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3 years ago

In which state of matter are the particles at rest (not moving at all)?

Chemistry

2 answers:

Sidana [21]3 years ago

8 0

Answer:

Solids for sure

particles of solid cant flow.

miss Akunina [59]3 years ago

4 0

Answer:

B)Solids

Solids have tightly packed particles unlike liquids and gases whose particles can move freely but rate of movement is highest in gas while compared to water

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The molar mass of K2S is 110.27 g/mol. What is the mass of 2.75 moles K2S? [?] g K₂S

aliya0001 [1]

The mass of 2.75 mol K₂S is 303.24 grams.

Applying the mole concept:

Number of moles(n) = given mass(m) / molar mass(M)

n = m / M

Now applying the formula for the number of moles-

i.e. number of moles of K₂S = mass of K₂S / Molas mass of K₂S

As per question, Molar mass of K₂S, M = 110.27 g/mol

and, number of moles of K₂S, n = 2.75 moles

∴ n = m / 110.27

2.75 = m / 110.27

m = 2.75 x 110.27

= 303.24

m = 303.24 grams.

Hence, the mass of 2.75 mol K₂S is 303.24 grams.

To learn more about the mole concept, refer to:

brainly.com/question/768852

# SPJ2

6 0

2 years ago

A same of gas in a rigid container is at 25.0Cand 1.00atm. What is the pressure of the sample when heated to 220.0C

Crazy boy [7]

Answer:

1.654 atm.

Explanation:

We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

If n and V are constant, and have different values of P and T:

(P₁T₂) = (P₂T₁)

Knowing that:

P₁ = 1.0 atm, T₁ = 25°C + 273 = 298 K,

P₂ = ??? atm, T₂ = 220°C + 273 = 493 K,

Applying in the above equation

(P₁T₂) = (P₂T₁)

∴ P₂ = (P₁T₂)/(T₁) = (1.0 atm)(493 K)/(298 K) = 1.654 atm.

7 0

3 years ago

What is the calculated value of the cell potential at 298K for an

Tpy6a [65]

The question is incomplete, here is the complete question:

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H₂ pressure is 6.56 x 10⁻² atm, the H⁺ concentration is 1.39 M, and the Sn²⁺ concentration is 9.35 x 10⁻⁴ M?

$2H^+(aq)+Sn(s)\rightarrow H_2(g)+Sn^{2+}(aq)$

Answer: The cell potential of the given electrochemical cell is 0.273 V

Explanation:

For the given chemical equation:

$2H^+(aq)+Sn(s)\rightarrow H_2(g)+Sn^{2+}(aq)$

The half cell reactions for the given equation follows:

Oxidation half reaction: $Sn(s)\rightarrow Sn^{2+}(aq)+2e^-;E^o_{Sn^{2+}/Sn}=-0.14V$

Reduction half reaction: $H_2+2e^-\rightarrow H_2(g);E^o_{2H^{+}/H_2}=0.0V$

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

Putting values in above equation, we get:

$E^o_{cell}=0.0-(-0.14)=0.14V$

To calculate the EMF of the cell, we use the Nernst equation, which is:

$E_{cell}=E^o_{cell}-\frac{0.059}{n}\log \frac{[Sn^{2+}]\times p_{H_2}}{[H^+]^2}$

where,

$E_{cell}$ = electrode potential of the cell = ?

$E^o_{cell}$ = standard electrode potential of the cell = +0.14 V

n = number of electrons exchanged = 2

$[H^{+}]=1.39M$

$[Sn^{2+}]=9.35\times 10^{-4}M$

$p_{H_2}=6.56\times 10^{-2}atm$

Putting values in above equation, we get:

$E_{cell}=0.14-\frac{0.059}{2}\times \log(\frac{(9.35\times 10^{-4})\times (6.56\times 10^{-2})}{(1.39)^2})\\\\E_{cell}=0.273V$

Hence, the cell potential of the given electrochemical cell is 0.273 V

4 0

3 years ago

Use your understanding of the ideal gas law to

WITCHER [35]

Answer:
Pressure is inversely related to volume.
Temperature is inversely related to moles.
Volume is inversely related to pressure.
Moles are inversely related to temperature.

6 0

3 years ago

Write a balanced chemical equation for the reaction that occurs when barium carbonate decomposes into barium oxide and carbon di

n200080 [17]

BaCO3=BaO+CO2
IS THE EQUATION REPLACE = WITH AN ARROW.

4 0

3 years ago