Consider the following potential energy diagrams for two different reactions.
Which plot represents an exothermic reaction? In plot a, do the reactants on average have stronger or weaker bonds than the products? In plot b, reactants must gain potential energy to convert to products. How does this occur?
Answer to relevant QuestionsConsider a sample containing 2.00 moles of a monatomic ideal gas that undergoes the following changes: For each step, assume that the external pressure is constant and equals the final pressure of the gas for that step. ...A biology experiment requires the preparation of a water bath at 37.0oC (body temperature). The temperature of the cold tap water is 22.0oC, and the temperature of the hot tap water is 55.0oC. If a student starts with 90.0 g ...The heat capacity of a bomb calorimeter was determined by burning 6.79 g of methane (energy of combustion = –802 kJ/ mol CH4) in the bomb. The temperature changed by 10.8oC. a. What is the heat capacity of the bomb? b. A ...Given the following data: 2ClF(g) + O2(g) → Cl2O(g) + F2O(g) ΔH = 167.4 kJ 2ClF3(g) + 2O2(g) → Cl2O(g) + 3F2O(g) ΔH = 341.4 kJ 2F2(g) + O2(g) → 2F2O(g) ΔH = –43.4 kJ Calculate ΔH for the reaction ClF(g) + F2(g) ...The combustion of methane can be represented as follows: a. Use the information given above to determine the value of ΔH for the combustion of methane to form CO2(g) and 2H2O(l). b. What is ΔHof for an element in its ...
Post your question