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zimovet [89]
3 years ago
11

Adding energy has no effect on the rate of evaporation? True or False ?

Chemistry
1 answer:
zlopas [31]3 years ago
5 0

Answer:

False

Explanation:

Evaporation occurs when molecules in a liquid gain enough energy that they overcome attractions from other molecules and break away to become a gas. Adding energy increases the rate of evaporation.

Hope this helped!

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If 82.5 mol of an ideal gas occupies 10.5 l at 317 k, what is the pressure of the gas?
Natali5045456 [20]

P=20707.7 atm

<h3>What is the molar form of the ideal gas law?</h3>

The ideal gas law is a straightforward formula that describes the relationship between an ideal gas's pressure P, volume V, and temperature T. Unless there is a strong reason to treat gases differently, we normally treat gases as ideal because of how straightforward this relationship is:-

PV=nRT

where ;

P= Pressure=?

V= Volume= 10.5 L

n= no.of mol.= 82.5 mol

R=Ideal gas constant= 8.314 joule / mol kelvin

T=Temperature= 317 K

using Given value:-

P= nRT/ V

P=(82.5 x 8.314 x 317) / 10.5

P=20707.7 atm

Learn more about Ideal gas law here:-

brainly.com/question/15132707

#SPJ4

8 0
1 year ago
How many grams of Br2 are needed to form 67.1 g of AlBr3 ?<br><br> 2Al(s)+3Br2(l)⟶2AlBr3(s)
Romashka [77]

Answer:

Approximately 60.3\; \rm g.

Explanation:

Look up the relative atomic mass of \rm Al and \rm Br on a modern periodic table:

  • \rm Al: 26.982.
  • \rm Br: 79.904.

Calculate the formula mass of \rm AlBr_3 and \rm Br_2:

\begin{aligned}& M(\mathrm{AlBr_3}) = 26.982 + 3 \times 79.904 \approx 266.694\; \rm g \cdot mol^{-1} \\ & M(\mathrm{Br_2}) = 2\times 79.904 \approx 159.808\; \rm g \cdot mol^{-1}\end{aligned}.

Calculate the number of moles of formula units in 67.1\; \rm g of \rm AlBr_3:

\begin{aligned}n(\mathrm{AlBr_3}) &= \frac{m(\mathrm{AlBr_3})}{M(\mathrm{AlBr_3})} \\ &\approx \frac{67.1\; \rm g}{266.694\; \rm g \cdot mol^{-1}} \approx 0.2516\; \rm mol \end{aligned}.

Refer to the balanced equation for this reaction. The ratio between the coefficients of \rm Br_2 and \rm AlBr_3 in that equation is three-to-two. That corresponds to the ratio:

\begin{aligned}\frac{n(\text{$\mathrm{Br_2}$, consumed})}{n(\text{$\mathrm{AlBr_3}$, produced})} &= \frac{3}{2}\end{aligned}.

It is already calculated that approximately 0.2516\; \rm mol of \rm AlBr_3 was produced through this reaction. Apply this ratio to approximate the (minimum) number of moles of \rm Br_2 that is consumed:

\displaystyle \frac{3}{2} \times 0.2516\; \rm mol \approx 0.3774\; \rm mol.

Calculate the mass of that 0.3774\; \rm mol of \rm Br_2:

\begin{aligned}m(\mathrm{Br_2}) &= n(\mathrm{Br_2})\cdot M(\mathrm{Br_2}) \\ &\approx 0.3774\; \rm mol \times 159.808\; \rm g \cdot mol^{-1} \approx 60.3\; \rm g\end{aligned}.

8 0
3 years ago
Which of these is an example of chemical separation of a substance?
OleMash [197]

Answer:

Bond broking

Explanation:

Bond broking.

6 0
3 years ago
An element 'X after reacting with acids liberates hydrogen gas and candisplace lead and mercury from their salt solutions. The m
adell [148]

The element X is Copper.

Explanation :

Reactive metals from 3d transition series like Cu are very reactive because their standard reduction potential values are low.

Hence, when treated with a acid it tends to liberate hydrogen gas.

Also, because of  its low reduction potential value, it can easily displace lead and tin from their salt solutions.

Learn more :

https://brainly.in/question/6679934

5 0
3 years ago
Describe how a metal less reactive than carbon can be reduced from its ore
trapecia [35]

Answer:

If a metal is less reactive than carbon, it can be extracted from its oxide by heating with carbon. The carbon displaces the metal from the compound, and removes the oxygen from the oxide. This leaves the metal.

8 0
2 years ago
Read 2 more answers
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