So, qwater = qmetal Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation. Part II: Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. Show ALL your work.
(4 points) q = m × c × Δt Given: q=? m = 34.720g c = 4.18 j/(g x °C) Δt = 41.6°C - 25.2°C = 16.4°C q = (34.720g) (4.18 j/(g x °C) (16.4°C) q = 2380.13j You are trying to figure out the energy change of the water which is the surroundings in the lab. To do that you must take the mass of the metal, which for me was Aluminum, and multiply it by the heat capacity of the water, which was given, then multiply that by the change in temperature, which is the final temperature of the mixture
Is There a Change in Temperature when an Alkali Neutralizes an Acid? Aim The aim of the experiment was to find out if there was a change in temperature when we added an alkali (Sodium Hydroxide) to an acid (Hydrochloric Acid) to neutralize it. Hypothesis We hypothesized that there was going be a raise in temperature as we add 1ml of Sodium Hydroxide at a time to the Hydrochloric Acid due to the neutralization of the acid. The neutralization is chemical reaction that causes an exothermic reaction. Sodium Hydroxide + Hydrochloric Acid Sodium Chloride + Water NaOH(aq) + HClaq → NaCl(aq) + H2O(l) Variables Independent The independent variable of the experiment was the amount of sodium hydroxide that we added to the acid.
Siddharth Rajendran Chemistry HL Urea Dissolution Lab Raw Data:- (Expected Values) Change in Enthalpy: 14 kJ mol-1 Change in Gibbs free energy: 6.86 kJ mol-1 Change in Entropy: 69.5 J mol-1 Molar Mass of Urea: 60.06 g mol-1 Heat Capacity: 4.184 J g-1º Data Table 1: To calculate the Enthalpy change Mass of Urea Tablet (g) (±0.01g) | Volume of Water(mL) (±0.05mL) | Initial Temperature (Cº) (±0.2 Cº) | Final Temperature(Cº) (±0.2 Cº) | 3.04 | 50.0 | 21.3 | 17.4 | Initial Observations:- * There was a decrease in temperature at a fast rate. * The temperature of the solution was slowing down continuously but the rate started decreasing. * The Urea dissolved and the rate was decreasing continuously. * The temperature gradually started to increase after almost the Urea present had dissolved. Data Table 2: Mass, Volume and Temperature during Dissolution of Urea (To calculate Keq) Mass of Urea(g) (±0.01g) | Initial Temperature(Cº) (±0.2 Cº) | Final TemperatureCº) (±0.2 Cº) | Initial Volume(mL)(±0.05 mL) | Final Volume(mL)(±0.05 mL) | 3.76 | 21.4 | 22.9 | 5.02 | 7.14 | Processing Raw Data * Determining the Final temperature of dissolution of Urea in the Styrofoam cup.
Then prepare the unknown sample by pipetting 1 ml of the unknown solution into the cuvette and mix with 1 ml of dilute ferric nitrate. Then after that you calculate the concentration for each of the solutions. Cuvette # | 25 mg/dl Standard | H2O ml | Dilute Iron III Nitrate (ml) | .039 M HNO3 (ml) | Concentration | 1 | 0 | 1 | 0 | 1 | 0 | 2 | 0.1 | 0.9 | 1 | 0 | 0.09 | 3 | 0.3 | 0.7 | 1 | 0 | 0.287 | 4 | 0.5 | 0.5 | 1 | 0 | 0.407 | 5 | 0.7 | 0.3 | 1 | 0 | 0.706 | 6 | 1 | 0 | 1 | 0 | 1.316 | When then use the calibration curve to determine the concentration of the unknown and we get .747. IV. As you can see from our data as the amount of H2O decreases and the 25mg/dl standard increases as does our concentration for the salicylic acids.
Purpose: The purpose of this lab is to verify Hess’s Law of Additivity of Reaction Enthalpies Chemical Reaction/Physical Reaction: 1.) Na(aq) + OH(aq) -> NaOH(s) 2.) NaOH + HC2H3O2(aq) -> H2O(l) + Na(aq) + C2H3O2 3.) Na(aq) + OH(aq) + HC2H3O2(aq) -> H2O(l) + Na(aq) + C2H3O2 List of Materials:Digital Thermometer, foamed polystyrene cups (3), 250 mL beaker,Weighing boat or small beaker, Graduated cylinders, 100mL(1), 25 mL(2),sodium hydroxide pellets, sodium hydroxide 2.0M, Acetic acid 1.0M and 2.0M. Safety Considerations: Always have safety goggles covering your eyes, do not inhale the fumes of chemicals used.
300 mL of tap water in a 400 mL beaker was placed on a hot plate and warmed. Once the water was hot, the beaker still remained on the hot plate to maintain the hot temperature. 7. An ice-water bath was created using a second 400 mL beaker. 8.
Chemistry 3/19/13 Calorimetry Lab Report Purpose: Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical purposes. The purpose of this lab was to use calorimetry to find how much heat is absorbed or released when NaCl is dissolved in water. In this case, we will find the heat coming out of the system, in a chemical process. Hypothesis: Once the sodium chloride is put into the water, the temperature of the water will rise. Procedure: 1.
The reaction of water and carbon dioxide is catalyzed by You correctly answered: a. carbonic anhydrase. 03/12/13 page 1 Experiment Results Predict Question: Predict Question: What do you think will happen to the pH and PCO2 levels with hyperventilation? Your answer : c. pH will increase and PCO2 will decrease. Stop & Think Questions: Were the pH and PCO2 in the normal range? You correctly answered: c. Both pH and PCO2 were in the normal range.
Observation: The temperature of acid and base are the same (room temperature). When start to pouring NaOH into HCl, the temperature increases rapidly. Chemical Equation: NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) Calculations: (Stapled together, at the back of Data Sheet 2) Results: (Stapled together) Conclusion: We always find the heat of neutralization when we mix acid with base. The heat is the proof for the forming of H2O. We know it exists but we can’t find the way to measure it.