In the following experiment, a coffee-cup calorimeter containing 100.0 mL of H2O is used. The initial temperature of the calorimeter is 23.0 °C. If 9.20 g of CaCl, is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The enthalpy of dissolution A,H of CaCl, is –82.8 kJ mol 1 Express your answer with the appropriate units.

When 35.0 mL of 0.250 M acetic acid solution, initially at 25.00oC, is added to excess dilute sodium hydroxide solution, also initially at 25.00oC, in a neutralization reaction, in a calorimeter, the temperature increases to 26.35 oC. The mass of the final solution is 85.0 g. Assuming the specific heat of the solution and products is 4.18 J/goC. Calculate the enthalpy change in kJ, Δ H, for this reaction.HC2H3O2(aq) + NaOH(aq) --> NaC2H3O3(aq) + H2O(l)

A generic solid, X, has a molar mass of 84.9 g/mol.84.9 g/mol. In a constant‑pressure calorimeter, 13.0 g13.0 g of X is dissolved in 259 g259 g of water at 23.00 °C. X(s)⟶X(aq)X(s)⟶X(aq) The temperature of the resulting solution rises to 25.00 ∘C.25.00 ∘C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? ?=q=   kJkJ What is the enthalpy of the reaction? Δ?rxn=ΔHrxn=

6. 100.0 mL of 1.00 M of HCl and 100.0 mL of 2.00 M of Ca(OH)2 are mixed at 298K. During the experiment, the temperature rose to 298.0067 K. Assume the heat capacities of the two solutions and densities are the same as that of water (4.184 J/g °C and 1.00 g/mL). Calculate the heat of neutralization in units of (kJ/mol H₂0 produced).

Please if possible to be done on text and not writing

In a constant‑pressure calorimeter, 55.0 mL55.0 mL of 0.900 M H2SO40.900 M H2SO4 was added to 55.0 mL55.0 mL of 0.250 M NaOH.0.250 M NaOH. The reaction caused the temperature of the solution to rise from 22.90 ∘C22.90 ∘C to 24.60 ∘C.24.60 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184 J/(g⋅°C),4.184 J/(g⋅°C), respectively), what is Δ?ΔH for this reaction (per mole of H2OH2O produced)? Assume that the total volume is the sum of the individual volumes.

2 HCI(aq) + Ba(OH)2(aq) --> Bacl2(aq) + 2 H2O(1) AH= -118 kJ Calculate the heat when 114.0mL of 0.500M HCl is mixed with 300.0 mL of 0.435M Ba(OH)2. Assuming that the temperature of both solutions was initially 25.0°C and that the final mixture has a mass of 414.0g and a specific heat capacity of 4.18 J/°Cg, calculate the final temperature of the mixture. Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 10)

4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.0 J K–1. Prior to mixing everything was equilibrated to 21.2 °C. The resulting solution with a mass of 23.4 g was observed to be at a temperature of -6.8 °C and have a specific heat capacity of 4.61 J g–1 K–1. Determine q per mole for this dissolution process.   a. -5150 J/mol b. -1.94 × 104 J/mol c. 2.89 × 105 J/mol d. -3.39 × 105 J/mol e. 3.30 × 104 J/mol

Mg(s) + 1/2 O2(g) -> MgO(s). Determind the value of the standard enthalphy change for the reaction.  Mg(s) + 2 HCI(aq) -> MgCl2(aq) + H2(g). ∆Hrxn = -316 kJ mol-1 MgO(s) + 2 HCI(aq) -> MgCl2(aq) + H2O. ∆Hrxn = -45.7 kJ mol-1 H2(g) + 1/2 O2(g) -> H2O. ∆Hrxn = -286 kJ mol-1

A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). (   Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = J