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solniwko [45]
3 years ago
14

‘solution 1', ‘solution 2', and ‘solution 3'. present one solution when each menu button is clicked.

Chemistry
1 answer:
arlik [135]3 years ago
7 0
What are you trying to ask?
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Explain why a single atom of hydrogen cannot produce all four hydrogen spectral lines simultaneously.
brilliants [131]
<span>When the electron in a hydrogen atom transitions from a high energy state to a lower energy state, the energy lost from the electron is used to produce a photon corresponding to the loss of energy. That photon will correspond to exactly 1 wavelength. And since a hydrogen atom has only 1 electron, at any given moment, it can only produce 1 photon. And in order to simultaneously produce 4 photons for 4 spectral lines, that would require a simultaneous transition of 4 electrons which is 3 too many for a hydrogen atom.</span>
7 0
3 years ago
What type of variable should there only be one of in an experiment? A) dependent B) independent C) control D) responding​
gavmur [86]
B) independent


here’s the explanation

3 0
3 years ago
A buffer is made that is .10M propanoic acid (pKa = 4.9) and .05M sodium propanoate. Calculate the pH.
inna [77]
PKa= 4.9 therefore ka= 10^-4.9=  1.259x10^-5

ka= \frac{[H^+][CH3CH2COO^-]}{[CH3CH2COOH]}

[CH3CH2COO^-]&#10;= 0.05
[CH3CH2COOH]= 0.10

Therefore 1.259x10^-5 = \frac{[H^+][0.05]}{[0.1]}
Rearrange the equation to make the concentration of hydrogen the subject.
Therefore [H^+] =  \frac{(1.259*10^-5)(0.1)}{0.05}

Therefore [H^+]= 2.513*10^-5

pH= -log [H^+] = -log(2.513*10^-5)= 4.59.
7 0
3 years ago
230g sample of a compound contains 136.6g carbon, 26.4g hydrogen, and 31.8g nitrogen. What is masspercentif oxygen
natulia [17]

Answer:

15.3 %

Explanation:

Step 1: Given data

  • Mass of the sample (ms): 230 g
  • Mass of carbon (mC); 136.6 g
  • Mass of hydrogen (mH): 26.4 g
  • Mass of nitrogen (mN): 31.8 g

Step 2: Calculate the mass of oxygen (mO)

The mass of the sample is equal to the sum of the masses of all the elements.

ms = mC + mH + mN + mO

mO = ms - mC - mH - mN

mO = 230 g - 136.6 g - 26.4 g - 31.8 g

mO = 35.2 g

Step 3: Calculate the mass percent of oxygen

%O = (mO / ms) × 100% = (35.2 g / 230 g) × 100% = 15.3 %

6 0
3 years ago
Particle quantity/number of Cu(NO3)2
Murrr4er [49]

Answer:

Cupid nitrate is what I'm going for

8 0
3 years ago
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