Question

How many grams of Ni are formed from 54.5 g of Ni2O3? (Do not include units in your answer.)

2Ni3O3(s)→4Ni(s)+3O2(g)

Answer 1

54.5 g of Ni2O3 will produce 38.7 g of Ni using stoichiometry based on the molar masses and the balanced chemical equation.

Step-by-step explanation:

The question is asking how many grams of nickel (Ni) can be formed from a given mass of nickel(III) oxide (Ni2O3). To find the mass of Ni produced, we need to use stoichiometry based on the provided balanced chemical equation 2Ni2O3(s) → 4Ni(s) + 3O2(g).

First, calculate the moles of Ni2O3 using its molar mass (Molar mass Ni2O3 = 74.69 g/mol x 2 + 16.00 g/mol x 3 = 165.39 g/mol). Then, use the stoichiometry from the balanced equation to find the moles of Ni produced. Finally, convert the moles of Ni to mass using the molar mass of Ni (58.69 g/mol).

Step by step calculation:

1. Calculate moles of Ni2O3: 54.5 g / 165.39 g/mol = 0.3296 mol Ni2O3
2. Using the balanced equation, 2 mol of Ni2O3 produce 4 mol of Ni, so 0.3296 mol will produce: 0.3296 mol Ni2O3 x (4 mol Ni / 2 mol Ni2O3) = 0.6592 mol Ni
3. Convert moles of Ni to mass: 0.6592 mol x 58.69 g/mol = 38.7 g of Ni

Therefore, 54.5 g of Ni2O3 will produce 38.7 g of Ni.