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crimeas [40]
3 years ago
11

an ------ model with dark bands representing energy levels shows where an atoms electrons are most likely to be.

Chemistry
1 answer:
oksano4ka [1.4K]3 years ago
7 0
Is it an atomic model? I'm not really sure
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The density of whole milk 1.04 g per mL. What is the volume (in quarts) of 18.5 pounds of whole milk?
nadya68 [22]

The volume : 8,526 quarts

<h3>Further explanation</h3>

Given

The density of whole milk = 1.04 g/ml

mass = 18.5 pounds

Required

The volume

Solution

Conversion of mass

1 pound = 453,592 g

18.5 pounds = 8391,45 g

Density formula:

\large{\boxed {\bold {\rho~=~ \frac {m} {V}}}}.

Input the value :

V = m : ρ

V = 8391,45 g : 1.04 g/ml

V = 8068.7 ml

1 ml = 0,00105669 quarts

8068.7 ml =8,526 quarts

3 0
2 years ago
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0- L vessel at 300 K . The following equilibr
umka2103 [35]

Answer:

The concentration of N2 at the equilibrium will be 0.019 M

Explanation:

Step 1: Data given

Number of moles of NO = 0.10 mol

Number of moles of H2 = 0.050 mol

Number of moles of H2O = 0.10 mol

Volume = 1.0 L

Temperature = 300K

At equilibrium [NO]=0.062M

Step 2: The balanced equation

2NO(g) + 2H2(g) → N2(g) + 2H2O(g)

Step 3: Calculate the initial concentration

Concentration = Moles / volume

[NO] = 0.10 mol / 1L = 0.10 M

[H2] = 0.050 mol / 1L = 0.050 M

[H2O] = 0.10 mol / 1L = 0.10 M

[N2] = 0 M

Step 4: Calculate the concentration at the equilibrium

[NO] at the equilibrium is 0.062 M

This means there reacted 0.038 mol (0.038M) of NO

For 2 moles NO we need 2 moles of H2 to produce 1 mol N2 and 2 moles of H2O

This means there will also react 0.038 mol of H2

The concentration at the equilibrium is 0.050 - 0.038 = 0.012 M

There will be porduced 0.038 moles of H2O, this means the final concentration pf H2O at the equilibrium is 0.100 + 0.038 = 0.138 M

There will be produced 0.038/2 = 0.019 moles of N2

The concentration of N2 at the equilibrium will be 0.019 M

5 0
3 years ago
What is the mass of 3.20x10^23 formula units of iron (III) oxide (Fe2O3)?
yaroslaw [1]

The mass of iron (III) oxide (Fe2O3) : 85.12 g

<h3>Further explanation</h3>

Given

3.20x10²³ formula units

Required

The mass

Solution

1 mole = 6.02.10²³ particles  

Can be formulated :

N = n x No

N = number of particles

n = mol

No = 6.02.10²³ = Avogadro's number

mol of Fe₂O₃ :

\tt n=\dfrac{3.2.10^{23}}{6.02.10^{23}}=0.532

mass of Fe₂O₃ (MW=160 g/mol)

\tt mass=mol\times MW=0.532\times 160=85.12~g

4 0
2 years ago
Help me due tomorrow :,)
lesya [120]

#a

  • Zinc displaces copper

It means

  • Zinc is more reactive than copper

#b

  • Zinc+Copper sulphate--> Zinc sulphate+Copper

#c

No reaction because

  • Magnesium is more reactive than zinc

#d

Reaction occurs

  • Iron is more reactive than copper
  • Magnesium is more reactive than iron

Order:-

  • Cu<Fe<Zn<Mg
3 0
3 years ago
How many atoms are in a sample of 0.75 moles of carbon atoms
vova2212 [387]

Answer: 4.5165 *10^-23 moles Carbon

Explanation:

There are 6.022*10^23 atoms in a mole.

Therefore, there would be 6.022*10^-23*0.75 atoms in 0.75 moles of Carbon.

= 4.5165 *10^-23 moles Carbon

8 0
3 years ago
Read 2 more answers
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