Using chemical equation to find moles of product from moles of reactant

0.21 mole of C8H18.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

2C8H18 + 25O2 —> 16CO2 + 18H2O

Next, we shall determine the number of mole of C8H18 that reacted and the number of mole water (H2O) produced from the balanced equation.

This is illustrated below:

From the balanced equation above,

2 moles of C8H18 reacted to produce 18 moles of H2O.

Finally, we shall determine the number of mole C8H18 needed to produce 1.90 moles of H2O.

This can be obtained as follow:

From the balanced equation above,

2 moles of C8H18 reacted to produce 18 moles of H2O.

Therefore, Xmol of C8H18 will react to produce 1.90 moles of H2O i.e

Xmol of C8H18 = (2 × 1.90)/18

Xmol of C8H18 = 0.21 mole

Thus, 0.21 mole of C8H18 is needed for the reaction.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

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