# How much calcium metal must be added to an excess of water to produce 3.7g of calcium hydroxide?

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As usual, our reasoning must be guided by the following stoichiometric equation:

And we calculate (i) the calcium hydroxide moles...

Therefore, (ii) we require an equivalent molar amount of metal.

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The mass of calcium is

The way that calcium and water interact is

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To calculate the amount of calcium metal needed to produce 3.7g of calcium hydroxide, you need to use stoichiometry. The balanced chemical equation for the reaction between calcium metal ((Ca)) and water ((H_2O)) to produce calcium hydroxide ((Ca(OH)_2)) is:

[Ca + 2H_2O \rightarrow Ca(OH)_2 + H_2]

From the equation, you can see that one mole of calcium metal reacts with two moles of water to produce one mole of calcium hydroxide.

1 mole of (Ca(OH)_2) has a molar mass of approximately (74.09 g/mol).

Using the molar mass of calcium hydroxide, you can convert the given mass (3.7g) to moles. Then, using the stoichiometry of the reaction, you can determine the moles of calcium metal required. Finally, using the molar mass of calcium, you can convert the moles of calcium to grams.

The calculation steps are as follows:

- Calculate moles of (Ca(OH)_2) using its molar mass.
- Use stoichiometry to find moles of (Ca) required.
- Convert moles of (Ca) to grams.

[Moles \ of \ Ca(OH)_2 = \frac{3.7g}{74.09g/mol} = 0.05 \ moles ]

[Moles \ of \ Ca = \frac{0.05 \ moles \ Ca(OH)_2}{1} = 0.05 \ moles ]

[Grams \ of \ Ca = 0.05 \ moles \times \frac{40.08g}{1 \ mole} = 2.004 \ g ]

So, approximately (2.004 \ g) of calcium metal must be added to produce (3.7g) of calcium hydroxide.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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