**Thermochemistry: Calculating Specific Heat Capacity**A chemist carefully measures the amount of heat needed to raise the temperature of an 860.0 g sample of a pure substance from 14.8 °C to 22.4 °C. The experiment shows that 4.6 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits.**[ ] J·g⁻¹·K⁻¹**In this task, you are required to calculate the specific heat capacity. Use the formula:\[ q = m \cdot c \cdot \Delta T \]where:- $ q $ is the heat added (4.6 kJ = 4600 J),- $ m $ is the mass of the sample (860.0 g),- $ c $ is the specific heat capacity,- $ \Delta T $ is the change in temperature (22.4 °C - 14.8 °C = 7.6 °C).Solve for $ c $ and enter your result in the provided unit format.

O THERMOCHEMISTRY Griffin Calculating specific heat capacity A chemist carefully measures the amount of heat needed to raise the temperature of a 860.0 g sample of a pure substance from 14.8 °C to 22.4 C. The experiment shows that 4.6 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. II

O THERMOCHEMISTRY Griffin Calculating specific heat capacity A chemist carefully measures the amount of heat needed to raise the temperature of a 860.0 g sample of a pure substance from 14.8 °C to 22.4 C. The experiment shows that 4.6 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. II

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

11 A chemist carefully measures the amount of heat needed to raise the temperature of a 192.0 g sample of C4H₁1 N from -9.6 °C to 7.4 °C. The experiment shows that 7.86 x 10³ J of heat are needed. What can the chemist report for the molar heat capacity of CH₁,N? Round your answer to 3 significant digits. -1 -1 J. J.mol¹¹.K x10 X $ ?
Calculate the energy required to heat 511.0 g of silver from 10.8 °C to 19.9 °C. Assume the specific heat capacity of silver under these conditions is - 1 -1 0.235 J'g K your answer to 2 significant digits. Round x10
In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a metal.She heats 19.2 grams of magnesium to 98.96°C and then drops it into a cup containing 77.8 grams of water at 22.66°C. She measures the final temperature to be 27.15°C.Assuming that all of the heat is transferred to the water, she calculates the specific heat of magnesium to be ________ J/g°C.
A backpacker wants to carry enough fuel to heat 2.4kg of water from 25 C to 100.0 C. If the fuel he carries produces 36 kJ of heat per gram when it burns, how much fuel should he carry? (Assume that the transfer of heat is 100% efficient)
A chemist carefully measures the amount of heat needed to raise the temperature of a 517.0mg sample of a pure substance from −4.5°C to 13.7°C . The experiment shows that 2.21J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits.
Calculate the energy required to heat 668.0 g of ethanol from 1.3 °C to 16.2 °C. Assume the specific heat capacity of ethanol under these conditions is - 1 1 2.44 J.g .K Round your answer to 3 significant digits. 0 x10 ロ・ロ X μ 00
A student measures the following data regarding the heat of fusion of ice: 24.8 g ice at 0.0°C is placed into the calorimeter which contains 100.0 g water at 21.5°C. The final temperature comes to 2.0°C. The calorimeter has a heat capacity of 15.4 J/°C.
A 325.7 gram sample of copper is initially at 20.8 °C, and it absorbs 17.88 kJ of heat from its surroundings. What is its final temperature? (specific heat = 0.387 J g¹ °C-1 for copper) Do not put units in your answer. Give your answer to one decimal place.
A chemist carefully measures the amount of heat needed to raise the temperature of a 712.5 g sample of a pure substance from 22.1 degrees Celsius to 38.2 degrees Celsius. The experiment shows that 55.7 kJ of heat are formed. Calculate the specific heat capacity of this substance in J/gC. Report your answer with the proper amount of significant figures and no unit.
Part A If 52 J of heat is added to an aluminum can with a mass of 29.1 g , what is the temperature change? The specific heat capacity of aluminum is 0.903 J/g°C. Express your answer using two significant figures. ΑΣφ AT = °C
A 25.0g piece of aluminum sits in a room and cools. It loses 4300.0 J of heat. If the initial temperature of aluminum is 125.3°C, what is the final temperature? The specific heat capacity of aluminum is 0.900 J/g°C.
A sample of copper absorbs 4.41E1 kJ of heat, resulting in a temperature rise of 6.21E1 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C. (using coffee cup)