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2 years ago

Which of these statements best describes physical properties?

Chemistry

1 answer:

balu736 [363]2 years ago

5 0

The correct answer would be D: Physical properties can be observed without changing the identity of a substance

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The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of lead acetate. When the test tube wa

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PbCl₂(s) ⇄ Pb²⁺(aq) + 2Cl⁻(aq)

Pb(CH₃COO)₂(s) → Pb²⁺(aq) + 2CH₃COO⁻(aq)

At lead acetate disolution, concentration of lead cations will increase. According to Le Chatelie's principle equilibrium will be displaced towards formation of solid lead chloride.

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3 years ago

Please answer asap.......................

Margarita [4]

Answer:

Explanation

Devision

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3 years ago

Scientists predict that polymer products will increase the use of

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Increase the use of nuclear energy

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3 years ago

Identify this reaction <br><br> HBr+ Al(OH)3 —-> H2O + AlBr3

Vikki [24]

<h2><em><u>Answer</u></em></h2>

Neutralization reaction

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4 years ago

For the following reaction, 4.53 grams of calcium hydroxide are mixed with excess sulfuric acid. The reaction yields 6.75 grams

vagabundo [1.1K]

Answer:

$\large \boxed{\text{8.32 g; 81.1 \%}}}$

Explanation:

MM: 74.09 136.14

H₂SO₄ + Ca(OH)₂ ⟶ CaSO₄ + 2H₂O

m/g: 4.53

1. Theoretical yield

(a) Moles of Ca(OH)₂

$\text{Moles of Ca(OH)${_2}$} = \text{4.53 g Ca(OH)${_2}$} \times \dfrac{\text{1 mol Ca(OH)${_2}$}}{\text{74.09 g Ca(OH)${_2}$}} = \text{0.161 14 mol Ca(OH)${_2}$}$

(b) Moles of CaSO₄

$\text{Moles of NH${_3}$} = \text{0.061 14 mol Ca(OH)${_2}$} \times \dfrac{\text{1 mol CaSO${_4}$}}{\text{1 mol Ca(OH)${_2}$}} = \text{0.061 14 mol CaSO${_4}$}$

(c) Theoretical yield

$\text{Mass of CaSO${_4}$} = \text{0.061 14 mol CaSO${_4}$} \times \dfrac{\text{136.14 g CaSO${_4}$}}{\text{1 mol CaSO${_4}$}} = \textbf{8.32 g CaSO${_4}$}$

2. Percent yield

$\text{Percent yield} = \dfrac{\text{ actual yield}}{\text{ theoretical yield}} \times 100 \% = \dfrac{\text{6.75 g}}{\text{8.32 g}} \times 100 \, \% = \text{81.1 \%}$

$\text{The percent yield is } \large \boxed{\textbf{81.1 \%}}}$

4 0

3 years ago