Question

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

Balance Equation 1st: Ag2O + 2HCl = 2AgCl + H2O

A) 19.8 g

B) 39.6 g

C) 4.95 g

D) 3.975 g

Answer 1

To react with 7.9 g of hydrochloric acid, 25.13 g of silver oxide are required based on stoichiometry and molar mass calculations.

Step-by-step explanation:

To find out how many grams of silver oxide (Ag2O) are needed to react with 7.9 g of hydrochloric acid (HCl) to produce silver chloride (AgCl) and water (H2O), we need to use the stoichiometry of the balanced chemical equation. The balanced equation for this reaction is:

Ag2O + 2 HCl → 2 AgCl + H2O

First, we need to calculate the moles of HCl using its molar mass:

7.9 g HCl × (1 mol HCl / 36.46 g HCl) = 0.2168 moles HCl

From the stoichiometry of the balanced equation, 1 mole of Ag2O reacts with 2 moles of HCl, so:

0.2168 moles HCl × (1 mol Ag2O / 2 mol HCl) = 0.1084 moles Ag2O

Finally, we'll convert the moles of Ag2O to grams using its molar mass (231.74 g/mol):

0.1084 mol Ag2O × (231.74 g Ag2O / 1 mol Ag2O) = 25.13 g Ag2O

So, you would need 25.13 grams of silver oxide to react with 7.9 grams of hydrochloric acid.