4 years ago

Which student was practicing poor laboratory safety?

Chemistry

1 answer:

insens350 [35]4 years ago

8 0

Answer herbert

Explanation:

cause he did not do any of the safety precautions and he was prob not listening to the teacher

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A sample of gas occupies a volume of 67.1 mL . As it expands, it does 135.3 J of work on its surroundings at a constant pressure

Semmy [17]

Answer:

$V_2=1.363x10^{-3}m^3=1363mL$

Explanation:

Hello,

In this case, since the work done at constant pressure as in isobaric process is computed by:

$W= P(V_2-V_1)$

Thus, given the pressure, initial volume and work, the final volume is:

$V_2=V_1+\frac{W}{P}$

Whereas the pressure must be expressed in Pa as the work is given in J (Pa*m³):

$P=783Torr*\frac{101325Pa}{760Torr} =104394Pa$

And the volumes in m³:

$V_1=67.1mL*\frac{1m^3}{1x10^6mL} =6.71x10^{-5}m^3$

Thus, the final volume turns out:

$V_2=6.71x10^{-5}m^3+\frac{135.3Pa*m^3}{104394Pa}\\\\V_2=1.363x10^{-3}m^3=1363mL$

Best regards.

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3 years ago

Why can evaporation be used to separate a mixture? check all that apply.

LUCKY_DIMON [66]

Answer:

A C F

Explanation:

brainly.com/question/4694205

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3 years ago

The pictures above show a gerbera daisy that has experienced a change called wilting. Which of the statements below best describ

Brilliant_brown [7]

Answer:

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3 years ago

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How many moles of Na are in 11.9 grams of Na

hram777 [196]

Answer:

sdgas

Explanation:

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3 years ago

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Find the ph of a buffer that consists of 0.18 m ch3nh2 and 0.73 m ch3nh3cl (pkb of ch3nh2 = 3.35)?

ozzi

Hello!

First, we need to determine the pKa of the base. It can be found applying the following equation:

$pKa=14-pKb=14-3,35=10,65$

Now, we can apply the Henderson-Hasselbach's equation in the following way:

$pH=pKa+log( \frac{[CH_3NH_2]}{[CH_3NH_3Cl]} )=10,65+log( \frac{0,18M}{0,73M} )=10,04$

So, the pH of this buffer solution is 10,04

Have a nice day!

8 0

3 years ago