Determine the approximate density of a high-leaded brass that has a composition of 60.5 wt% Cu, 34.5 wt% Zn, and 5.0 wt% Pb. The densities of Cu, Zn, and Pb are 8.94, 7.13 and 11.35 g/cm3, respectively.

Approximate density of the high-leaded brass(alloy) =8.306g/cm³

Explanation:

The density of an  alloy is its mass (100g) divided by its volume

Therefore we have that the alloy (high-leaded brass) has a composition of

60.5 wt% Cu with density  8.94g/cm3

34.5 wt% Zn, wth densty  7.13g/cm3

5.0 wt% Pb with densty g/cm3

The total volume of the alloy will be the mass / density of ts composition given as :

60.5gCu/DCu + 34.5gZn/DZn + 5.0gPb/Dpb

= 60.5/8.94 + 34.5/7.13+ 5.0/11.35

= 6.76 cm³ + 4.838 cm³+0.4405 cm³ = 12.0385cm³

Approximate density of the high-leaded brass(alloy) = 100g/  12.0385cm³ =8.306g/cm³

4 g AgCl

General Formulas and Concepts:

Math

Pre-Algebra

Order of Operations: BPEMDAS

Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to Right

Chemistry

Stoichiometry

Reading a Periodic TableUsing Dimensional AnalysisExplanation:

Step 1: Define

[RxN]   2AgNO₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂

[Given]   5.0 g AgNO₃

Step 2: Identify Conversions

[Reaction - Stoich] 2AgNO₃ → 2AgCl

Molar Mass of Ag - 107.87 g/mol

Molar Mass of N - 14.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of Cl - 35.45 g/mol

Molar Mass of AgNO₃ - 107.87 + 14.01 + 3(16.00) = 169.88 g/mol

Molar Mass of AgCl - 107.87 + 35.45 = 143.32 g/mol

Step 3: Stoichiometry

Set up:                              Multiply/Divide:                                                                                                  

Step 4: Check

Follow sig fig rules and round. We are given 1 sig fig.

4.21533 g AgCl ≈ 4 g AgCl