Respuesta :
Answer: The mass of AgCl formed in the reaction is 0.841 grams.
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of silver nitrate = 1.00 g
Molar mass of silver nitrate = 170 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of silver nitrate}=\frac{1.00g}{170g/mol}=5.88\times 10^{-3}mol[/tex]
For the given chemical equation:
[tex]CaCl_2+2AgNO_3\rightarrow 2AgCl+Ca(NO_3)_2[/tex]
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 2 moles of AgCl
So, [tex]5.88\times 10^{-3}mol[/tex] of silver nitrate will produce = [tex]\frac{2}{2}\times 5.88\times 10^{-3}=5.88\times 10^{-3}mol[/tex] of AgCl
Now, calculating the mass of AgCl by using equation 1.
Moles of AgCl = [tex]5.88\times 10^{-3}mol[/tex]
Molar mass of AgCl = 143.32 g/mol
Putting values in equation 1, we get:
[tex]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[/tex]
Hence, the mass of AgCl formed in the reaction is 0.841 grams.
