How much heat is evolved in converting 1.00 mol of steam at 130.0 C to ice at -50.0 C? The heat capacity of steam is 2.01 J/(g⋅C) and of ice is 2.09 J/(g⋅C).

I'm not sure if my calculations are correct:

Part A: Solving for Calorimeter Constant

TRIAL 1

Involving 50 mL of 1.83M HCl and 50 mL of 2.08M NaOH, trial 1 lasted for 9 minutes, temperature rose from 21.5 celsius to 34.3 celsius in 3.15 minutes and then fell to 32.3 celsius at the end of the 9 minutes

Solutions

Temperature change >>>> 12.80 celsius

Average temperature change >>>> 1.2 celsius / sec

Mass of solution, g >>>> 7.50g

Solution heat capacity, C_s, Joule/Kelvins >>>> 404.4 J/K

deltaH_rxn, Joule >>>> -5554 J

Calorimeter Constant, C_c, Joule/Kelvin >>>> -465.5 J/K

Part B: Calculation of Enthalpy of Neutralization

TRIAL 1

Involving 50 mL of 2.18M HNO3 and 50 mL of 2.16M NH3, trial 1 lasted for 9 minutes, temperature rose from 22.5 celsius to 35.8 celsius in 3.5 minutes and then fell to 33.7 by the end of the 9 minutes

Solutions

Temperature change >>>> 13.30 celsius

Average temperature change >>>> 1.24 celsius / sec

Mass of solution, g >>>> 102.9g

Solution heat capacity, C_s, Joule/Kelvins >>>> 401.31 J/K

deltaH_rxn, Joule >>>> -5726.1 J

Molar Enthalpy of neutralization >>>> -53.0 kJ

Part C: Enthalpy of Dissolution of Ammonium Salt

TRIAL 1

Involving 8.164g of NH4NO3 in 100 mL of H2O, trial lasted for 9 minutes, temperature fell from 23.2 celsius to 16.8 celsius in 4 minutes and then rose to 17.0 celsius by the end of the 9 minute trial.

Solutions

Temperature change >>>> 7.90 celsius

Average temperature change >>>> -.566 celsius / sec

Mass of solution, g >>>> 108g

Solution heat capacity, C_s, Joule/Kelvins >>>> 421 J/K

deltaH_rxn, Joule >>>> 3565J

Molar enthalpy of dissolution >>>> -32.3 kJ/mol

A quantity of 2.00 × 102 mL of 0.852 M HCl is mixed with 2.00 × 102 mL of 0.426 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.69°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions?

H⁺(aq) + OH⁻(aq) → H₂O(l)

The strongest lines in the solar spectrum are the Ca H and K lines which are produced by singly-ionized Ca atoms in the ground state. Show that, in the solar atmosphere (Teff = 5777 K, ne = 2

Use equations to discuss why a peak value of the UV-Visble Spectra should be used so that the Beer's Law is followed.

Predict the order of reactivity for the following monomers in anionic polymerization for the following monomers a) styrene b) methyl methacrylate c) acrylonitrile d) cyanoacrylate?

What is the ionic strength of each of the following solutions: a. 0.1 M NaCl b. 0.1 M Na2-oxalate c. 0.1 M CuSO4

A 1-L flask is filled with 1.30 g of argon at 25 ∘C. A sample of ethane vapour is added to the same flask until the total pressure is 1.06 bar .

a) What is the partial pressure of argon, PAr, in the flask?

b)What is the partial pressure of ethane, Pethane, in the flask?

The conversion of solid wastes to innocuous gases can be accomplished in incinerators in an environmentally acceptable fashion. However, the hot exhaust gases often must be cooled or diluted with air. An economic feasibility study indicates that solid municipal waste can be burned to a gas of 9.2% CO2, 1.5% CO, 6.5%O2, 78% N2 and rest water on a molar basis. You can neglect any energy effects resulting from the mixing of gaseous components. What is the enthalpy difference if 300 m^3/h of the stack at 290C is cooled to 30C?

Find the pH of a 0.150M solution of a weak monoprotic acid having Ka= 0.20.

Calculate the entropy change when a He atom in the gas phase expands from V1 to 2V1 at constant temperature.

A) 5.8 kJ/K

B) 9.6 x 10-24 kJ/K

C) -5.8 kJ/K

D) 0 kJ/K

E) not enough information

Describe the effects of adding Mn to steel and give a use for manganese-steel alloys.

A sample of 25.00 ml of 0.1007 M acetic acid (HC2H2o2 was titrated with 0.1004 M NAOH what is the pH of the sample at the equicalence point of the titration? The Ka for accetic acid is 1.8 x 10^-5