If 0.1g of Unknown chloride reacts with 0.164 g of AgNo3 to form 0.05g of Agcl and unknown Nitrate.How do we find Unknown chloride?
To find the mass of the unknown chloride, we can use the concept of stoichiometry.
First, we need to balance the chemical equation for the reaction between the unknown chloride and AgNO3:
Unknown chloride + AgNO3 → AgCl + Unknown nitrate
Let's assume the unknown chloride is represented by the formula XCl.
The balanced equation would be:
XCl + AgNO3 → AgCl + XNO3
According to the question, we have the following information:
Mass of AgCl formed = 0.05 g
Mass of AgNO3 used = 0.164 g
To find the mass of XCl, we need to use the molar ratio between AgCl and AgNO3 from the balanced equation. This ratio can be obtained by comparing the coefficients of these two compounds in the equation.
The molar mass of AgCl is 143.32 g/mol, and the molar mass of AgNO3 is 169.87 g/mol. Using these molar masses along with the given masses, we can find the number of moles of AgCl and AgNO3.
Number of moles of AgCl = Mass of AgCl / Molar mass of AgCl
Number of moles of AgNO3 = Mass of AgNO3 / Molar mass of AgNO3
Now, by comparing the coefficients of AgCl and AgNO3 in the balanced equation, we can write the mole ratio:
Moles of AgCl : Moles of AgNO3 = Coefficient of AgCl : Coefficient of AgNO3
Using this ratio, we can determine the number of moles of XCl:
Moles of XCl = Moles of AgCl × (Coefficient of XCl / Coefficient of AgCl)
Finally, we can find the mass of XCl using the mole-mass relationship:
Mass of XCl = Moles of XCl × Molar mass of XCl
By following these steps, you should be able to calculate the mass of the unknown chloride (XCl).