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tangare [24]
3 years ago
11

Use the balanced equation to work the following problem:

Chemistry
2 answers:
tankabanditka [31]3 years ago
4 0
The answer is 0.841 g AgCl
qwelly [4]3 years ago
3 0

<u>Answer:</u> The mass of AgCl formed in the reaction is 0.841 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of silver nitrate = 1.00 g

Molar mass of silver nitrate = 170 g/mol

Putting values in equation 1, we get:

\text{Moles of silver nitrate}=\frac{1.00g}{170g/mol}=5.88\times 10^{-3}mol

For the given chemical equation:

CaCl_2+2AgNO_3\rightarrow 2AgCl+Ca(NO_3)_2

By Stoichiometry of the reaction:

2 moles of silver nitrate produces 2 moles of AgCl

So, 5.88\times 10^{-3}mol of silver nitrate will produce = \frac{2}{2}\times 5.88\times 10^{-3}=5.88\times 10^{-3}mol of AgCl

Now, calculating the mass of AgCl by using equation 1.

Moles of AgCl = 5.88\times 10^{-3}mol

Molar mass of AgCl = 143.32 g/mol

Putting values in equation 1, we get:

5.88\times 10^{-3}mol=\frac{\text{Mass of AgCl}}{143.32g/mol}\\\\\text{Mass of AgCl}=(5.88\times 10^{-3}mol\times 143.32g/mol)=0.841g

Hence, the mass of AgCl formed in the reaction is 0.841 grams.

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saul85 [17]

32.8 g of Butane is required and 99.3 g of CO₂ is produced

<u>Explanation:</u>

The above mentioned reaction can be written as,

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