Zinc metal reacts with hydrochloric acid according to the following balanced equation.Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)When 0.111 g of Zn(s) is combined with enough HCl to make 53.8 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘C to 24.0 ∘C.Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g⋅∘C as the specific heat capacity.)

In the following experiment, solid CaCl2 is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq)     ΔsolnH = −82.8 kJ mol−1A coffee-cup calorimeter containing 145 mL of H2O is used. The initial temperature of water in the calorimeter is 18.9°C. If 3.04 g of CaCl2 is added to the water, what will be the final temperature of the solution in the calorimeter? Assume the density and specific heat capacity of the solution is the same as water (d=1 g/mL, Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.

Help

4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).

3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g °C and the density of the water is 1.00 g/ mL). You can assume that the specific heat of the solution is the same as that of water.

When a 7.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 5.28 kJ⋅K^-1, the temperature decreases by 0.330 K Calculate the molar heat of solution of KSCN.

In a constant‑pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2 was added to 60.0 mL of 0.640 M HCl.The reaction caused the temperature of the solution to rise from 24.50 ∘C to 28.86 ∘C. If the solution has the same density and specific heat as water (1.00 g/mLand 4.184J/g⋅°C, respectively), what is ΔH for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes. ΔH= _________ kJ/mol H2O

A student determines the heat of dissolution of solid potassium bromide using a coffee-cup calorimeter of negligible heat capacity.When 4.93 g of KBr(s) is dissolved in 108.00 g of water, the temperature of the solution drops from 25.00 to 23.11 °C. Based on the student's observation, calculate the enthalpy of dissolution of KBr(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.ΔHdissolution =  kJ/mol

4.71 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g.°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.

A student dissolves 10.7 g of lithium chloride (LiCl)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 22.0 °C to 28.4 °C over the course of 3.6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: LiCl (s) Lit (aq) + Cl(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 2 significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ. per mole of LiCl. rxn 0 exothermic…