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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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
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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)
In a simple calorimeter, a piece of metal weighing 48.67 g was heated to 120.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. Is this process endothermic or exothermic? Explain. Show Your Work
In a coffee cup calorimeter, 40.0 mL of 0.33 M nitric acid (HNO3) and 40.0 mL of 0.33 M potassium hydroxide (KOH) are mixed to observe the heat released during the neutralization reaction. Based on the data in the table, what is the enthalpy of the neutralization reaction between HNO3 and KOH? Initial temperature in the calorimeter (°C) Final temperature in the calorimeter (°C) Final mass of the neutralized solution (g) Calorimeter constant (J/C)) 21.3 23.5 79.74 4.57
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
At constant volume, the heat of combustion of a particular compound, compound A, is −3046.0 kJ/mol.−3046.0 kJ/mol. When 1.753 g1.753 g of compound A (molar mass =112.07 g/mol)=112.07 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.475 ∘C.6.475 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter? Suppose a 3.771 g3.771 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.65 ∘C25.65 ∘C to 29.76 ∘C.29.76 ∘C. What is the heat of combustion per gram of compound B?