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lidiya [134]
2 years ago
13

What should you be careful of when measuring the temperature of a liquid in a beaker

Chemistry
1 answer:
andrezito [222]2 years ago
3 0

The precaution to be taken while measuring the temperature of a liquid in a beaker is applying proper heat balance and taking all the required precautions.

  • A beaker with an open top contains a sample of liquid. It exposes this sample to light.
  • That liquid absorbs the light energy, turning it into heat energy. As a result, the liquid becomes warmer and evaporation is accelerated. As a result, there is less liquid in the beaker.
  • Since it is well known that the surface temperature of a liquid, along with air movement above the liquid surface, is one of the dominant factors affecting evaporation, I want to measure the evaporation rate as a function of surface temperature.
  • This can be done by applying a heat balance.

Learn more about heat balance at:

brainly.com/question/1292905

#SPJ9

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1 mole of nacl(s) has a greater entropy than 1 mole of nacl(aq). true or false g
Svetradugi [14.3K]
It  is  false   that  1  mole  of  nacl(s)  has  a  greater  entropy  than   1  mole  of  nacl (aq).  

  this  is  because    nacl(aq)   is  in  aqueous  state  while  nacl(s)  is  in  solid  state.  Nacl(aq)  has  greater  entropy  than  nacl(s)  because    in 
aqueous   state  their   is  increase  in  entropy. the  entropy   of  the  two  ions  in  water  has   greater  entropy  than  the  solid   nacl.
3 0
3 years ago
A chef finds a sealed container consisting of an ingredient that goes into his restaurant’s secret sauce. The ingredient’s molec
ozzi

The ingredient's molecules would be more free and move faster, then the phase would change to liquid from solid.

<u>Explanation</u>:

  • This task seeks to examine the knowledge of the kinetic phase and characteristics of matters.
  • Here we see the chef described that the ingredient's molecules are moving in place – solid.
  • On the advent of causing the ingredient to change phase by transferring energy into it – the ingredient's molecules would be more free and move faster, then the phase would change to liquid from solid.

6 0
2 years ago
What is the molar mass of Aul ​
torisob [31]

Answer:

no idea

Explanation:

7 0
3 years ago
Suppose 0.708g of copper(II) acetate is dissolved in 50.mL of a 46.0mM aqueous solution of sodium chromate.
lisabon 2012 [21]

Answer:

The final molarity of acetate anion in the solution is 0.0046 moles

Explanation:

The balanced equation is

Cu(C₂H₃O₂)₂ + Na₂CrO₄ = CuCrO₄ + 2Na(C₂H₃O₂)

Therefore one mole of Cu(C₂H₃O₂)₂ react with one mole of Na₂CrO₄ to form one mole of CuCrO₄ and two moles of Na(C₂H₃O₂)

Mass of copper (II) acetate present = 0.708 g

Volume of aqueous sodium present = 50 mL

Molarity of sodium chromate = 46.0 mM

Therefore

Number of moles of sodium chromate present = (50 mL/1000)×46/1000 = 0.0023 M

Number of moles of copper (II) acetate present = 181.63 g/mol

number of moles of copper (II) acetate present = (0.708 g/181.63 g/mol) =0.0039 moles

Therefore 0.0039 moles of Cu(C₂H₃O₂)₂ × (2 moles of Na(C₂H₃O₂))/1 Cu(C₂H₃O₂)₂) = 0.00779 moles of Na(C₂H₃O₂)

also 0.0023 moles of Na₂CrO₄ × (2 moles of Na(C₂H₃O₂))/1 Na₂CrO₄) = 0.0046 moles of Na(C₂H₃O₂)

Therefore the Na₂CrO₄ is the limiting reactant and 0.0046 moles of Na(C₂H₃O₂) or acetate anion is formed

7 0
2 years ago
Consider the chemical system co + cl2 cocl2; k = 4.6 ? 109 l/mol. 2. how do the equilibrium concentrations of the reactants comp
ikadub [295]
<span>they are much bigger because </span><span>equilibrium constant shows ratio of  </span><span>concentrations of the reactants to the equilibrium concentration of the product.</span>
3 0
3 years ago
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