calculate how many moles of CaCl2•2H2O are present in 1.0 g of CaCl2•2H2O and then calculate how many moles of pure CaCl2 are present in the 1.0 g of CaCl2•2H2O

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  1. mols CaCl2.2H2O = grams/molar mass = ?

    There is 1 mol of CaCl2 in 1 mol CaCl2.2H2O

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  2. Nitrogen dioxide reacts with water to produce oxygen and ammonia:

    Using the ideal gas law equation, calculate the grams of NH3 that can be produced when 4.10 L of NO2 react at a temperature of 385 ∘C and a pressure of 695 mmHg .

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  3. Stoichiometry of a Precipitation Reaction – Lab Report Assistant
    Exercise 1: Stoichiometry and a Precipitation Reaction
    Data Table 1. Stoichiometry Values
    Initial: CaCl2•2H2O (g)
    Initial: CaCl2•2H2O (moles)
    Initial: CaCl2 (moles)
    Initial: Na2CO3 (moles)
    Initial: Na2CO3 (g)
    Theoretical: CaCO3 (g)
    Mass of Filter paper (g)
    Mass of Filter Paper + CaCO3 (g)
    Actual: CaCO3 (g)
    % Yield:

    A) A perfect percent yield would be 100%. Based on your results, describe your degree of accuracy and suggest possible sources of error.
    B) What impact would adding twice as much Na2CO3 than required for stoichiometric quantities have on the quantity of product produced?
    C) Determine the quantity (g) of pure CaCl2 in 7.5 g of CaCl2•9H2O.
    D) Determine the quantity (g) of pure MgSO4 in 2.4 g of MgSO4•7H2O.
    E) Conservation of mass was discussed in the background. Describe how conservation of mass (actual, not theoretical) could be checked in the experiment performed.

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  4. 4.6

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  5. what are the answers? im in need of some help

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  6. 0.0034 Mol of CaCl2

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  7. fdgf

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