### Heat Energy Calculation**Problem Statement:**Calculate the energy required to heat 513.0 mg of mercury from 0°C to 10.0°C. Assume the specific heat capacity of mercury under these conditions is 0.139 J·g⁻¹·K⁻¹. Be sure your answer has the correct number of significant digits.**Inputs and Explanation:**- **Mass of mercury (m):** 513.0 mg (which needs to be converted to grams because the given specific heat capacity is in J·g⁻¹·K⁻¹)- **Initial temperature (T₁):** 0°C- **Final temperature (T₂):** 10.0°C- **Specific heat capacity (c):** 0.139 J·g⁻¹·K⁻¹**Conversion:**1 mg = 0.001 g So, 513.0 mg = 513.0 * 0.001 g = 0.513 g**Formula to use:**The energy required (Q) can be calculated using the formula:\[ Q = m \cdot c \cdot \Delta T \]Where:- \( Q \) is the heat energy (in joules, J)- \( m \) is the mass (in grams, g)- \( c \) is the specific heat capacity (J·g⁻¹·K⁻¹)- \( \Delta T \) is the change in temperature (T₂ - T₁) (in Celsius or Kelvin, K since the difference in temperature in Celsius and Kelvin is the same)**Calculation:**1. Calculate the change in temperature (ΔT):\[ \Delta T = T₂ - T₁ = 10.0°C - 0°C = 10.0 K \]2. Substitute the values into the formula:\[ Q = 0.513 \, \text{g} \times 0.139 \, \text{J·g}^{-1} \text{·K}^{-1} \times 10.0 \, \text{K} \]\[ Q = 0.513 \times 0.139 \times 10.0 \]\[ Q = 0.71307 \text{ J} \]**Result:**\[ Q = 0.713 \

Formula used q = mCdT Where q = heat energy ; m = mass of mercury C = specific heat capacity; dT =…

Calculate the energy required to heat 513.0 mg of mercury from 0 °C to 10.0 °C. Assume the specific heat capacity of mercury under these conditions is 0.139 J-g K Be sure your answer has the correct number of significant digits. ロロの

Calculate the energy required to heat 513.0 mg of mercury from 0 °C to 10.0 °C. Assume the specific heat capacity of mercury under these conditions is 0.139 J-g K Be sure your answer has the correct number of significant digits. ロロの

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 sheet of gold weighing 9.0 g and at a temperature of 13.8 °C is placed flat on a sheet of iron weighing 20.2 g and at a temperature of 57.8 °C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. Be sure your answer has the correct number of significant digits. GC ☐ x10 ☑ ملام 18 Ar 日。 ☑
Maritza Using specific heat capacity to find heat Calculate the energy required to heat 1.50 kg of water from 40.4 °C to 48.9 °C. Assume the specific heat capacity of water under these conditions is 4.18 J g -1 -1 K. Round your answer to 2 significant digits. x10
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 2.30 kg of water at 35.8 °C. During the reaction 74.9 kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions 1 is 4.18 J.g •K`1 ▪ Be sure your answer has the correct number of significant digits.
Calculate the energy required to heat 775.0 mg of iron from 0.5 °C to 11.2 °C. Assume the specific heat capacity of iron under these conditions is 1 0.449 J.g K Round your answer to 3 significant digits. 0 ロ・ロ X μ
1,922 Joules of heat are added to 42.5 grams of water, initially at 20∘C. What is the final temperature of the water?
A 0.2415 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 The temperature increases by 1.978 °C. Part 1 of 2 kJ Calculate the heat associated with the burning of Mg in Be sure your answer has the correct number of significant digits. g Part 2 of 2 kJ g ☐ x10 ☑ Calculate the heat associated with the burning of Mg in kJ mol Be sure your answer has the correct number of significant digits. KJ mol x10 ☑
The work done to compress a gas is 69.0 J. As a result, 29.0 J of heat is given off to the surroundings. Calculate the change in energy of the gas. Be sure your answer has the correct number of significant digits. J ☐x10
be sure your answer is correct and have the correct number of significant digits
how much energy in joules is needed to heat 200.0 g of water by 10.0 degrees celsius? the heat capacity of water is 4.185 joules/grams x degrees celsius
Calculate the energy required to heat 718.0 mg of water from 46.0 °C to 56.7 °C. Assume the specific heat capacity of water under these conditions is -1 -1 4.18 J∙g¯¹·K-¹ Be sure your answer has the correct number of significant digits. 0 x10 X μ 010 ? 00. 18 Ar
A chemist carefully measures the amount of heat needed to raise the temperature of a 284.0 mg sample of a pure substance from 51.6 °C to 61.2 °C. The experiment shows that 13. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. - 1
Calculate the energy required to heat 1.10 kg of water from 49.1 °C to 62.6 °C. Assume the specific heat capacity of water under these conditions is 4.18 J-g ¹K¹. Round your answer to 3 significant digits. 1 H X 10 S 5 ob Ar