# Exothermic: Thermodynamics and Data Table

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Heidi Duncan 11/24/13 Exothermic and Endothermic Reactions Lab The purpose of this lab is to observe how heat is released or absorbed with different chemicals. Data Table 1 – HCI and NaOH Trial 1 Trial 2 Avg Volume 1.0 M HCI(ml) 25 25 - Volume1.0 M NaOH (ml) 25 25 - Ti of HCI before mixing 20 20 - Ti of NaOH before mixing( 20 20 - Average Ti before mixing( 20 20 - Tf of mixture ) 26 26 - T ) 6 6 - Specific Heat (J/g) 4.184 4.184 - Heat, q (J) 1255.2 1255.2 1255.2 Data Table 2- NH4 NO3 and H20 Trial 1 Trial 2 Avg Mass of NH4 NO3 (g) 12 11.93 - Volume of H20 ( ml) 25 25 - Ti of H2O ) 20 20 - Tf of mixture ) -3 -2 - T ) -23 -22 - Specific Heat(J/g) 4.184 4.184…show more content…
Record in data table 1. Calculate the average heat (q) by averaging trials 1 and 2. Record in data table 1. Q=? M = 50g S =4.184 J/g T=26 - 20 = 6 Q=( 50g)(4.184J/g)(6=1255.2J *Both Trials had the same results 5. Classify the reaction as either exothermic or endothermic. Give evidence for your answer. -The reaction is exothermic because the temperature rose. Reaction 2 – NH4 NO3 and H20 1. Calculate the change in temperature (T) for each trial. Record in Data Table 2. Trial # Tf Ti T Trial 1 -3 20 -3 -20= -23 Trial 2 -2 20 -2- 20 -22 2. Did the temperature of the water rise or fall when the NH4NO3 was added. Explain this in terms of heat transfer. -The temperature of the water fell because the NH4NO3 absorbed the heat of the water. 3. Calculate the heat ( q in joules ) for the reaction. Record q for each trial in data table 2. Trial 1 Trial 2 Avg Q = ? Q = ? Q = ? M=25g M=25g M=25g S=4.184J/g S=4.184J/g S=4.184J/g T= -3 – 20 =-23 T=-2 -20= -22 T=-22.5 Q= (25g)(4.184)(-23)= -2405.8j Q=(25g)(4.184)(-22) = -2301.2J Q=(25g)(4.184)(-22.5)= -2353.5 4.Calculate the heat absorbed or released per gram of solute added to the water (in joules/g) record in data table 2. Calculate the average heat per gram by averaging trials 1 and 2. Trial 1 Trail 2 Avg -2405.8J/12g -2301.2 J / 11.93 g -2353.5 J /11.965 g -200 J/g -193 J/g -197 J/g 5.Classify the reaction as either exothermic or endothermic. Give evidence for