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Marta_Voda [28]
3 years ago
10

What are the basic steps of the scientific method??

Chemistry
1 answer:
finlep [7]3 years ago
4 0
1) Make an observation
2) Come up with a question
3) Making a hypothesis
4) Testing the hypothesis
5) Analyze the conclusions
6) Draw conclusions

this is how I've always learned it in school so I'm not sure if you learned it differently. 
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Match each term in the first column with an example in the second column. On a sheet of paper, write the letter of the answer.
Andrews [41]

Answer:

wait can you go more in detail i can help you because i dont understand whats going on

7 0
3 years ago
What is the osmotic pressure of a 100 ml of toluene solution that contains a total of 0.005 moles of a polymer dissolved in it a
allsm [11]

Osmotic pressure is the pressure that would have to be applied to a pure solvent to prevent it from passing into a given solution by osmosis.

That can be mathematical computed from the expression:

Osmotic pressure=C×R×T

Where,

C= Concentration

R=Gas constant

T=Temperature

Concentration=Number of moles of solute/Volume(L)

=0.005*1000/100

=0.05

R= 0.08206 atm L/mol K

T=25+273

=298

Osmotic pressure= 0.05×0.08206×298

=1.2 atm

4 0
3 years ago
How do I convert 0.43 atm to mmhg? (Question 2)
Dafna1 [17]
<h2>Greetings!</h2>

Because 1 atm is equal to 760mm Hg, you can use the following equation to find the correct atm measurement:

atm x 760

Simply plug the values given in:

0.43 x 760 = 326.8mm Hg


<h2>Hope this helps!</h2>
4 0
4 years ago
In a salt water solution, what is the water?
antoniya [11.8K]
A solute, hope it helps
7 0
3 years ago
Read 2 more answers
PLEASE HELP ASAP. I WILL MARK BRAINLIEST!!!
iris [78.8K]

I Cant Answer your question but maybe this will help

Volume Changes for Gases

Particles in a gas have more freedom of movement than they do in a liquid. According to the ideal gas law, the pressure (P) and volume (V) of a gas are mutually dependent on temperature (T) and the number of moles of gas present (n). The ideal gas equation is PV = nRT, where R is a constant known as the ideal gas constant. In SI (metric) units, the value of this constant is 8.314 joules ÷ mole - degree K.

Pressure is constant: Rearranging this equation to isolate volume, you get: V = nRT ÷ P, and if you keep the pressure and number of moles constant, you have a direct relationship between volume and temperature: ∆V = nR∆T ÷ P, where ∆V is change in volume and ∆T is change in temperature. If you start from an initial temperature T0 and pressure V0 and want to know the volume at a new temperature T1 the equation becomes:

V1 = [n • R • (T1 - T0) ÷ P] +V0

Temperature is constant: If you keep the temperature constant and allow pressure to change, this equation gives you a direct relationship between volume and pressure:

V1 = [n • R • T ÷ (P1 - P0)] + V0

Notice that the volume is larger if T1 is larger than T0 but smaller if P1 is larger than P0.

Pressure and temperature both vary: When both temperature and pressure vary, the the equation becomes:

V1 = n • R • (T1 - T0) ÷ (P1 - P0) + V0

Plug in the values for initial and final temperature and pressure and the value for initial volume to find the new volume.

6 0
3 years ago
Read 2 more answers
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