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Thermochemical equations are chemical equations that clearly show the relationship between mass of products and reactants and enthalpy changes. For example CH4 (g) + 202 (g) → CO2 (g) + 2H2O (1) AH = - 890.4 kJ moles of CH4 = - 890.4 kJ moles of O2 = - 890.4 kJ moles of CO2 = - 890.4 kJ moles of H20 = - 890.4 kJ - 890.4 kJ - 890.4 kJ mol - 890.4 kJ mol - 890.4 kJ mol mol Determine the heat produced in the above reaction when 1.6 grams of methane is burned in excess oxygen. Show your work! Determine the heat produced in the above reaction when 3.8 grams of oxygen is burned in excess methane. Show your work! Determine the heat produced in the above reaction when 5.2 grams of carbon dioxide is produced. Show your work! Determine the heat produced in the above reaction when 2.6 grams of water is produced. Show your work! Does the amount of heat released or absorbed depend on the mass of substance present? What is your evidence?

Thermochemical equations are chemical equations that clearly show the relationship between mass of products and reactants and enthalpy changes. For example CH4 (g) + 202 (g) → CO2 (g) + 2H2O (1) AH = - 890.4 kJ moles of CH4 = - 890.4 kJ moles of O2 = - 890.4 kJ moles of CO2 = - 890.4 kJ moles of H20 = - 890.4 kJ - 890.4 kJ - 890.4 kJ mol - 890.4 kJ mol - 890.4 kJ mol mol Determine the heat produced in the above reaction when 1.6 grams of methane is burned in excess oxygen. Show your work! Determine the heat produced in the above reaction when 3.8 grams of oxygen is burned in excess methane. Show your work! Determine the heat produced in the above reaction when 5.2 grams of carbon dioxide is produced. Show your work! Determine the heat produced in the above reaction when 2.6 grams of water is produced. Show your work! Does the amount of heat released or absorbed depend on the mass of substance present? What is your evidence?

Chemistry
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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Thermochemical equations are chemical equations that clearly show the relationship between mass of products and reactants and enthalpy changes. For example CH4 (g) + 202 (g) → CO2 (g) + 2H2O (1) AH = - 890.4 kJ moles of CH4 = - 890.4 kJ moles of O2 = - 890.4 kJ moles of CO2 = - 890.4 kJ moles of H20 = - 890.4 kJ - 890.4 kJ mol - 890.4 kJ mol - 890.4 kJ mol - 890.4 kJ mol Determine the heat produced in the above reaction when 1.6 grams of methane is burned in excess oxygen. Show your work! Determine the heat produced in the above reaction when 3.8 grams of oxygen is burned in excess methane. Show your work! Determine the heat produced in the above reaction when 5.2 grams of carbon dioxide is produced. Show your work! Determine the heat produced in the above reaction when 2.6 grams of water is produced. Show your work! Does the amount of heat released or absorbed depend on the mass of substance present? What is your evidence?
Transcribed Image Text:Thermochemical equations are chemical equations that clearly show the relationship between mass of products and reactants and enthalpy changes. For example CH4 (g) + 202 (g) → CO2 (g) + 2H2O (1) AH = - 890.4 kJ moles of CH4 = - 890.4 kJ moles of O2 = - 890.4 kJ moles of CO2 = - 890.4 kJ moles of H20 = - 890.4 kJ - 890.4 kJ mol - 890.4 kJ mol - 890.4 kJ mol - 890.4 kJ mol Determine the heat produced in the above reaction when 1.6 grams of methane is burned in excess oxygen. Show your work! Determine the heat produced in the above reaction when 3.8 grams of oxygen is burned in excess methane. Show your work! Determine the heat produced in the above reaction when 5.2 grams of carbon dioxide is produced. Show your work! Determine the heat produced in the above reaction when 2.6 grams of water is produced. Show your work! Does the amount of heat released or absorbed depend on the mass of substance present? What is your evidence?
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