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777dan777 [17]
3 years ago
14

Write the following numbers in scientific notation.

Chemistry
1 answer:
Basile [38]3 years ago
3 0

Answer:

2,5,10

Explanation:

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A solution of 1.50 g of solute dissolved in 25.0 mL of H₂O at 25°C has a boiling point of 100.45°C. (d) Find the van’t Hoff fact
givi [52]

The van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved and the concentration of a substance as calculated from its mass. For most non-electrolytes dissolved in water, the van 't Hoff factor is essentially 1.

<h3>What is the value of van 't Hoff factor?</h3>

For most non-electrolytes dissolved in water, the Van 't Hoff factor is essentially $ 1 $ . For most ionic compounds dissolved in water, the Van 't Hoff factor is equal to the number of discrete ions in a formula unit of the substance.

Which has highest Van t Hoff factor?

The Van't Hoff factor will be highest for

  A. Sodium chloride.

  B. Magnesium chloride.

  C. Sodium phosphate.

  D. Urea.

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4 0
1 year ago
Using the following equation, 2C2H6 +7O2 --&gt;4CO2 +6H2O, if 2.5g C2H6 react with 170g of O2, how many grams of water will be p
kirill [66]

The mass of water (H₂O) that would be produced is 4.5 g

<h3>Stoichiometry </h3>

From the question, we are to determine the mass of water that would be produced.

From the given balanced chemical equation

2C₂H₆ +7O₂ → 4CO₂ +6H₂O

This means

2 moles of C₂H₆ reacts with 7 moles of O₂ to produce 4 moles of CO₂ and 6 moles of H₂O

Now, we will determine the number of moles of each reactant present

  • For Ethane (C₂H₆)

Mass = 2.5 g

Molar mass = 30.07 g

Using the formula,

Number\ of\ moles = \frac{Mass}{Molar\ mass}

Number of moles of C₂H₆ present = \frac{2.5}{30.07}

Number of moles of C₂H₆ present = 0.08314 mole

  • For Oxygen (O₂)

Mass = 170g

Molar mass = 31.999 g/mol

Number of moles of O₂ present = \frac{170}{31.999}

Number of moles of O₂ present = 5.3127 moles

Since

2 moles of C₂H₆ reacts with 7 moles of O₂

Then,

0.08314 mole of C₂H₆ will react with \frac{7 \times 0.08314 }{2}

 \frac{7 \times 0.08314 }{2} = 0.58198 mole

Therefore,

0.08314 mole of C₂H₆ reacts with 0.58198 mole of O₂ to produce 3 × 0.08314 moles of H₂O

3 × 0.08314 = 0.24942 mole

Thus, the number of moles of water (H₂O) produced is 0.24942 mole

Now, for the mass of water that would be produced,

Using the formula,

Mass = Number of moles × Molar mass

Molar mass of water = 18.015 g/mol

Then,

Mass of water that would be produced = 0.24942 × 18.015

Mass of water that would be produced = 4.4933 g

Mass of water that would be produced ≅ 4.5 g

Hence, the mass of water (H₂O) that would be produced is 4.5 g

Learn more on Stoichiometry here: brainly.com/question/14271082

3 0
2 years ago
what is the chemical reaction and mole ratio between oxalate and permanganate in the titration reaction
Tom [10]

5C2O4^(2-)(aq) + 2MnO4^-(aq) + 16H+(aq) → 10CO2(g) + 2Mn2+(aq) + 8H2O(l)` is the chemical reaction and mole ratio between oxalate and permanganate in the titration reaction.

A chemical reaction is a procedure that causes one group of chemical components to change chemically into another. Chemical reactions, which can frequently be described by a chemical equation, traditionally include changes that only affect the locations of electrons in the formation and dissolution of chemical bonds between atoms, with no change to the nuclei (no change to the elements present). The study of chemical processes involving unstable and radioactive elements, where both electronic and nuclear changes may take place, is known as nuclear chemistry.

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6 0
1 year ago
I hate chemistry sm pls help
Liono4ka [1.6K]
Answer:
c
O2: 7 mol
CO2: 4 mil
5 0
2 years ago
Can anyone help me with this since it is a quiz and I am really bad at chemistry!!
lord [1]

Answer:

Down below <3

Explanation:

1. <u> 1 </u> N_{2} + <u> 3 </u> H_{2} ---> <u> 2 </u> NH_{3}

2. <u> 2 </u> KClO_{3} ---> <u> 2 </u> KCl + <u> 3 </u> O_{2}

3. <u> 1 </u> Na_{3}PO_{4} + <u> 3 </u> HCl ---> <u>_ 3_</u> NaCl + <u> 1 </u> H_{3}PO_{4}

4. <u> 1 </u> C_{2}H_{6}O + <u> 3 </u> O_{2} ---> <u> 2 </u> CO_{2} + <u> 3 </u> H_{2}O

5 0
3 years ago
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