Question

Cu(s) + 2 AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s)

In a rate experiment, a coil of copper wire is placed into a solution of silver nitrate. The following data are recorded.
Time (hours): 0.0, 4.0
Mass of Copper (g): 3.45, 2.12
Calculate the rate of this reaction.
a) 1.33 , g/hour/M

b) 0.83 , g/hour/M

c) 0.58 , g/hour/M

d) 0.33 , g/hour/M

Answer 1

The rate of this reaction is 0.33 g/hour.

Step-by-step explanation:

The rate of a reaction can be calculated by determining the change in mass of one of the reactants or products over time. In this case, we can calculate the rate of the reaction by finding the difference in mass of copper wire (Cu) before and after a certain time interval. The rate of the reaction is calculated using the formula:

Rate = (Change in mass of copper)/(Time interval)

In the given data, the initial mass of copper wire is 3.45 g and after 4.0 hours the mass is 2.12 g. The change in mass is 3.45 g - 2.12 g = 1.33 g. The time interval is 4.0 hours. Plugging in these values into the above formula, we get:

Rate = (1.33 g)/(4.0 hours) = 0.33 g/hour

Therefore, the rate of this reaction is 0.33 g/hour.