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. A chunk of platinum weighing 19.07 grams and originally at 97.71 °C is dropped into an insulated cup containing 79.75 grams of water at 20.99 °C Thermometer Stirring rod The heat capacity of the calorimeter (sometimes referred to as the calorimeter Water constant) was determined in a separate experiment to be 1.60 J/OC Metal sample e2003 Thomson-Brooks/Cols Using the accepted value for the specific heat of platinum (See the References tool) calculate the final temperature of the water. Assume that no heat is lost to the surroundings

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. A chunk of platinum weighing 19.07 grams and originally at 97.71 °C is dropped into an insulated cup containing 79.75 grams of water at 20.99 °C Thermometer Stirring rod The heat capacity of the calorimeter (sometimes referred to as the calorimeter Water constant) was determined in a separate experiment to be 1.60 J/OC Metal sample e2003 Thomson-Brooks/Cols Using the accepted value for the specific heat of platinum (See the References tool) calculate the final temperature of the water. Assume that no heat is lost to the surroundings

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. The heat of the solution of a solid sample was determined using a coffee cup calorimeter that contains 250ml of water initially at 25C. As the sample is dissolved in the water, the temperature of the water decreased to 11C. What is the heat of the solution of the sample? Assume that the density of water is 1.00g/ml and that the coffee cup is a good insulator. Is the process endothermic or exothermic?
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. Thermemeter trng o A student heats 61.30 grams of lead to 98.08 °C and then drops it into a cup containing 82.53 grams of water at 22.76 °C. She measures the final temperature to be 24.74 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.88 J/ °C. Witer Assuming that no heat is lost to the surroundings calculate the specific heat of lead. Meal mple Specific Heat (Pb) = J/g°C. Submit Answer Retry Entire Group 8 more group attempts remaining
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. A student heats 65.54 grams of copper to 98.08 °C and then drops it into a cup containing 78.67 grams of water at 23.78 °C. She measures the final temperature to be 29.26 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Specific Heat (Cu) = J/g°C.
nuraipy changes in chemical reactions Read through pages 18-20 in your laboratory manual for information on how to calculate the enthalpy change in a solution. Part A - Calculating ms In a calorimetry experiment 5.6 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 °C. The effective mass of the glass in the thermos flask (mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-¹K-1¹. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-¹K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Calculate the total mass of solution in kilograms (ms) Give your answer to four significant figures. ▾ View Available Hint(s) Hint 1. Calculating ms mg = mass water (kg) + mass solute (kg) —| ΑΣΦ Submit Request Answer ? kg < Pear 10
Thermometer 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. Stiring md A student heats 63.29 grams of nickel to 97.88 °C and then drops it into a cup containing 76.34 grams of water at 21.12 °C. She measures the final temperature to be 27.55 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.60 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of nickel. Metal- sample at Specific Heat (Ni) = J/g°C. 2003 Thomwan-drookaCole ot pt Submit Answer Try Another Version 3 item attempts remaining Previous Next Save and Exit nt Cengage Learning | Cengage Technical Support MacBook Pro
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to Thermometer measure the energy of a solution phase reaction. Stirring rod A student heats 64.79 grams of iron to 97.64 °C and then drops it into a cup containing 83.33 grams of water at 20.56 °C. She measures the final temperature to be 26.59 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.63 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of iron. Metal sample Specific Heat (Fe) = J/g°C. 2000 Thomson-BrooksCole
A calorimeter contains 140 g water. The calorimeter and the water inside are both at 24 °C. A piece of metal weighing 45 g was heated to 98 °C and then put into the water inside the calorimeter. The equilibrium temperature was determined to be 35 °C. Assuming no heat is lost to the environment, calculate the specific heat of the metal. Calorimeter constant: 130 J°C-1 Specific heat of water: 4.184 J°C*g1 O A. 2.26 J°C-lg1 O B. 2.78 J°Clg-1 oc.1.81 J°Cg1 O D.193 J°C-lg1 O E. 2.37 J°C-1g-1
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 1.44 g of CaClh(s) are dissolved in 104.80 g of water, the temperature of the solution increases from 24.43 to 26.88 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CaCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol
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A 77.5g piece of brass is heated so that its temperature is 98.7◦C. Next,it is quickly placed in a calorimeter containing 102.76 g of water at 18.5◦C.Knowing that the final temperature is 23.5◦C, what is the specific heat of this alloy?Note: Brass is an alloy of copper and zinc. From 98.7 to 23.5◦C, this alloy does not changeno phase, it remains in solid form.
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. Thermometer Stirring rod A student heats 66.89 grams of platinum to 99.25 °C and then drops it into a cup containing 83.90 grams of water at 22.41 °C. She measures the final temperature to be 24.37.°C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.72 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of platinum. Metal sample Specific Heat (Pt) =| J/g °C. 02003 Thomeo-BrockaCoe
A student mixed 50.0 mL of water containing 0.010 moles of HCI (weighing 50.0 g) with 60.0 mL of water containing 0.012 moles of NaOH (weighing 60.0 g) in a coffee cup calorimeter. Both solutions were initially at 25.00°C, but after reaction upon mixing the temperature rose to 26.20°C. The specific heat of the solution is the same as that of water, 4.18 J/g °C, and the calorimeter has a heat capacity of 35 J/°C. The reaction is shown below. (a) How much heat is produced in the reaction? (b) How much heat is produced if one mole of water is formed in this chemical reaction? HCl(aq) + NaOH(aq) → NaCl(aq) + H20(l)