A 23.7g sample of a metal was heated to 61.67 C. When the metal was placed into 24.1g of water in a calorimeter, the temperature of the water increased from 25.00'C to 30.00°C. What is the specific heat of the metal? The specific heat of water is 4.18 g "C). Specific beat = Submit Answer Try Another Version 1 hem attempt remaining

A 23.7g sample of a metal was heated to 61.67 C. When the metal was placed into 24.1g of water in a calorimeter, the temperature of the water increased from 25.00'C to 30.00°C. What is the specific heat of the metal? The specific heat of water is 4.18 g "C). Specific beat = Submit Answer Try Another Version 1 hem attempt remaining

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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K Question 8 of 13 Macmillan Learning qwater = How much heat did the metal lose? qmetal > A student places a block of hot metal into a coffee cup calorimeter containing 152.0 g of water. The water temperature rise from 23.3 °C to 34.7 °C. How much heat (in joules) did the water absorb? OO E HUAWEI P30 LEICA TRIPLE CAMERA Resources Ex Give Up? N Hint Check Answer 7:37 PM 11/20/2022 ☐
A coffee-cup calorimeter contains 60 mL of water with an initial temperature of 24.9°C. An unknown sample with a mass of 15.963 grams was placed inside making the water temperature rise up to 25.5°C. The initial temperature of the metal was 69.8°C. 1. How much heat was absorbed by the water in the calorimeter? (round off final answer to 2 decimal places)
A chemical reaction is performed in a solution with a mass of 125.0 g, a specific heat of 4.184 J/g°C, and an initial temperature of 22.44°C. After mixing the two reactants in the solution, the temperature of the solution decreases to 18.62°C. What is qrxn in kJ? Show your work. Round your final answer to four significant figures. Type your answer... Previous Next
Hi there, I was working through some questions and want to know if I am doing them right, there was no answer sheet attached to the practice questions and just want to make sure I understand how to do these types of questions 1. A metal weighing 30 g absorbs 200.0 J of heat when its temperature increases by 80.0°C. What is the specific heat capacity of the metal? c=J/g°C c=200J/ (30g)(80°C) = 0.083J/g °C Therefore the specific heat capacity of the metal is 0.083J/g°C 2. Calculate the mass (in grams) of iron that could be warmed from 20°C to 65°C by applying 4.5 kJ of energy. The specific heat capacity of iron is 0.45 J/g•°C. 4.5kJ = 4,500 J q = mcΔT m = 4,500 J(0.45J/g°C)(65°C - 20°C) m = 222g Therefore the mass of iron is 222g 3. How much heat in kilojoules is released when 500.0 g of water is cooled from 85.0ºC to 10.0ºC? The specific heat capacity of water is 4.184 J/(g•°C). q = mcΔT q = (500g)(4.184 Jg°C) (10ºC - 85ºC) = -156,900 kJ Therefore the amount of heat released…
I Review I Use the heat equation to calculate the energy for each of the following (see the table): Specific Heats for Some Substances Part A cal/g °C J/g°C Substance Elements calories to heat 9.0 g of water from 15 °C to 31 °C Express your answer to two significant figures and include the appropriate units. Aluminum, Al(s) Copper, Cu(s) Gold, Au(s) Iron, Fe(s) Silver, Ag(s) 0.214 0.897 0.0920 0.385 HẢ ? 0.0308 0.129 0.108 0.452 Ω % (X) 0.0562 0.235 Titanium, Ti(s) 0.125 0.523 Value Units Compounds Ammonia, NH3 (g) Ethanol, C2HsO(1) 0.488 2.04 Submit Previous Answers Request Answer 0.588 2.46 Sodium chloride, NaCl(s) Water, H20(1) Water, H20(s) 0.207 0.864 X Incorrect; Try Again; 2 attempts remaining 1.00 4.184 0.485 2.03 Part B
SIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 7. Given the following reactions N2(g) + O2(g) → 2NO(g) ΔH = +180.7 kJ 2N2O(g) → O2(g) + 2N2(g) ΔH = -163.2 kJ Determine the enthalpy of reaction: 2N2O(g) → 2NO(g) + N2(g).
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The molar heat of combustion of a compound is 1,408 kJ/mol. If 0.600 moles of this compound was burned in a bomb calorimeter containing 1,544 g of water, what would be in the increase of the temperature be? Specific heat of water is 4.184 J/mol. Answer to 1 decimal place Your Answer: Answer
For Lab 4 Energy of food content Experiment, use the following data. The specific heat (Water) is 1.00 cal/g°C. Make sure to fill up all of the Table 1, 2, 3, 4 such as your post-lab report. a) What is Average energy content of sample (Cal/g)? b) What is Theoretical energy content of sample (Cal/g)? c) What is the Percent Error (%) of Experimental energy content of sample?
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