Use the following information to answer the next question. Calcium carbonate as many uses including in the oil industry it is as a weighting material to increase the density of drilling fluids. Calcium carbonate decomposes according to the following reaction equation: CaCO3(s)→ CO₂(g) + CaO(s) The standard enthalpy of reaction for the reaction shown above is + + kJ. Record your 4-digit answer. Include sign; do not include units.

Use the following information to answer the next question. Calcium carbonate as many uses including in the oil industry it is as a weighting material to increase the density of drilling fluids. Calcium carbonate decomposes according to the following reaction equation: CaCO3(s)→ CO₂(g) + CaO(s) The standard enthalpy of reaction for the reaction shown above is + + kJ. Record your 4-digit answer. Include sign; do not include units.

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

Acetylene, C,H,, is used in welding torches. It releases a lot of energy when burned in oxygen. The combustion of one gram of acetylene releases 48.2 kJ. A 0.750-gram sample of acetylene is burned in a bomb calorimeter (heat capacity = 1.117kJ/°C) that contains 800.0 g of water. The final temperature of the bomb and water after combustion is 35.2°C. What is the initial temperature of the bomb and water?
Propane reacts with oxygen gas to produce carbon dioxide and water as shown in the reaction below. How much energy in kJ will be released if 500 kg of propane is burned in the air? C3H8 + 50₂ 3CO₂ + 4H₂0 AH = -2221 kJ
When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175.0 g of water was placed in a coffee-cup calorimeter and chilled to 10.0 °C. Then 49.0 g of pure sulfuric acid, also at 10.0 °C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9 °C. Assume that the specific heat capacity of the resulting sulfuric acid solution is 4.19 J/g °C. Calculate the quantity of thermal energy transferred, Q, for the formation of this solution, and calculate the molar enthalpy of solution in kilojoules per mole of H₂SO4.
Please don't provide handwriting solution
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).
A 88.8 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 24.8°C. Ignoring significant figures, calculate the mass of water in the calorimeter.
Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 38.7 °C. During the reaction 55.6 kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is -1 4.18 J∙g¯¹·K¯¹. Be sure your answer has the correct number of significant digits. 心。 °℃ x10 S
An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.73 kj/°c. When a 0.26-g sample is used, the temperature change is 10.5°C. What is the energy density of the sample in k/g? Round your answer to 2 decimal places.
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.57 kg sample of a pure substance from 18.0 °C to 35.9 °C. The experiment shows that 19. 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. - 1 - 1 •K J. g x10
When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature of the water rises from 21.6 to 37.8oC. Was the chemical reaction (dissolving the solid) endothermic or exothermic? How do you know? Write a balanced chemical equation for this process. Determine how many joules of heat (q) were involved in changing the temperature of the water. If the heat that changed the temperature of the water was a result of the chemical reaction, determine the ΔH of the chemical reaction in kJ/mol of sodium hydroxide.