How many grams of NO are produced from 15.8 g of H2O

26.33 g of NO.

Explanation:

We'll begin by writing the balanced equation to produce NO from H2O. This is given below:

5N2 + 6H2O —> 4NH3 + 6NO

Next, we shall determine the mass of H2O that reacted and the mass of NO produced from the balanced equation. This is illustrated below:

Molar mass of H2O = (2x1) + 16 = 18 g/mol

Mass of H2O from the balanced equation = 6 x 18 = 108 g

Molar mass of NO = 14 + 16 = 30 g/mol

Mass of NO from the balanced equation = 6 x 30 = 180 g

From the balanced equation above,

108 g of H2O reacted to produce 180 g of NO.

Finally, we shall determine the mass of NO produced by the reaction of 15.8 g of H2O.

This is illustrated below:

From the balanced equation above,

108 g of H2O reacted to produce 180 g of NO.

Therefore, 15.8 g of H2O will react to produce = (15.8 x 180)/108 = 26.33 g of NO.

Therefore, 26.33 g of NO were obtained from the reaction.

the volume increases

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2