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3 years ago

Which statement is true according to the kinetic theory?

Chemistry

1 answer:

Elza [17]3 years ago

5 0

Answer:

Molecules of different gases with the same mass and temperature always have the same average kinetic energy.

Explanation:

According to the kinetic theory:

The average kinetic energy of gaseous particles is proportional to absolute temperature of all gases at the same temperature and have same kinetic energy

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Answer:

Explanation:

I would ask him why would he want to add the blue stripe?

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3 years ago

Use the collision theory to explain how increasing the surface area of a solute will increase the rate of the dissolving process

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More surface area --> more molecules of the solute in contact with the solvent --> more chance for a solvent molecule to collide with the solute molecules --> dissolves faster

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A boy kicks a ball with a force of 40 N. At exactly the same moment, a gust of wind blows in the opposite direction of the kick

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4 years ago

Read 2 more answers

In an experiment to find the concentration of calcium hydroxide in limewater , 25.0 cm3 of limewater needed 18.8 cm3 of 0.0400 m

Andre45 [30]

Answer:

0.01504 mol/dm3

Explanation:

Calcium Hydroxide - Ca(OH)2

Hydrochloric acid - HCl

The reaction between both is given as;

2HCl + Ca(OH)2 --> CaCl2 + 2H2O

2 : 1

The relationship between the concentration and volume is given as;

CaVa / CbVb = na / nb

where a = acid (HCl) and b = base Ca(OH)2

Inserting the values;

0.04 * 18.8 / (Cb * 25) = 2 / 1

0.752 / 25Cb = 2

Cb = 0.752 / 50 = 0.01504

6 0

3 years ago

Two liquids are analyzed and found to both be 85.7% carbon and 14.3% hydrogen. At 750 mmHg and 150 C, both are gases. At these c

vodomira [7]

Answer:

Molecular formula A: C₅H₁₀

Molecular formula B: C₇H₁₄

Explanation:

It is possible to obtain empirical formula of compounds using percent composition, thus:

C: 85.7% × (1mol / 12.01g) = 7.136 moles C

H: 14.3% × (1mol / 1.01g) = 14.158 moles H

Mole ratio of H:C is:

14.158mol / 7.136mol = 2

That means in compounds A and B you have 2 hydrogens per atom of carbon and empirical formila is:

CH₂

Using PV = nRT, moles of A and B are:

Where P is pressure (750mmHg / 760 = 0.987atm), V is volume (0.8000L), R is gas constant (0.082atmL/molK), and T is temperature (150°C +273.15 = 423.15K)

Moles A and B: n = PV / RT

n = 0.987atm×0.8000L / 0.082atmL/molK×423.15K

n = 0.0228 moles of A and B.

Using the mass of A and B it is possible to find molar mass of each compound:

A = 1.60g / 0.0228mol = 70.31g/mol

B = 2.22g / 0.0228mol = 97.56g/mol

As empirical formula of both compounds is CH₂, (molar mass = 14.03g/mol). Molecular formula of compounds is:

A = 70.31g/mol / 14.03g/mol = 5 → Molecular formula: 5×CH₂ = C₅H₁₀

B = 97.56g/mol / 14.03g/mol = 7 → Molecular formula: 7×CH₂ = C₇H₁₄

8 0

3 years ago