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity of 1.47 kJ · K-, the temperature decreases by 0.360 K. Calculate the molar heat of solution of RbBr. AH soln -2 1.28 x10 kJ/mol Incorrect

When a 3.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity of 1.89 kJ · K¯¹, the temperature decreases by 0.210 K. Calculate the molar heat of solution of RbBr. AH S = soln kJ/mol