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DaniilM [7]
1 year ago
5

When water evaporates (which involves breaking of hydrogen bonds), it removes energy from its surroundings in a fashion that ren

ders water an:_____.
Chemistry
1 answer:
WITCHER [35]1 year ago
4 0

When water evaporates (which involves breaking of hydrogen bonds), it removes energy from its surroundings in a fashion that renders water an Excellent coolant.

Within water molecules, polar covalent connections are created between the hydrogen and oxygen atoms. The shared electrons are attached to the oxygen atom for a longer period of time than they are to the hydrogen atoms. A water molecule has no overall charge, but each hydrogen atom has a little positive charge, and each oxygen atom has a slight negative charge. The slightly positive hydrogen atoms repel one another and form the distinctive shape as a result of these charges. The positive and negative charges in the various regions of each water molecule cause them to attract other water molecules. Additionally, water forms hydrogen bonds with other polar molecules (like sugars) by attraction.

To know more about hydrogen bonds

brainly.com/question/1420470

#SPJ4

You might be interested in
According to the reaction below, how many grams of KCl (potassium chloride) can be formed from 70.90 g of chlorine with excess p
Pepsi [2]

Answer:

149.1 g KCl

Explanation:

2 K  +  Cl₂  ⇒  2 KCl

This is your chemical equation.  Use this equation to figure out the stoichiometry between Cl₂ and KCl.  According to the equation, for every 2 moles of KCl, you need 1 mole of Cl₂, making the ratio between KCl and Cl₂ 2/1.

First, convert grams of Cl₂ to moles of Cl₂.  The molar mass is 70.906 g/mol.

(70.90 g Cl₂)/(70.906 g/mol) = 0.9999 mol Cl₂

Convert moles of Cl₂ to moles of KCl using the stoichiometric relationship.

(0.9999 mol Cl₂) × (2 mol KCl/1 mol Cl₂) = 1.9998 mol KCl

Convert moles of KCl to grams of KCl.  The molar mass is 74.55 g/mol.

(1.998 mol KCl) × (74.55 g/mol KCl) = 149.1 g KCl

You will produce 149.1 g KCl.

5 0
3 years ago
If a solution containing 0.10 M Cl-, Br-, I-, and LaTeX: CrO_4^2-C r O 4 2 − is treated with Ag+, in what order will the anions
Musya8 [376]

Answer:

AgI \longrightarrow AgBr \longrightarrow Ag_2CrO_4 \longrightarrow AgCl

Explanation:

The first thing to have in mind is that the Ksp (constant of solubility) gives you an idea of how much soluble a salt is.  <u>If the concentration of ions of that salt exceeds the kps, the salt will precipitate</u>.

The Kps of all these salts are very small compared to the 0.1 M concentration of the anions so all of them will precipitate.

The smaller the constant, the faster the salt precipitates

Having that concept in mind, the order of precipitation from first to last would be:

AgI \longrightarrow AgBr \longrightarrow Ag_2CrO_4 \longrightarrow AgCl

6 0
3 years ago
Given: 36.7 grams of CaF2 is added to 300 mL water. Find molarity?
BigorU [14]
<h3>Answer:</h3>

2 M

<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>Unit 0</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis

<u>Aqueous Solutions</u>

  • Molarity = moles of solute / liters of solution
<h3>Explanation:</h3>

<u>Step 1: Define</u>

36.7 g CaF₂

300 mL H₂O

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

Molar Mass of Ca - 40.08 g/mol

Molar Mass of F - 19.00 g/mol

Molar Mass of CaF₂ - 40.08 + 2(19.00) = 78.08 g/mol

1000 mL = 1 L

<u>Step 3: Convert</u>

<em>Solute</em>

  1. Set up:                               \displaystyle 36.7 \ g \ CaF_2(\frac{1 \ mol \ CaF_2}{78.08 \ g \ CaF_2})
  2. Multiply:                             \displaystyle 0.470031 \ mol \ CaF_2

<em>Solution</em>

  1. Set up:                              \displaystyle 300 \ mL \ H_2O(\frac{1 \ L \ H_2O}{1000 \ mL \ H_2O})
  2. Multiply:                            \displaystyle 0.3 \ L \ H_2O

<u>Step 4: Find Molarity</u>

  1. Substitute [M]:                    \displaystyle x \ M = \frac{0.470031 \ mol \ CaF_2}{.3 \ L \ H_2O}
  2. Divide:                                \displaystyle x = 1.56677 \ M

<u>Step 5: Check</u>

<em>Follow sig fig rules and round.</em> <em>We are given 1 sig fig as our lowest.</em>

1.56677 M ≈ 2 M

8 0
3 years ago
Calculate the mass in grams of carbon needed to produce 160 g of CO2 in burning: C + O2 --&gt; CO2
Vladimir [108]
160gof CO2×1molof CO2\44g of CO2×1mole of C\1mol of CO2×12g of C\1mole of C=
43.63g of C
5 0
3 years ago
Which describes an atom that has fewer neutrons than protons and more electrons than protons?
Eva8 [605]

Answer:

Option d is correct = Negative ion

Explanation:

We know that an atom consist of electrons, protons and neutrons. Neutrons and protons are present inside the nucleus while electrons are present out side the nucleus. Electron has a negative charge and is written as e⁻. The mass of electron is 9.10938356×10⁻³¹ Kg . While mass of proton and neutron is 1.672623×10⁻²⁷Kg  and 1.674929×10⁻²⁷ Kg  respectively.

Symbol of proton= P⁺  

Symbol of neutron= n⁰  

The number of electron or number of protons are called atomic number while mass number of an atom is sum of protons and neutrons. The  umber of protons and electrons are always equal to make the atom electrically neutral and when an atom loses its valance electron the number of protons increases and thus positive charge increased and atom form cation.

When an atom gain electron negative charge increase because of more number of electron thus atom form negative ion or anion. For example,

Anion formation:

X + e⁻ → X⁻

Cation formation:

X → X⁺ + e⁻

Thus option d is correct option.

5 0
4 years ago
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