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natali 33 [55]
2 years ago
11

Which on goes where please help!!!

Chemistry
1 answer:
EastWind [94]2 years ago
6 0
Pretty easy.. The ice is a solid, the rain is a liquid the drink is a liquid, the water drain is a liquid, the wood is a solid,
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1 2 3 4 5 6 7 8 9 10TIME REMAINING53:56A scientist told his student assistants that he had sorted groups of mice by their intell
Gekata [30.6K]

Answer:

People can introduce their own biases into an experiment.

Explanation:

4 0
2 years ago
The equilibrium 2NO(g)+Cl2(g)⇌2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures
QveST [7]

<u>Answer:</u>

<u>For A:</u> The K_p for the given reaction is 4.0\times 10^1

<u>For B:</u> The K_c for the given reaction is 1642.

<u>Explanation:</u>

The given chemical reaction follows:

2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)

  • <u>For A:</u>

The expression of K_p for the above reaction follows:

K_p=\frac{(p_{NOCl})^2}{(p_{NO})^2\times p_{Cl_2}}

We are given:

p_{NOCl}=0.24 atm\\p_{NO}=9.10\times 10^{-2}atm=0.0910atm\\p_{Cl_2}=0.174atm

Putting values in above equation, we get:

K_p=\frac{(0.24)^2}{(0.0910)^2\times 0.174}\\\\K_p=4.0\times 10^1

Hence, the K_p for the given reaction is 4.0\times 10^1

  • <u>For B:</u>

Relation of K_p with K_c is given by the formula:

K_p=K_c(RT)^{\Delta ng}

where,

K_p = equilibrium constant in terms of partial pressure = 4.0\times 10^1

K_c = equilibrium constant in terms of concentration = ?

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature = 500 K

\Delta ng = change in number of moles of gas particles = n_{products}-n_{reactants}=2-3=-1

Putting values in above equation, we get:

4.0\times 10^1=K_c\times (0.0821\times 500)^{-1}\\\\K_c=\frac{4.0\times 10^1}{(0.0821\times 500)^{-1})}=1642

Hence, the K_c for the given reaction is 1642.

7 0
2 years ago
Please help ASAP
DochEvi [55]
Aluminum. chemical element with symbol Al
4 0
3 years ago
The nonvolatile, nonelectrolyte DDT , C14H9Cl5 (354.5 g/mol), is soluble in benzene, C6H6. Calculate the osmotic pressure (in at
Ainat [17]

Step 1

The osmotic pressure is calculated as follows:

\begin{gathered} \pi\text{ = C x R x T} \\ C\text{ = molarity = }\frac{moles\text{ of solute}}{Volume\text{ of solution \lparen L\rparen}} \\ R\text{ = 0.082 }\frac{atmxL}{mol\text{ x K}} \end{gathered}

-------------

Step 2

<em>Information provided:</em>

The mass of solute = 13.6 g

Volume of solution = 251 mL

Absolute temperature = T = 298 K

The molar mass of solute = M = 354.5 g/mol

-------------

Step 3

Procedure:

1 L = 1000 mL => Volume = 251 mL x (1 L/1000 mL) = 0.251 L

---

C = moles of solute/volume of solution (L)

C = mass of solute/(molar mass x Volume (L))

C = 13.6 g/(354.5 g/mol x 0.251 L)

C = 0.153 mol/L

---

π = C x R x T

π = 0.153 mol/L x 0.082 atm L/mol K x 298 K

π = 3.74 atm

Answer: π = 3.74 atm

4 0
1 year ago
Choose the description that matches the law of included fragments.
GREYUIT [131]

Answer:

The answer is B

Explanation:

3 0
2 years ago
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