Final answer:
To find the mass of Ni that reacts with 0.310 g of Ag in the given reaction, we need to calculate the moles of Ag first and then use the stoichiometry of the reaction to find the moles of Ni.
Step-by-step explanation:
The balanced chemical equation is: Ni (s) + 2 AgNO3 (aq) → Ni(NO3)2 (aq) + 2 Ag (s). From the equation, we can see that 1 mole of Ni reacts with 2 moles of AgNO3 to produce 1 mole of Ni(NO3)2 and 2 moles of Ag. To find the mass of Ni that reacts with 0.310 g of Ag, we need to use the stoichiometry of the reaction.
First, we need to convert the given mass of Ag to moles. The molar mass of Ag is 107.87 g/mol, so the moles of Ag is calculated as: 0.310 g / 107.87 g/mol = 0.00287 mol Ag.
Since the stoichiometry of the reaction is 1:2, the moles of Ni that reacts with 0.00287 mol Ag is half of that, which is 0.00143 mol Ni. Now, we can convert the moles of Ni to mass using the molar mass of Ni, which is 58.69 g/mol: 0.00143 mol * 58.69 g/mol = 0.084 g Ni.