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DiKsa [7]
3 years ago
5

Please match these thanks and have a great day!!! :)) due in 4 minutes

Chemistry
1 answer:
valentina_108 [34]3 years ago
6 0

Answer:

fist one is freezing next two is condensation

Explanation:

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In-s [12.5K]
C) is correct, because there are 2 carbons and 4 oxygens on both sides, making the equation balanced.
7 0
3 years ago
How did Dalton gather evidence for the existence of atoms?
Morgarella [4.7K]

Dalton gathers evidence for the existence of atoms by measuring the masses of elements after compounds are formed.

<u>Explanation</u>:

  • John Dalton accumulated proof for the presence of atoms by estimating the majority of components that responded to frame mixes. All components are made out of molecules. All particles of a similar component have a similar mass, and atoms of various components have various masses. Mixes contain atoms of more than one component.  
  • Dalton did numerous investigations that gave proof to the presence of particles. For instance, He researched pressure and different properties of gases, from which he induced that gases must comprise of little, singular particles that are in steady, arbitrary movement.
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3 years ago
What are Kr and Xe. (elements)?
nasty-shy [4]
The elements are Krypton and Xenon
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3 years ago
The exhaust gas from an automobile contains 1.5 percent by volume of carbon monoxide. What is the concentration of CO in mg/m' a
FrozenT [24]

Answer:

(a) 17,178 mg/m3

(b) 11,625 mg/m3

Explanation:

The concentration of CO in mg/m3 can be calculated as

C (mg/m3) =(P/RT)*MW*C_{ppm}

For standard conditions (1 atm and 25°C), P/RT is 0.0409.

Concentration of 1.5% percent by volume of CO is equivalent to 1.5*10,000 ppm= 15,000 ppm CO.

The molecular weigth of CO is 28 g/mol.

(1) For 25°C and 1 atm conditions

C=(P/RT)*MW*C_{ppm}\\\\C=0.0409*28*15,000=17,178

(b) For 200°C and 1.1 atm,

P/RT=0.0409*(P/P_{std})*(T_{std}/T)\\P/RT=0.0409*(1.1atm/1atm)*(273+15K/273+200K)=0.0277

Then the concentration in mg/m3 is

C=(P/RT)*MW*C_{ppm}\\\\C=0.0277*28*15,000=11,625

5 0
2 years ago
A typical aspirin tablet contains 500. mg of c9h8o4. how many moles of c9h8o4 molecules and how many molecules of acetylsalicyli
joja [24]
From the periodic table:
molar mass of carbon = 12 gm
molar mass of hydrogen = 1 gm
molar mass of oxygen = 16 gm

molar mass of <span>acetylsalicylic acid = 9(12) + 8(1) + 4(16) = 180 gm

Number of moles = mass / molar mass = 0.5 / 180 = 2.778 x 10^-3 moles

To get the number of molecules, we multiply the number of moles by Avogadro's number as follows:
number of molecules = </span>2.778x10^-3x6.02x10^23 =1.672 x 10^21 molecules
6 0
3 years ago
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