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Jul 06, 2017 · 1. Experimentally determine a specific heat. 2. Calculate ∆H for a given reaction using thermodynamic data from tables. 3. Determine ∆H experimentally for a givenreaction using a coffee cup calorimeter. 4. Predict how thermodynamic values change when varying the quantity or concentration of reactants. 5. Investigate factors that affect ΔT, q
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1) Using a graduated cylinder, add about 75.0 mL of 6.00 M HCl in the dry calorimeter. Determine the mass of the HCl solution in the calorimeter to 0.001 g, then record the temperature. 2) Weigh about 0.65 g of Zn to the nearest 0.001 g. Nov 13, 2013 · Determine the total mass of the calorimeter, m (includes the mass of the cup and everything in it), by adding the mass of the dry cup and stir bar, the mass of HCl and the mass of NaOH . Using the total mass, Δ H rxn, moles of the limiting reagent, and Δ T calculate the specific heat capacity of the calorimeter, C.
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Constant-Pressure Calorimetry. A crude constant-pressure calorimeter can be constructed from two Styrofoam coffee cups, as shown in Figure 5.8.This device, called a coffee-cup calorimeter, can be used to measure the heat exchanged between the system and surroundings for a variety of reactions, such as acid-base neutralization, heat of solution, and heat of dilution. 1. Calculate the heat absorbed by the solution in the calorimeter (assume the volumes are additive, the solution is 1.0 g·mL-1, and the specific heat of solution is the same as that of water). 2. Calculate q reaction. 3. Determine the limiting reactant of the reaction. Show the balanced equation, detailed mole
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a) Calculate ΔH (in kJ/mol NH4NO3) for the solution process NH4NO3 (s)→NH+4 (aq)+NO−3 (aq) Assume that the specific heat of the solution is the same as that of pure water. Express your answer to...1. Experimentally determine a specific heat. 2. Calculate ∆H for a given reaction using thermodynamic data from tables. 3. Determine ∆H experimentally for a givenreaction using a coffee cup calorimeter. 4. Predict how thermodynamic values change when varying the quantity or concentration of reactants. 5. Investigate factors that affect ΔT, q
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Thermodynamics I: Energy, Heat, Enthalpy. 7.2A Coffee Cup Calorimetry II – Specific heat capacity of a Metal. Subjects: Thermodynamics, enthalpy, calorimetry, specific heat. Description: Using a coffee cup calorimeter, the specific heat of a metal is experimentally determined. Materials: Two Styrofoam coffee cups – nested, with 250 mL water
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In this virtual lab, you will use coffee cup calorimetry to determine the specific heat, c, of a metal. Coffee-cup calorimeter should be rinsed and placed upside down on the lab bench, with the lid removed. Rinse off the thermometer and graduated cylinders as well. 4 (70 min) (1) Demonstration of student learning: *2 minutes for collection* Students will submit their laboratory write-up individually.
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Students will be able to calculate the amount of Calories per gram of different foods and determine the specific heat capacity of various substances through performing two virtual labs. Big Idea Calorimetry experiments allow scientists to determine the Calories per gram of various foods and determine the specific heat capacities of substances.
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ΔH = -q/1000 ÷ n (solute) = -1046/1000 ÷ 0.030 = -35 kJ mol -1. ΔH is negative because the reaction is exothermic (energy is released causing the temperature of the solution to increase). For a more detailed tutorial go to Heat of Solution tutorial.
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1) Using a graduated cylinder, add about 75.0 mL of 6.00 M HCl in the dry calorimeter. Determine the mass of the HCl solution in the calorimeter to 0.001 g, then record the temperature. 2) Weigh about 0.65 g of Zn to the nearest 0.001 g. If you used pure water, the same temperature differences would have been obtained, and since the final temperature is the same as the expected temperature, the specific heat capacity of the calorimeter must be very high (it requires a lot of energy to get hot, and hence is an insulator, and like any insulator, it won't take much heat from its ...
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How much will the temperature of a cup (180 g) of coffee at 95 °C be reduced when a 45 g silver spoon (specific heat 0.24 J/g °C) at 25 °C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same density and specific heat as water.
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It is assumed that the heat loss to the Styrofoam cup and thermometer is negligible and if the heat exchange with the environment is kept small, then the heat lost by the metal sample is equal to the total heat gained by the water. PURPOSE: To apply the experimental methods of calorimetry in the determination of the specific heat of a metal.
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identify three unknown substances using coffee cup calorimetry. Use the steps from the pre-class and in-class activities to guide your construction of the labs. Jul 31, 2013 · A coffee cup calorimeter is used to to determine the specific heat of a metal. The calorimeter is filled with 50.0 mL water (density =.997 g/mL) at 25.0 deg C. A 36.5 g metal sample is removed from boiling water (100.0 deg C) and placed in the calorimeter. The final temperature of water and sample is 32.5 deg C.
