Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate (CaCO3) at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one particular reaction, 70 g of CaCO3 is heated at 600°C in a 5.0 L vessel. The pressure of CO2 is 0.20 atm after 3.0 minutes. What is the average rate of CO2 production in moles per minute during the 3 minutes? (Enter in mol/min.)   If you assume this rate of decomposition remains constant, how many minutes will it take for the entire sample of CaCO3 to decompose?

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Q: In the synthesis of ammonia, if -A[H2]/At = 4.7 x 10-4 mol/L · min, what is ANH3]/At? N2 (g) + 3 H2…

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Q: Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate…

A: Given: Volume = 5.0 L Mass of calcium carbonate = 30 g Pressure = 0.13 atm Temperature = 500°C…

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A: Use definition of the equilibrium and the Le-chatelier principle to find the rate of the reaction.

Q: Consider the combustion of ethane: 2C2H6(g)+ 7O2(g) ---> 4CO2 (g) + 6H2O(g) If the ethane is…

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Q: Find A[F2]/At Express your answer to two significant figures and include the appropriate units. HẢ ?…

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Q: One reaction that occurs in an automobile catalytic converter is the conversion of nitrogen monoxide…

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Q: Part A Consider the following data for the gas-phase decomposition of NO2: 2NO2 (9) → 2NO (9) + O2…

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Q: The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g) + ½ O₂(g) is second order…

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Q: given: 2O3 (g) --> 3O2 if the rate of O3 loss is 3.91 x10^-1 what is the rate of formation of O2

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