Question

How many grams of silver oxide are needed to react with 7.9 g of hydrochloric acid produce silver chloide and water?

Answer 1

Approximately 7.88 grams of silver oxide are needed to react with 7.9 grams of hydrochloric acid to produce silver chloride and water.

Step-by-step explanation:

To determine the amount of silver oxide needed to react with hydrochloric acid, we need to use stoichiometry and the balanced chemical equation for the reaction. The balanced equation is:

2 AgOH + 2 HCl → 2 AgCl + 2 H2O

From the equation, we can see that 2 moles of AgOH react with 2 moles of HCl to produce 2 moles of AgCl and 2 moles of H2O. Therefore, the molar ratio between AgOH and HCl is 1:1. To find the mass of AgOH needed, we need to convert the mass of HCl given to moles using its molar mass, and then use the mole ratio to determine the mass of AgOH.

First, calculate the number of moles of HCl:

moles HCl = mass of HCl / molar mass of HCl

moles HCl = 7.9 g / 36.46 g/mol = 0.216 mol HCl

Since the molar ratio between AgOH and HCl is 1:1, the molar mass of AgOH is the same as HCl (36.46 g/mol).

Now, we can calculate the mass of AgOH:

mass AgOH = moles AgOH × molar mass of AgOH

mass AgOH = 0.216 mol × 36.46 g/mol = 7.88 g

Therefore, approximately 7.88 grams of silver oxide are needed to react with 7.9 grams of hydrochloric acid.

Answer 2

25.11 g.

Step-by-step explanation:

• It is clear from the balanced equation:

Ag₂O + 2HCl → 2AgCl + H₂O.

that 1.0 mole of Ag₂O reacts with 2.0 moles of HCl to produce 2.0 mole of AgCl and 1.0 moles of H₂O.

• 7.8 g of HCl reacts with excess Ag₂O. To calculate the no. of grams of Ag₂O that reacted, we should calculate the no. of moles of HCl:

no. of moles of HCl = mass/atomic mass = (7.9 g)/(36.46 g/mol) = 0.2167 mol.

• From the balanced equation; every 1.0 mol of Ag₂O reacts with 2 moles of HCl.

∴ 0.2167 mol of HCl will react with (0.2617 mol / 2 = 0.1083 mol) of Ag₂O.

∴ The mass of reacted Ag₂O = no. of moles x molar mass = (0.1083 mol)(231.735 g/mol) = 25.11 g.