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2. When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 °C to 16.9°C. Calculate ∆H in (kJ/mol NH4NO3) for the solution process NH4NO3 (s) → NH4 + (aq) + NO 3 − (aq) Assume that the specific heat of the solution is the same as that of pure water.
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2. Calculate the heat gained by the water using Equation 1 from the Background section. The mass of water used is 50.0 g and the specific heat of water (C) is 1.0 cal/g °C. These values will give you the heat gained in calories. Q = m× C × T = 50.0 g× 1.0 cal/g°C × 5.3 °C = 265 cal. 3.
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cal is the heat capacity of the entire calorimeter (both water and hardware). However, since the “hardware” of a coffee cup calorimeter is really just a styrofoam cup, you can assume the hardware heat capacity is zero and only consider the water. Now using the specific heat of water and its mass you get Δq 4. Measure and record the mass of the empty calorimeter cup. (M c). 5. Fill the calorimeter cup about one-half full of cold water (about 5 ° below room temperature) and measure the mass of the cup and water (Mcw). Subtract the mass of the cup to obtain the mass of the water in the cup (Mw).
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In a coffee-cup calorimeter, 1.60 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.00ºC. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34ºC. Assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in kJ/mol. When a 9.55-g sample of solid NaOH dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 23.6*C to 47.4*C. Calculate Delta H (in kJ/mol NaOH) for the solution process . NaOH(s) -> Na+(aq) + OH-(aq) Assume that the specific heat of the solution is the same as that of pure water. So, I've got:
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Digby wants to determine the amount of calories in his bag of chips and hence should either look at the packaging to see or find another instrument used in measuring calories to do so. Coffee cup calorimeter and bomb calorimeter do not measure calories. While a bomb calorimeter is used to measure the amount of energy in a substance as a function of the heat that was generation in the course of combustion, coffee cup calorimeter is basically used for solution. 7 1 point A simple coffee-cup calorimeter is often used to determine the amount of heated released when an acid is neutralized by a base. When 75.0 g of 2.00 M hydrobromic acid (HBr) is neutralized with 75.0 g of 2.00 M potassium hydroxide (KOH), the temperature of the solution increases from 20.0 °C to 33.0 °C.
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A reaction known to release 1.78kJ of heat took place in a coffee cup calorimeter containing 0.100L of solution where the temp rose by 3.65 deg. C. In a second experiment, when 50.0mL of 0.20M HCl and 50.0mL of 0.20M NaOH were mixed in the same calorimeter, the temp rose 1.26 deg. C. Assume the specific heat of all the solutions is 4.18J/g deg. C.Jul 06, 2017 · 1. Experimentally determine a specific heat. 2. Calculate ∆H for a given reaction using thermodynamic data from tables. 3. Determine ∆H experimentally for a givenreaction using a coffee cup calorimeter. 4. Predict how thermodynamic values change when varying the quantity or concentration of reactants. 5. Investigate factors that affect ΔT, q
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Assume the specific heat capacity of the solution is {eq}4.18 \ J° C^{-1} g^{-1} {/eq} and that no heat is transferred to the surroundings or to the calorimeter.
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4. Measure and record the mass of the empty calorimeter cup. (M c). 5. Fill the calorimeter cup about one-half full of cold water (about 5 ° below room temperature) and measure the mass of the cup and water (Mcw). Subtract the mass of the cup to obtain the mass of the water in the cup (Mw).
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Coffee cup calorimetry, performed with calorimeters made with styrofoam coffee cups, is a familiar experiment in the general chemistry laboratory. These calorimeters are inexpensive, easy to use, and provide good insulation for most thermodynamics experiments. This paper presents the successful substitution of paper coffee cups for styrofoam cups to construct homemade calorimeters. Important ...
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A coffee cup calorimeter contains 100.0 g of water at 10.0 C. A 72.4 g sample of iron is heated to 100 C and dropped into the calorimeter. Assuming there is no heat lost to the coffee cup, calculate the final temperature of the system. The specific heats of iron and water are 0.449 J/g C and 4.184 J/g C, respectively. 1.
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In the laboratory, a "coffee cup" calorimeter or constant pressure calorimeter, is frequently used to determine the specific heat of a solid or to measure the energy of a solution phase reaction....
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Nov 23, 2016 · q­‎ = m × c × Δ T. q is the quantity of heat measured at constant pressure , m is the mass , c is the specific heat , Δ T is the change in temperature ( Δ T = T2 – T1 ) . Combustion ( bomb ) Calorimeter. Dec 20, 2015 · A coffee cup calorimeter contains 480.0 g of water at 25.0 oC. To it are added: 380.0 g of water at 53.5 oC 525.0 g of water at 65.5 oC Assuming the heat absorbed by the styrofoam is negligible, calculate the expected final temperature. The specific heat of water is 4.184 J g–1 K–1.