Question

Gold reacts with the elements in Group 7 of the periodic table. 0.175 g of gold reacts with chlorine.
The equation for the reaction is: 2 Au + 3 Cl22 AuCl3
Calculate the mass of chlorine needed to react with 0.175 g of gold.
Give your answer in mg Relative atomic masses (Ar): Cl = 35.5 Au = 197

Answer 1

Answer:

The atmosphere of Earth is the layer of gases, commonly known as air, retained by Earth's gravity, surrounding the planet Earth and forming its planetary atmosphere.

Answer 2

Gold reacts with a mass of 94.6 mg of chlorine gas.

Step-by-step procedure

Given:

given mass of Au= 0.175g

Atomic mass of Au= 197g

Atomic mass of chlorine atom= 35.5 g

Formula:

The number of moles of gold is calculated by

Number of moles= given mass/ molar mass

Putting the values in equation, we get:

number of moles of gold =  0.1175/197= 0.000888 moles

Now, the balanced equation for the reaction is given as:

2Au + 3$Cl_{2}$ → 2AuC$l_{3}$

From stoichiometry, if 2 moles of gold readily react with 3 moles of Cl.

0.000888 moles of gold will react with = 3/2 x 0.000888 x 35.5

Number of moles of Cl = 0.001332 moles

Result:

Thus, the mass of Cl that will react with Au is:

Mass of Cl= 0.01332 x 71= 0.0946 g

0.0946 g  x 1000= 94.6mg

Thus, the mass of Cl that reacts with Au is 94.6 mg