Question

A student places a 2.0 gram sample of magnesium metal in a bottle and fits the bottle with a two hole rubber stopper as shown in the diagram. Hydrochloric acid is added to the bottle and a
reaction occurs. As the reaction proceeds hydrogen gas travels through the tubing to an inverted
bottle filled with water, displacing some of the water in the bottle.

1. Calculate the number of grams of magnesium the students should mass out, to make 0.40 Liters of Hydrogrm gas at STP, show set up

Answer 1

The required number of grams of magnesium to make 0.40 Liters of Hydrogen gas at STP is 0.43 grams.

What is ideal gas equation?

Ideal gas equation gives idea about the behavior of gas at different condition & represented as:

PV = nRT, where

• P = standard pressure = 1atm
• V = volume = 0.4 L
• n = moles = ?
• R = universal gas constant = 0.082 L.atm / K.mol
• T = standard temperature = 273.15K

On putting values, we get moles as:

n = (1)(0.4) / (0.082)(273.15) = 0.0178 mol

Given chemical reaction is:

Mg + 2HCl → MgCl₂+ H₂

From the stoichiometry of the reaction:

0.0178 moles of H₂ = produced by the reaction 0.0178 moles of Mg

Mass of Mg = (0.0178mol)(24.3g/mol) = 0.43g

Hence required mass of magnesium is 0.43g.

To know more about mass & moles, visit the below link:

brainly.com/question/20562198

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