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Diano4ka-milaya [45]
3 years ago
14

At what temperature would 0.500 moles of gas particles stored in a 100.0 mL container reach a pressure of 15.0 atm?

Chemistry
2 answers:
pychu [463]3 years ago
8 0
We use the ideal gas equation in order to calculate the temperature of the system. It is expressed as follows:

PV=nRT

where P is pressure, V is volume, n is the number of moles, R is the universal gas constant and T is the temperature.

15 atm (.1 L) = 0.5 mol (0.08206 L-atm / mol-K) T
T = 36.56 K

Hope this answers the question. Have a nice day.
sergeinik [125]3 years ago
4 0

Ideal gas law: p·V = n·R·T.

p = 15.0 atm; pressure of gas.

V = 100 mL ÷ 1000 mL/L.

V = 0.100 L; volume of gas.

n = 0.500 mol; amount of substance.

R = 0,08206 L·atm/mol·K; universal gas constant.

T = ?; temperature of gas.

T(gas) = p · V ÷ (R · n).

T(gas) = 15.0 atm · 0.1 L ÷ (0,08206 L·atm/mol·K · 0.5 mol).

T(gas) =  36,500 K; calculation is correct.


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Zigmanuir [339]

molar concentration of AgNO₃ solution = 0.118 mole/L

Explanation:

Because we have the volume of the solution and there is no information about the density of the solution I will asume that you ask for the molar concentration.

number of moles = mass / molecular weight

number of moles of AgNO₃ = 10 / 170 = 0.0588

molar concentration = number of moles / volume (L)

molar concentration of AgNO₃ solution = 0.0588 / 0.5

molar concentration of AgNO₃ solution = 0.118 mole/L

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3 years ago
A sample of barium nitrate is placed into a jar containing water. The mass of the barium nitrate sample is 27g. Assume the water
34kurt
So we have Barium nitrate with a solubility of 8.7g in 100g water at 20°C.

using that relation
i.e.
8.7g (barium nitrate) =100g (water)
1g barium nitrate = 100/8.7 g water

27g barium nitrate = (100/ 8.7 ) × 27
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5 0
3 years ago
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Determine the molar concentration of na+ and po4 3- in a 2.25 M Na3 PO4 solution
muminat

Answer:

A. The concentration of Na^+ in the solution is 6.75 M.

B. The concentration of PO4^3- in the solution is 2.25 M.

Explanation:

We'll begin by writing the balanced dissociation equation for Na3PO4.

This is illustrated below:

Na3PO4 will dissociate in solution as follow:

Na3PO4(aq) —> 3Na^+(aq) + PO4^3-(aq)

Thus, from the balanced equation above,

1 mole of Na3PO4 produce 3 moles of Na^+ and 1 mole of PO4^3-

A. Determination of the concentration of Na+ in 2.25 M Na3PO4 solution.

This can be obtained as follow:

From the balanced equation above,

1 mole of Na3PO4 produce 3 moles of Na^+.

Therefore, 2.25 M Na3PO4 solution will produce = (2.25 x 3) /1 = 6.75 M Na^+.

Therefore, the concentration of Na^+ in the solution is 6.75 M

B. Determination of the concentration of PO4^3- in 2.25 M Na3PO4 solution.

This can be obtained as follow:

From the balanced equation above,

1 mole of Na3PO4 produce 1 mole of PO4^3-

Therefore, 2.25 M Na3PO4 solution will also produce 2.25 M PO4^3-.

Therefore, the concentration of PO4^3- in the solution is 2.25 M.

7 0
3 years ago
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musickatia [10]

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We can <u>find the equivalent number of O₂ molecules for 100 molecules of CO₂</u> using a <em>conversion factor containing the stoichiometric coefficients of the balanced reaction</em>, as follows:

  • 100 molecules CO₂ * \frac{6moleculesO_2}{4moleculesCO_2} = 150 molecules O₂

150 molecules of O₂ would produce 100 molecules of CO₂.

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Nat2105 [25]
ANSWER- ocean winds can carry moisture with then mmm and can bring rain.

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2 years ago
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