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3 years ago

9

Which of the following measurements is equal to 2.3 dL?

1 answer:

kondaur [170]3 years ago

5 0

Which of the following measurements is equal to 2.3 dL?

23 L

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How many grams of potassium chlorate are needed to saturate 100g of water at 70 celsius? Group of answer choices 48 g 100 g 34 g

marissa [1.9K]

Answer:

34g of potassium chlorate.

Explanation:

A saturated solution is a solution that, under a temperature, has the maximum amount of solute possible. The maximum amount that a solvent can dissolve of a solute is called <em>solubility.</em>

<em> </em>

The solubility of potassium chlorate in water at 70°C is 34g/ 100g of water.

That means, to saturate 100g of water at 70°C you need yo add:

<h3>34g of potassium chlorate.</h3>

3 0

3 years ago

The ozone "hole" over Antarctica formed as the result of a series of chemical reactions. The loss occurs in part through three c

mixer [17]

Answer:

A)

Cl + O3 --> ClO + O2

2ClO --> ClOOCl

ClOOCl --> 2 Cl + O2

B)

Cl2 + 4O3 -> 2 ClO + 5O2

Explanation:

Step 1: Chlorine atoms react with ozone (O3) to form chlorine monoxide and molecular oxygen

Cl + O3 --> ClO + O2

Step 2: Chlorine monoxide molecules combine to form ClOOCl gas

2ClO --> ClOOCl

Step 3: ClOOCl absorbs sunlight and breaks into chlorine atoms and molecular oxygen

ClOOCl --> 2 Cl + O2

B) Overall Balanced equation

Cl2 + 4O3 -> 2 ClO + 5O2

7 0

3 years ago

What is the final pressure, in mmHg, for a gas in an aerosol can at an initial pressure of 1.40 atm at 12°C which is heated to 3

liubo4ka [24]

Answer:

b. 1150 mmHg

General Formulas and Concepts:

<u>Chemistry - Gas Laws</u>

Gay Lussac Law - $\frac{P_1}{T_1} =\frac{P_2}{T_2}$

P₁ is Pressure 1
T₁ is Temperature 1 in Kelvin
P₂ is Pressure 2
T₂ is Temperature 2 in Kelvin

Explanation:

<u>Step 1: Define</u>

P₁ = 1.40 atm

T₁ = 12°C

P₂ = unknown

T₂ = 35°C

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

1 atm = 760 mmHg

K = °C + 273.15

<u>Step 3: Convert</u>

P₁ = 1.40 atm = 1064 mmHg

T₁ = 12°C = 285.15 K

T₂ = 35°C = 308.15 K

<u>Step 4: Find P₂</u>

Substitute: $\frac{1064 \ mmHg}{285.15 \ K} =\frac{P_2}{308.15 \ K}$
Cross-multiply: $(1064 \ mmHg)(308.15 \ K)=P_2(285.15 \ K)$
Multiply: $327872 \ mmHg \cdot K=P_2(285.15 \ K)$
Isolate P₂: $\frac{327872 \ mmHg \cdot K}{285.15 \ K}=P_2$
Divide: $1149.82 \ mmHg=P_2$
Rewrite: $P_2=1149.82 \ mmHg$

<u>Step 5: Check</u>

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

1149.82 mmHg ≈ 1150 mmHg

4 0

3 years ago

what is the maximum amount of moles of P2O5 that can theoretically be made from 136 g of P4 and excess oxygen

zhuklara [117]

We are given with
136 g P4
excess oxygen

The complete combustion reaction is
P4 + 5O2 => 2P2O5
Converting the amount of P4 to moles
136/123.9 = 1.098 moles

Using stoichiometry
moles P2O5 = 1.098 x 2 = 2.195 moles P2O5

6 0

4 years ago

Read 2 more answers

2. Name three factors that influence the rate at which a solute dissolves in a solvent?<br>

agasfer [191]

Answer:

1. Temperature

2. Surface area

3. Catalyst

Explanation:

3 0

3 years ago

Read 2 more answers