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Pepsi [2]
3 years ago
13

What pressure is exerted by 0.625 moles of a gas in a 45.4 L container at -24.0 °C? Find pressure in units of atm.

Chemistry
1 answer:
scoundrel [369]3 years ago
3 0

Answer:

Ok to solve this you will need to use the Ideal Gas Law Formula which is as follows:

PV = nRT

P= pressure

V= volume

n= # of moles

R= Universal Gas Constant (0.0821 L x atm/mol x K)

T= Kelvin temperature

1.Simplify the Ideal Gas Law formula to what you need to solve for:

P = (nRT)/ V

2. List all you components as follows (this makes the process easier):

P = ?

V = 45.4 L

n = 0.625 mol

R = 0.0821 L x atm/ mol x K

T = 249 K

To find the Kelvin temperature K = C + 273

3. Plug in all your components in your set up formula:

P = [(0.625 mol)(0.0821 L x atm/ mol x K)(249 K)] / (45.4 L)

4. Cross out all similar units so the only thing left is atm because you are trying to find pressure.

P = [(0.625)(0.0821atm)(249)] / (45.4)

5. Multiply through and simplify

P = 0.28 atm

B. is the correct answer.

Glad I could help!! If you have any other questions just message me. Hopefully this was helpful.

Explanation:

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What volume of 0.160 m li2s solution is required to completely react with 130 ml of 0.160 m co no3 2?
Over [174]
The  volume  of  0.160    m   Li2S  solution  required  to  completely  react  with  130 ml  of 0.160  CO(NO3)2  is calculated   as  below

write the  reacting  equation

Co(NO3)2 +  Li2S = 2LiNO3  +  COS

find the    moles  of CO(NO3)2  = molarity  x  volume

=  130 ml  x  0.160=20.8  moles

since the reacting moles between CO(NO3)2  to LiS  is   1:1  the  moles of LiS  is  also  20.8  moles

volume  of Lis  is  therefore =  moles of Lis/ molarity  of LiS

=  20.8/0.160 =  130 Ml
3 0
3 years ago
Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of nitrogen and oxygen in the air: N2 (g) + O2 (g) ↔ NO (
Solnce55 [7]

Answer:

The equilibrium concentration of NO is 0.001335 M

Explanation:

Step 1: Data given

The equilibrium constant Kc is 0.0025 at 2127 °C

An equilibrium mixture contains 0.023M N2 and 0.031 M O2,

Step 2: The balanced equation

N2(g) + O2(g) ↔ 2NO(g)

Step 3:  Concentration at the equilibrium

[N2] = 0.023 M

[O2] = 0.031 M

Kc = 0.0025 = [NO]² / [N2][O2]

Kc = 0.0025 = [NO]² / (0.023)(0.031)

[NO] = 0.001335 M

The equilibrium concentration of NO is 0.001335 M

6 0
3 years ago
What is the theoretical yield of aluminum oxide if 1.40 mol of aluminum metal is exposed to 1.35 mol of oxygen?
jasenka [17]

Answer:

71.372 g or 0.7 moles

Explanation:

We are given;

  • Moles of Aluminium is 1.40 mol
  • Moles of Oxygen 1.35 mol

We are required to determine the theoretical yield of Aluminium oxide

The equation for the reaction between Aluminium and Oxygen is given by;

4Al(s) + 3O₂(g) → 2Al₂O₃(s)

From the equation 4 moles Al reacts with 3 moles of oxygen to yield 2 moles of Aluminium oxide.

Therefore;

1.4 moles of Al will require 1.05 moles (1.4 × 3/4) of oxygen

1.35 moles of Oxygen will require 1.8 moles (1.35 × 4/3) of Aluminium

Therefore, Aluminium is the rate limiting reagent in the reaction while Oxygen is the excess reactant.

4 moles of aluminium reacts to generate 2 moles aluminium oxide.

Therefore;

Mole ratio Al : Al₂O₃ is 4 : 2

Thus;

Moles of Al₂O₃ = Moles of Al × 0.5

                         = 1.4 moles × 0.5

                         = 0.7 moles

But; 1 mole of Al₂O₃ = 101.96 g/mol

Thus;

Theoretical mass of Al₂O₃ = 0.7 moles × 101.96 g/mol

                                            = 71.372 g

3 0
3 years ago
2. When paleontologists study fossils, which is true of the fossil record that they find?
juin [17]

Answer:

Explanation:

d

7 0
3 years ago
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The answer is for this is A
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