1. A 32.07 gram sample of vanadium was heated to 75 deg. It was then dumped in which the initial temperature of the water inside was 22.50 deg C. After the metal was allowed to release its heat to the calorimeter's water, 26.30 deg C was read to be the final temperature. What is the mass (g) of the water inside the calorimeter? Specific heat capacity of water and vanadium is 4.184 and 0.4886 J/g-C, respectively.

1. A 32.07 gram sample of vanadium was heated to 75 deg. It was then dumped in which the initial temperature of the water inside was 22.50 deg C. After the metal was allowed to release its heat to the calorimeter's water, 26.30 deg C was read to be the final temperature. What is the mass (g) of the water inside the calorimeter? Specific heat capacity of water and vanadium is 4.184 and 0.4886 J/g-C, respectively.

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...

See similar textbooks

Similar questions

A bomb calorimeter has a heat capacity of 2.47 kJ/?. When a 1.00 mol sample of a certain hydrocarbon was burned in this calorimeter, the temperature increased by 2.14?. Calculate the heat of combustion per mole of the hydrocarbon.
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
An 84.01 g sample of water at 88.2 °C is mixed in a calorimeter with 43.6 g of water at 23.4 °C. Calculate the final temperature of the water.
A 0.602-g sample of isophthalic acid (C8H604) is burned in a bomb calorimeter and the temperature increases from 24.80 °C to 27.05 °C. The calorimeter contains 1.01x10³ g of water and the bomb has a heat capacity of 936 1/°C. The heat capacity of water is 4.1843 g ¹¹. Based on this experiment, calculate AE for the combustion reaction per mole of isophthalic acid burned. 9 kJ/mol
7. In a calorimeter, 50.00 mL of 2.50 M NaOH was combined with 50.00 mL of 2.25 M HCI to form a solution. The temperature of the solution went from 20.0 °C to 36.0 °C. The heat capacity of the solution is 4.184 J/g°C. Assume a density of 1.00 g/mL Determine the AHneutzn of HCI.
1. A certain two-step process involves transfer of heat and work between the system and the surroundings. In the first step, the internal energy, AE, of the system increases by 115.4 J when 95.1 J of work is done on the system. In the second step, the internal energy of the system decreases by 32.2 J when 15.6 J of work is done on the surroundings. In the first step of the two-step process, how much heat, in Joules, was absorbed or released? b. How much heat, in Joules, was absorbed or released in the whole two-step process? a.
In parts 2, 3 and 4 of this lab, you will be conducting calorimetry experiments on neutralization reactions in solution. Two solutions (each of volume 2.5 mL) will be mixed together to initiate the reaction. What mass of water should be used in the calculation of the heat energy absorbed by the calorimeter? 2.5 g 5.0 g (since the two solutions are mixed together, the volumes and hence their masses are added together).
A sample of copper was heated to 120o C and then plunged into an insulated vessel containing 200.g of water at 25.00o C. The final temperature of the mixture was 26.50o C. Assuming no heat was lost to the surroundings, calculate the mass of the copper sample. The specific heat of copper is 0.385 J/go C and the specific heat of water is 4.184 J/go C.
A 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The specific heat capacity of copper metal and water are J and 4.184 J respectively. g• °C 0.387 g• °C Assuming that heat was transferred from the copper to the water and the calorimeter, determine th heat capacity of the calorimeter. Heat capacity of calorimeter =
A 350.0 g iron pot is heated on a stove for a period of time until it is hot. The stove is turned off and 516 g of cold water (10.0 °C) is added to the pot. When thermal equilibrium is reached, the temperature of the water is 28.4 ° C. What was the initial temperature of the iron pot, assuming heat was exchanged between these two objects and none was lost to the surroundings? (The specific heat capacity of iron is 0.450 J/g °C. The specific heat capacity of water is 4.184 J/g °C) Give only the numerical answer in the box and not units. Give 4 sig figs in your answer. Show the calculations for the problem by writing it on a paper, upload the image file/pdf file in the question for file upload.
A sample of copper with a specific heat of 0.385 J goC is heated from 45.6 oC to 80.7 oC. What is the mass of the copper sample if this process required 816.24 J of energy?
A 29.00 g sample of metal alloy is heated to 92.6 °C; then placed in 55.23 g of water in an insulated calorimeter at 21.3 °C. If the final temperature of the system is 43.9 °C, what is the specific heat of the metal alloy? Assume that the calorimeter absorbs a negligible amount of heat.