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Kobotan [32]
3 years ago
13

Calculate the density of a rectangular solid which has a mass of 25.71g. It is 2.30cm long, 4.01 cm wide and 1.82 cm high.

Chemistry
2 answers:
pickupchik [31]3 years ago
3 0
V = a x b x c

V = 2.30 x 4.01 x 1.82

V = 16.78586 cm³

D = m / V

D = 25.71 / 16.78586

D = 1.53 g/cm³
faust18 [17]3 years ago
3 0
<span>Density is a value for mass, such as kg, divided by a value for volume, such as m3. Density is a physical property of a substance that represents the mass of that substance per unit volume. Calculation is as follows:

Density = mass / volume = 25.71 g / (</span><span>2.30cm x 4.01 cm x 1.82 cm)
Density = 1.53 g/cm^3</span>
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In the equilibrium constant expression for the reaction below what is the correct exponent for N2O4?
irga5000 [103]
As we have the balanced reaction equation is:

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8 0
2 years ago
How many moles of copper are in 1.51 x 1024 Cu atoms?
kkurt [141]
<h3>Answer:</h3>

2.51 mol Cu

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Using Dimensional Analysis
  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
<h3>Explanation:</h3>

<u>Step 1: Define</u>

1.51 × 10²⁴ atoms Cu

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

  1. Set up:                                \displaystyle 1.51 \cdot 10^{24} \ atoms \ Cu(\frac{1 \ mol \ Cu}{6.022 \cdot 10^{23} \ atoms \ Cu})
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<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

2.50747 mol Cu ≈ 2.51 mol Cu

8 0
2 years ago
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