1g, 2c, and 2g I need an answer to thank you very much and make it clear please

Question

1g, 2c, and 2g I need an answer to thank you very much and make it clear please

1. A metal sample weighing 45.2 g and at a temperature of 100.0°C was placed in 38.6 g of water in a calorimeter at 25.2 C. At equilibrium the temperature of the water and metal was 33.0°C. a. What was At for the water? (Ar tnal-tiinal) b. What was At for the metal? oC Taking the specific heat of water to be 41 8 J g°C calculate the specific heat of the metal using Eq 3. joules/g C 100 C- 33.0 C c. d. What is the approximate atomic mass of the metal? (Use Eq. 4.) 2. When 2.0 g of NaOH were dissolved in 53.0 g water in a calorimeter at 24.0°C, the temperature of the solution went up to 33.7°C. a. Is this solution reaction exothermic?Why?solued- 3.0 b. Calculate qno, using Eq. 1. 2 2 30 joules c. Find AH for the reaction as it occurred in the calorimeter (Eq. 5). joules d. Find for the solution of 1.00 g NaOH in water. e. Find AH for the solution of one mole NaOH in water. 2x53 h, x trw o.GO 2.ce/male - FYlSo9 joules/mole 2230/0.00 26415os f. Given that NaOH exists as Nat and OH ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water g. Using enthalpies of formation as given in thermodynamic tables, calculate Alf for the reaction in Part f and compare your answer with the result you obtained in Part e

Explanation / Answer

1.

c. specifc heat of metal = [38.6 x 4.18 x (33 - 25.2)]/[45.2 x (100 - 33)]

                                      = 0.4155 J/g.oC

d. comparinf literature data for specific heat of metals.

value 0.4155 matches with Cobalt

approximate atomic mass of metal = 59 g/mol

2.

c. dH = -(2+53) x 4.18 x (33.7 - 24) = 2230.03 J

g. dHrxn = dHproducts - dHreactants

               = (-240 - 167) - (0)

               = -407 kJ/mol

This value is lower than the value calculated in part e.

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