Question

1. Prepare for It! Prelab Question A A 235.0 g sample of metal is heated to 100.0°C and poured into a calorimeter containing 50.0 g of water at 20.5°C. The equilibrium temperature of the water and metal is 30.5°C. Using the specific heat of water, 4.18 J/g C, determine the specific heat of the metal from equation 3. Use equation 5 to find the approximate molar mass of the metal. Show your work! Use back if needed. 2. Prepare for It! Prelab Question B If 3.1 g of NaOH (s) is dissolved in 57.9 g of water with an initial temperature of 22.5°C and the temperature rises to 36.6°C, then find the enthalpy of solution (in J) using equation 6 Determine the enthalpy in J/g and kJ/mole. Show your work! kJ/mol II

Answer 1

Mass of metal - 23510g Initial tehting metal = 150°c Mass of water = 500g Intial tomp of water = 20.5°c ea temp water metal = 30.5 c. specific treat of water = 4.15 Tlf.00 reat lost by metal = in x cmt at - 235.og x cm x 30.5-100) = - 16332.5 cm theat gained by water = mx cox ot = 500 x 4.19 X (30.5-20:5) = Rogos out eq. (-heat lost by metal) = t tout gained by water => 16332.5 x cm = R090 = 01279557 Ilgooo Em = 2090 16332.5 = 0.128 Ilg.oc. Fm+. Na = 3:19 water = 57.gg Tis 22.5°C To=35.6°C theat gained by the water Ewenty = muxtur * AT = 57.9 x 4.10 x 36.6-22.5) = 3412.51 T alsoin = – a water AHS* = -342.51 GH Sol 9 - - 3412.51 g -100) hoteles d HGOH 31/40 = 0.075 hale -3412.51_-44032.39 A HSO 3 O s mole -44.03 K3 male