Copper is more reactive than silver.

Copper will displace silver from silver nitrate solution.

Two possible balanced equations for the reaction are:

Equation 1: $Cu+AgNO3→CuNO3+Ag\text{Cu} + \text{AgNO}_3 \rightarrow \text{CuNO}_3 + \text{Ag}$
Equation 2: Honor: $Cu+2AgNO3→Cu(NO3)2+2Ag\text{Cu} + 2\text{AgNO}_3 \rightarrow \text{Cu}(\text{NO}_3)_2 + 2\text{Ag}$

In an experiment, it was found that 1.27 g of copper reacted completely with excess silver nitrate solution to form 4.32 g of silver.

Carry out a calculation, using the information above, to show which equation represents the reaction taking place.

(Relative atomic masses, $A_r$ : $Cu=63.5\text{Cu} = 63.5$ , $Ag=108.0\text{Ag} = 108.0$ )

Copper is more reactive than silver.

Copper will displace silver from silver nitrate solution.

Two possible balanced equations for the reaction are:

Equation 1: $Cu+AgNO3→CuNO3+Ag\text{Cu} + \text{AgNO}_3 \rightarrow \text{CuNO}_3 + \text{Ag}$
Equation 2: Honor: $Cu+2AgNO3→Cu(NO3)2+2Ag\text{Cu} + 2\text{AgNO}_3 \rightarrow \text{Cu}(\text{NO}_3)_2 + 2\text{Ag}$

In an experiment, it was found that 1.27 g of copper reacted completely with excess silver nitrate solution to form 4.32 g of silver.

Carry out a calculation, using the information above, to show which equation represents the reaction taking place.

(Relative atomic masses, $A_r$ : $Cu=63.5\text{Cu} = 63.5$ , $Ag=108.0\text{Ag} = 108.0$ )

Calculations involving masses

Calculations involving masses Questions