Question

Part A Calculate the final temperature when 35 mL of water at 50 °C are added to 75 mL of water at 45 °C. Assume density of water is 1.00 g/mL and no heat is lost to the calorimeter. IVO AQ o 2 ? Part A If the specific heat of methanol is 2.51 J/K-g, how many joules are necessary to raise the temperature of 12 g of methanol from 26°C to 78°C ? IVO AO + O 2 ? Part A When a 1.78 g sample of solid sodium hydroxide was dissolved in a calorimeter in 60.0 g of water, the temperature rose from 4.2°C to 40.8 °C. Calculate AH (in kJ/mol NaOH) for the following solution process: NaOH(s) +Na+ (aq) + OH - (aq) Assume that it's a perfect calorimeter and that the specific heat of the solution is the same as that of pure water.

Answer 1

A Let the final temperature is T m, = 35 ml x 1g/ml = 35g T = 50°C m2 = 75 ml x 1g/m2 = 75 g T2 = 45°C Then, (T-45) 358 (50-T) = 758 - 1750-35T = 75T - 3375 = 35T+75T = 3375 + 1750 =) HOT - 5125 > Ta 5125 T = 40 46159°C 10 or 47°c) (or 46.6°C answer correct 47 is the most

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