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Llana [10]
2 years ago
9

There is an equal number of protons and __________ in a neutral atom.

Chemistry
1 answer:
tiny-mole [99]2 years ago
5 0

the answer is electrons

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Forming ionic compounds:
GREYUIT [131]

Answer:

Name Formula and Charge   Name Formula and Charge

ammonium NH4+   hydroxide OH−

acetate C2H3O2−, or CH3COO− nitrate NO3−

bicarbonate (hydrogen carbonate) HCO3− nitrite NO2−

bisulfate (hydrogen sulfate) HSO4− peroxide O22−

carbonate CO32− perchlorate ClO4−

chlorate ClO3− phosphate PO43−

chromate CrO42− sulfate SO42−

cyanide CN− sulfite SO32−

dichromate Cr2O72− triiodide I3−

Explanation:

4 0
3 years ago
Classify each of the following processes as spontaneous or nonspontaneous
Brilliant_brown [7]
What are the processes we are supposed to be classifying?
5 0
3 years ago
The mass of an unidentified rock is 15.5 grams. Students determine the volume of the rock by placing the rock in a cylinder with
Andre45 [30]
The concept of water by displacement. D=m/v therefore m=15.5 g and volume=5 mL (final - initial) then calculate the density
3 0
3 years ago
A 10.00 mL sample of a solution containing formic acid (a weak acid) was placed in a 25 mL volumetric flask and diluted to the m
Eddi Din [679]

Answer:

Molarity: 0.522M

Percentage by mass: 2.36 (w/w) %

Explanation:

Formic acid, HCOOH reacts with NaOH as follows:

HCOOH + NaOH → NaCOOH + H₂O

To solve this question we must find the moles of NaOH added = Moles formic acid. Taken into account the dilution that was made we can find the moles -And molarity of formic acid and its percentage by mass as follows:

<em>Moles NaOH = Moles HCOOH:</em>

0.01580L * (0.1322mol / L) =0.002089 moles HCOOH

<em>Moles in the original solution:</em>

0.002089 moles HCOOH * (25mL / 10mL) = 0.005222 moles HCOOH

<em>Molarity of the solution:</em>

0.005222 moles HCOOH / 0.01000L =

<h3>0.522M</h3>

<em>Mass HCOOH in 1L -Molar mass: 46.03g/mol-</em>

0.522moles * (46.03g / mol) = 24.04g HCOOH

<em>Mass solution:</em>

1L = 1000mL * (1.02g / mL) = 1020g solution

<em>Mass percent:</em>

24.04g HCOOH / 1020g solution * 100

2.36 (w/w) %

7 0
2 years ago
Kc= [3.1*10^-2]^2. (mol/L^2) divide by [8.5*10^-1] [3.1*10^-3]^3 (mol/L)^4​
jok3333 [9.3K]

Answer:

Kc = 12.58

Explanation:

Kc = [0.229]^2*[0.687]^6/[0.221]^4*[0.5685]^3

Kc = (0.052441)(0.10513)/(0.002385)(0.18373)

Kc = 0.0005513/0.000438

Kc = 12.58

Hope that helps!!

5 0
3 years ago
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