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Feliz [49]
2 years ago
7

Is it possible for a balloon with an initial pressure of 200.0 kPa to naturally expand to four times its initial volume when the

temperature remains constant and atmospheric pressure is 101.3kPa?
Chemistry
1 answer:
seropon [69]2 years ago
3 0
Yes it is possible for a balloon to expand under these conditions. When objects are exposed to an atmospheric pressure beyond their capabilities, their physical characteristics change. This is because, molecules within the balloon are constantly moving and reacting to its external environment.
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Particles in a liquid move around just as freely as particles in a solid.
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It is false :D I am 95% sure
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3 years ago
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What would be the mass of a 33.5dm3 sample of O2 at STP?
liraira [26]

Answer:

• One mole of oxygen is equivalent to 16 grams.

→ But at STP, 22.4 dm³ are occupied by 1 mole.

{ \tt{22.4 \:  {dm}^{3}   \: \dashrightarrow \: 16 \: grams}} \\  { \tt{33.5 \:  {dm}^{3}  \:  \dashrightarrow \: ( \frac{33.5 \times 16}{22.4} ) \: grams}} \\  \\  \dashrightarrow \: { \boxed{ \tt{23.94 \: g \approx \: 24 \: grams}}}

7 0
2 years ago
The particle picture is best described as...
mixas84 [53]

Answer:

Both are pure substances and a compound

8 0
3 years ago
List the elements and the amounts of each element below for 5 Li2S04.​
GREYUIT [131]

Answer:

Lithium has 5 elements, sulphur has 2 elements and oxygen has 4 elements

7 0
3 years ago
Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete
neonofarm [45]

Answer:

The amount of energy required to transport hydrogen ions from a cell into the stomach is 37.26KJ/mol.

Explanation:

The free change for the process can be written in terms of its equilibrium constant as:

ΔG° = -RTInK_(eq)

where:

R= universal gas constant

T= temperature

K_eq= equilibrum constant for the process

Similarly, free energy change and cell potentia; are related to each other as follows;

ΔG= -nFE°

from above;

F = faraday's constant

n = number of electrons exchanged in the process; and  

E = standard cell potential

∴ The amount of energy required for transport of hydrogen ions from a cell into stomach lumen can be calculated as:

ΔG° = -RTInK_(eq)

where;

[texK_eq[/tex]=\frac{[H^+]_(cell)}{[H^+(stomach lumen)]}

For transport of ions to an internal pH of 7.4, the transport taking place can be given as:

H^+_{inside} ⇒ H^+_{outside}

Equilibrum constant for the transport is given as:

K_{eq}=\frac{[H^+]_{outside}}{[H^+]_{inside}}

=\frac{[H^+]_{cell}}{[H^+]_{stomach lumen}}

[H^+]_{cell}= 10⁻⁷⁴

=3.98 * 10⁻⁸M

[H^+]_{stomach lumen} = 10⁻²¹

=7.94 * 10⁻³M

Hence;

K_{eq}=\frac{[H^+]_{cell}}{[H^+]_{stomachlumen}}

=\frac{3.98*10^{-8}}{7.94*10{-3}}

= 5.012 × 10⁻⁶

Furthermore, free energy change for this reaction is related to the equilibrium concentration given as:

ΔG° = -RTInK_(eq)

If temperature T= 37° C ; in kelvin

=37° C + 273.15K

=310.15K; and

R-= 8.314 j/mol/k

substituting the values into the equation we have;

ΔG₁ = -(8.314J/mol/K)(310.15)TIn(5.0126*10^{-6})

= 31467.93Jmol⁻¹

≅ 31.47KJmol⁻¹

If the potential difference across the cell membrane= 60.0mV.

Energy required to cross the cell membrane will be:

ΔG₂ = -nFE°_{membrane}

ΔG₂ = -(1 mol)(96.5KJ/mol/V)(60*10^{-3})

= 5.79KJ

Therefore, for one mole of electron transfer across the membrane; the energy required is 5.79KJmol⁻¹

Now, we  can calculate the total amount of energyy required to transport H⁺ ions across the membrane:

Δ G_{total} = G_{1}+G_{2}

= (31.47+5.79) KJmol⁻¹

= 37.26KJmol⁻¹

We can therefore conclude that;

   The amount of energy required to transport ions from cell to stomach lumen is 37.26KJmol⁻¹

5 0
3 years ago
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