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Dimas [21]
3 years ago
7

What is an atom? how can we predict it?

Chemistry
1 answer:
sattari [20]3 years ago
5 0

An atom is the what makes up elements. It is made up of positive particles (protons), negative particles (electrons), and neutrons (no charged particles).

Protons and neutrons are in the center of the atom while electrons hover around.

You cannot predict an atom. This is because it is not anything to guess about -if you know what I mean.

Happy to help!

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You want to make 500 ml of a 1 N solution of sulfuric acid (H2SO4, MW: 98.1). How many grams of sulfuric acid do you need?
umka21 [38]

Answer:

24.525 g of sulfuric acid.

Explanation:

Hello,

Normality (units of eq/L) is defined as:

N=\frac{eq_{solute}}{V_{solution}}

Since the sulfuric acid is the solute, and we already have the volume of the solution (500 mL) but we need it in liters (0.5 L, just divide into 1000), the equivalent grams of solute are given by:

eq_{solute}=N*V_{solution}=1\frac{eq}{L}*0.5L=0.5 eq

Now, since the sulfuric acid is diprotic (2 hydrogen atoms in its formula) 1 mole of sulfuric acid has 2 equivalent grams of sulfuric acid, so the mole-mass relationship is developed to find its required mass as follows:

m_{H_2SO_4}=0.5eqH_2SO_4(\frac{1molH_2SO_4}{2 eqH_2SO_4}) (\frac{98.1 g H_2SO_4}{1 mol H_2SO_4} )\\m_{H_2SO_4}=24.525 g H_2SO_4

Best regards.

4 0
3 years ago
Please help!!
Zinaida [17]
1.B
6.D 
D because t<span>he mass of one mole (molar mass) of helium gas is </span>4.002602 g/mol. 4.002602 * 5=20.01309. Rounded equals 20. So, the answer is D.20 g.
8 0
2 years ago
Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22°C and 100 kPa?
LenKa [72]

The volume could be calculated by using  <span>V = n RT / P </span>

In which V = Volume
n = number of Moles
R= The Gas constant
T = Temperature (ideally this would be in Kelvin, but i don't see it in the option)
P = Pressure


I believe the answer is

 <span>V = (1.5mol) (0.08205 L*kPa/K*mol) (22Celsius)/100 kPa 


</span>
6 0
3 years ago
What effects do catalysts have on chemical reactions?
cupoosta [38]

Answer:

3

Explanation:

8 0
2 years ago
When a hydrogen atom makes the transition from the second excited state to the ground state (at -13.6 eV) the energy of the phot
viktelen [127]

Answer : The energy of the photon emitted is, -12.1 eV

Explanation :

First we have to calculate the 'n^{th}' orbit of hydrogen atom.

Formula used :

E_n=-13.6\times \frac{Z^2}{n^2}ev

where,

E_n = energy of n^{th} orbit

n = number of orbit

Z = atomic number  of hydrogen atom = 1

Energy of n = 1 in an hydrogen atom:

E_1=-13.6\times \frac{1^2}{1^2}eV=-13.6eV

Energy of n = 2 in an hydrogen atom:

E_3=-13.6\times \frac{1^2}{3^2}eV=-1.51eV

Energy change transition from n = 1 to n = 3 occurs.

Let energy change be E.

E=E_-E_3=(-13.6eV)-(-1.51eV)=-12.1eV

The negative sign indicates that energy of the photon emitted.

Thus, the energy of the photon emitted is, -12.1 eV

3 0
2 years ago
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