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joja [24]
3 years ago
14

Which is greater in positive acceleration, initial or final velocity

Chemistry
1 answer:
Alex17521 [72]3 years ago
6 0

inital velocity (u) should be less


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What do you think happens to the bonds between atoms when substances melt?
Eduardwww [97]

Answer:

As a substance melts, and goes from a solid to a liquid state, the kinetic energy of the molecules increases, and the molecules move faster, and they separate further and further away from each other.  The intermolecluar forces holding the molecules together become weaker.  This is why a liquid can take fill the shape of its container, whereas a solid has a fixed shape.

Explanation:

take your notes man

6 0
3 years ago
Select all statements that are correct:____
topjm [15]

Answer:

A, C and D are correct.

Explanation:

Hello.

In this case, since the relationship between the vapor pressure of a solution is directly proportional to the mole fraction of the solvent and the vapor pressure of the pure solvent as stated by the Raoult's law:

P_{vap}^{solution}=x_{solvent}P_{solvent}

Since the solute is not volatile, the mole fraction of the solute is not taken into account for vapor pressure of the solution, therefore A is correct whereas B is incorrect.

Moreover, since the higher the vapor pressure, the weaker the intermolecular forces due to the fact that less more molecules are like to change from liquid to vapor and therefore more energy is required for such change, we can evidence that both C and D are correct.

Best regards.

4 0
3 years ago
25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq). What is the pH after 30 mL of NaOH have been added?
weeeeeb [17]

Answer:

pH = 11.95≈12

Explanation:

Remember  the reaction among aqueous acetic acid (CH_3COOH) and aqueous sodium hydroxide (NaOH)

CH_3COOH + NaOH ->  CH_3COONa + H_2O

First step. Need to know how much moles of the substances are present

0.1 \frac{mol NaOH}{L} * 0.030 L = 0.003 mol NaOH[tex]0.1 \frac{mol CH_3COOH}{L} * 0.025 L= 0.0025 mol CH_3COOHSecond step. Know wich substance is in excess.0.0025 mol CH_3COOH * [tex]1 mol NaOH/ 1 mol CH_3COOH = 0.0025 mol NaOH

0.003 mol NaOH * 1 mol CH_3COOH/ 1 mol NaOH = 0.003 mol CH_3COOH[/tex]

NaOH is in excess. Now, how much?

0.003 mole NaOH - 0.0025 mole NaOH = 0.0005 mole NaOH

Then, that amount in excess would be responsable for the pH.

Third step. Know the pH

Remember that pH= -log[H+]

According to the dissociation of water equilibrium

Kw=[H+]*[OH-]= 10^(-14)

The dissociation of NaOH is

NaOH -> Na^{+} + OH^{-}

Now, concentration of OH^{-}[/tex] would be given for the excess of NaOH.

[OH-]= 0.0005 mole / 0.055 L = 0.00909 M

Careful: we have to use the total volumen

Les us to calculate pH

pH= -log [H+]\\pH= -log \frac{K_w}{[OH-]} \\pH= 11.95

6 0
3 years ago
In what way would readings from a digital thermometer be preferable to those from a liquid-based thermometer
charle [14.2K]
A digital thermometer has less errors in reading temperatures because it displays the actual reading rather than approximating it in a liquid-based thermometer. Also, digital thermometer are advantageous to use in extreme temperature conditions because they can withstand in these type of conditions. 
7 0
3 years ago
Read 2 more answers
Consider the mechanism. step 1:step 2:overall:2a⟶bb c⟶d2a c⟶dslowfast determine the rate law for the overall reaction, where the
Ne4ueva [31]

Answer:

Rate: R = k [A]²

Explanation:

The rate law equation for a given complex chemical reaction is given as the product of molar concentrations of the reactant raised to the power their respective partial reaction orders. The sum of the partial reaction orders is equal to the overall order of reaction.

For a complex reaction, the rate law is generally determined by the slowest step, which is known as the rate-determining step.

<u>Given reaction mechanism:</u>

Step 1: 2 A⟶ B,               slow step

Step 2: B+ C⟶ D,            fast step

Overall: 2 A + C ⟶ D

In this given reaction mechanism, the <em>step 1 is the slow step and thus the rate determining step.</em>

Therefore, the rate law for the given mechanism is:

Rate: R = k [A]²

Here, k is the overall rate constant

Also, the overall order of the reaction = 2

Therefore, the given chemical reaction is said to be second order reaction.

3 0
3 years ago
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