Please help me. especially with figuring out c

A. 4Ni(s) + 3O2(g) —> 2Ni2O3(s)

B. Synthesis reaction.

C. 18.31g of O2

Explanation:

A. The equation for the reaction.

Ni(s) + O2(g) —> Ni2O3(s)

The above equation can be balance as follow:

There are 2 atoms of O on the left side and 3 atoms on the right side. It can be balance by putting 2 in front Ni2O3 and 3 in front of O2 as shown below:

Ni(s) + 3O2(g) —> 2Ni2O3(s)

There are 4 atoms of Ni on the right side and 1 atom on the left it can be balance by putting 4 in front of Ni as shown below:

4Ni(s) + 3O2(g) —> 2Ni2O3(s)

Now the equation is balanced

B. From the equation, we can see that two reactants combined to form a single product. Therefore, the reaction is termed synthesis reaction.

C. We'll begin by calculating the mass of Ni and O2 that reacted from the balanced equation. This is illustrated below:

4Ni(s) + 3O2(g) —> 2Ni2O3(s)

Molar mass of Ni = 59g/mol

Mass of Ni from the balanced equation = 4 x 59 = 236g

Molar mass of O2 = 16x2 = 32g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96g

Summary:

From the balanced equation above,

236g of Ni reacted with 96g of O2.

Now, we can obtain the mass of O2 needed to react with 45g of Ni as follow:

From the balanced equation above,

236g of Ni reacted with 96g of O2.

Therefore, 45g of Ni will react with = (45 x 96)/236 = 18.31g of O2.

Therefore, 18.31g of O2 is needed to react with 45g of Ni

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

14,16 18 reacts with group