You weigh a dry flask, and place a chunk of solid into it, then weigh it again. You then fil the flask to the top with water and weigh the full flask Finally, you take the solid out, fil the flask to the top with water and weigh it once more. Mass of flask in g) 56.89 Mass of flask plus solid (e) 133.6 Mass of flask plus solid and water (g) 146.26 Mass of flask filled with water Ig) 84.54 Density of water at the measured water temperature (g/cc) 0.992 Calculate the following Volume of the flask (not occupied by the solid) in (cc)

You weigh a dry flask, and place a chunk of solid into it, then weigh it again. You then fil the flask to the top with water and weigh the full flask Finally, you take the solid out, fil the flask to the top with water and weigh it once more. Mass of flask in g) 56.89 Mass of flask plus solid (e) 133.6 Mass of flask plus solid and water (g) 146.26 Mass of flask filled with water Ig) 84.54 Density of water at the measured water temperature (g/cc) 0.992 Calculate the following Volume of the flask (not occupied by the solid) in (cc)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 119QRT

See similar textbooks

Similar questions

A 11.2-g copper block, initially at 75.0 °C, is dropped into a Thermos flask containing 26.6 g of water initially at 7.71 °C. What is the final temperature of the Thermos flask contents?
In a freezer 160 g a water of zero Celsius is place in an ice cube tray how much he and kilo calories must be removed removed to form ice cubes at zero Celsius
A sample of solid copper is heated with an electrical coil. If 68.1 Joules of energy are added to a 12.2 gram sample and the final temperature is 35.5°C, what is the initial temperature of the copper?_______ °C.
Copper is sometimes coated on the bottom surface of cooking pans. Copper has a specific heat of 0.385 J/g∘CJ/g∘C. A 25.3 gg sample of copper heated to 86.0 ∘C∘C is dropped into water at an initial temperature of 13.6 ∘C If the final temperature reached by the copper-water mixture is 35.9 ∘C∘C, how many grams of water are present?
4. A 8.33 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. a. What is the total mass inside the calorimeter in grams? b. What is the change in temperature, in °C, inside the calorimeter? c. Was the dissolution process endothermic or exothermic? d. What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g･ °C. e. What is the total heat for the dissolution reaction of the 8.33 g of salt? f. What quantity in moles of the unknown salt were used in the reaction? g. What is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
by looking at the graph below, which section shows where the substance has the lowest average kinetic energy ?
a) Calculate the number of calories given off by 300 g of water cooling from 25 deg. C to 10 deg. C. b) What are 25 deg. C and 10 deg. C in Fahrenheit. 1 calorie = 4.184 J
What is the value of the final Temperature when 1g of silver 100 degrees Celsius is added to 50g of water 20 degrees Celsius
3.) Acetone (C3H6O) is quite flammable. If a bottle of nail polish (187 mL) burns, how muchheat is released? The density of acetone is 0.788 g/mL.C3H6O9(l) + 4 O2(g) 3 CO2(g) + 3 H2O(g) Hrxn = -1790 kJ I already solved number three and I got -4541.57kJ. I need help with question 4 (both questions connect) 4.) For problem 3, explain if the reaction is exothermic or endothermic, spontaneous or non spontaneous, and if the entropy of the system increases or decreases. Is there an activation energy? Is the reaction spontaneity temperature dependent? Explain.
When ignited, solid ammonium dichromate decomposes in a fiery display. This is the reaction for a "volcano" demonstration. The decomposition produces nitrogen gas, water vapor, and chromium(III) oxide. The temperature is constant at 25°C. Substance DHf° (kJ/mol) S° (kJ/mol K) Cr2O3(g) –1147 0.08118 H2O(l) –242 0.1187 N2(g) 0 0.1915 (NH4)2Cr2O7(s) –22.5 0.1137 Determine DSuniv° (in kJ/mol K) and the spontaneity of this reaction.
78. Calculate the amount of heat required to heat a 3.5-kg gold bar from 21 °C to 67 °C.
How much heat is gained by nickle when 500 grams of nickle is warmed from 22.4 to 58.4 degrees Celsius