label the state of matter changes42. two places you may find plasma are _______________ and _______________.43. iron and oxygen react to form rust. what will happen to the mass of the rust compared to the mass of the iron and oxygen before the reaction? explain why this will occur.44. the three points in the kinetic-molecular theory are _______________, _______________, and _______________.45. a piece of wood that measures 3 cm by 6 cm by 4 cm has a mass of 80 g. what is the density of the wood?_______________.46. find the mass of a 50 ml volume of water if the density of water is 1 g/ml.47. what is the volume of 72 g of copper if copper has a density of 9 g/cm3?48. a graduated cylinder has 33.5 ml of water. a piece of metal is added to the water and the new volume is now 46.2 ml. if the metal has a mass of 16.25 g, what is its density?49. draw the flow chart we use for classifying matter.50. name one similarity between compounds and homogeneous mixtures and one difference.

Question

Accepted Answer

### First: State of Matter Changes Labeling
# Brief Explanations:
Match each arrow to the correct phase change term based on the starting and ending states of matter.
# Answer:
- A: Sublimation (Solid to Gas)
- B: Deposition (Gas to Solid)
- C: Condensation (Gas to Liquid)
- D: Vaporization (Liquid to Gas)
- E: Melting (Solid to Liquid)
- F: Freezing (Liquid to Solid)

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### Question 42
# Brief Explanations:
Plasma is an ionized gas found in high-energy/high-temperature environments.
# Answer:
Two places you may find plasma are **lightning** and **stars (or neon signs)**.

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### Question 43
# Brief Explanations:
This follows the Law of Conservation of Mass, which states mass is neither created nor destroyed in a chemical reaction. Rust forms from the combination of iron and oxygen, so all reactant mass is retained in the product.
# Answer:
The mass of the rust will be equal to the total mass of the iron and oxygen before the reaction. This occurs because of the Law of Conservation of Mass: in a chemical reaction, the total mass of reactants equals the total mass of products, as no mass is created or destroyed.

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### Question 44
# Brief Explanations:
These are the core postulates of the kinetic-molecular theory for ideal gases.
# Answer:
The three points in the kinetic-molecular theory are:
1.  Particles of a gas are in constant, random motion.
2.  The collisions between gas particles are perfectly elastic (no net loss of energy).
3.  The volume of gas particles is negligible compared to the total volume of the gas, and there are no intermolecular forces between particles.

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### Question 45
# Explanation:
## Step1: Calculate volume of wood
Volume $V = l 	imes w 	imes h = 3\ 	ext{cm} 	imes 6\ 	ext{cm} 	imes 4\ 	ext{cm} = 72\ 	ext{cm}^3$
## Step2: Apply density formula
Density $
ho = \frac{	ext{mass}}{	ext{volume}} = \frac{m}{V}$
# Answer:
$
ho = \frac{80\ 	ext{g}}{72\ 	ext{cm}^3} \approx 1.11\ 	ext{g/cm}^3$

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### Question 46
# Explanation:
## Step1: Rearrange density formula for mass
Mass $m =
ho 	imes V$
## Step2: Substitute given values
$m = 1\ 	ext{g/mL} 	imes 50\ 	ext{mL}$
# Answer:
$m = 50\ 	ext{g}$

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### Question 47
# Explanation:
## Step1: Rearrange density formula for volume
Volume $V = \frac{m}{
ho}$
## Step2: Substitute given values
$V = \frac{72\ 	ext{g}}{9\ 	ext{g/cm}^3}$
# Answer:
$V = 8\ 	ext{cm}^3$

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### Question 48
# Explanation:
## Step1: Calculate metal volume
Volume $V = 	ext{Final Volume} - 	ext{Initial Volume} = 46.2\ 	ext{mL} - 33.5\ 	ext{mL} = 12.7\ 	ext{mL}$ (1 mL = 1 cm³)
## Step2: Apply density formula
$
ho = \frac{m}{V} = \frac{16.25\ 	ext{g}}{12.7\ 	ext{mL}}$
# Answer:
$
ho \approx 1.28\ 	ext{g/mL}$

---

### Question 49
# Brief Explanations:
The standard matter classification flowchart starts with a broad division, then narrows to specific types.
# Answer:
```
Matter
├─ Pure Substances
│  ├─ Elements (cannot be broken down)
│  └─ Compounds (can be broken down chemically)
└─ Mixtures
   ├─ Homogeneous Mixtures (uniform composition, solutions)
   └─ Heterogeneous Mixtures (non-uniform composition)
```

---

### Question 50
# Brief Explanations:
Compare the composition uniformity and chemical nature of compounds and homogeneous mixtures.
# Answer:
- **Similarity**: Both have a uniform, consistent composition throughout the sample.
- **Difference**: Compounds are pure substances formed by chemical bonding of elements in fixed ratios, and they can only be separated by chemical reactions. Homogeneous mixtures are physical combinations of substances in variable ratios, and they can be separated by physical methods (like evaporation or distillation).

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QUESTION IMAGE

Question

Explanation:

First: State of Matter Changes Labeling

Answer:

Question 42