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Objective: To analyze the stoichiometry of a chemical reaction involving a limiting and excess reactant.
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Limiting Reactants
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The Perfect Match
Relate the number of moles of reactant and product to one another in situations in which there is no limiting or excess reactant.
6-Row Table
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The Perfect Match, Moles on ICE, and Mass on ICE.
Moles on ICE
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Moles on ICE
Analyze the mole relationships for a chemical reaction for situations involving a limiting and excess reactant. Complete an ICE table (Initial-Change-Ending number of moles).
4 Questions
Mass on ICE
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Mass on ICE
Analyze the mass relationships for situations involving a limiting and excess reactant. Complete an ICE table (Initial-Change-Ending grams).
4 Questions
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Complete the Mole Table assuming that the two reactants are available in amounts that match the ratios given by the coefficients of the balanced chemical equation. In other words, assume no left-over or excess reactants.
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N2 + 3 H2 → 2 NH3
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The ICE Table shows the Initial # of Moles of reactants and product. Determine the Change in the # of Moles and the Ending # of Moles of the reactants and product.
The ICE Table shows the Initial Mass (in g) of reactants and product. Determine the Change in Mass (in g) and the Ending Mass (in g) of the reactants and product.
Enter mass values in grams. Enter positive values into all fields.