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3 years ago

2. If 1.75 L of a gas is at 700. K and is under 250. kPa of pressure, what will the new

Chemistry

1 answer:

Andrews [41]3 years ago

3 0

Answer:

Final volume is 3.50L

Explanation:

It is possible to find volume of a gas using combined gas law:

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

<em>Where P is pressure, V is volume and T is temperature of 1: initial state and 2: final state</em>

If initial state of the gas is:

1.75L of a gas is at 700K and is under 250kPa of pressure

And final state is:

298K and 53.2kPa.

Replacing:

$\frac{250kPa*1.75L}{700K} =\frac{53.2kPa*V_2}{298K}$

0.625L = 0.1785*V₂

Thus, <em>final volume is 3.50L</em>

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WRITE THE ELECTRONIC CONFIGURATION OF THE FOLLOWING ELEMENT

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Answer:WHAT IS THE ELEMENT NAME?

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3 years ago

Just as carbon dating is used to measure the age of organic material, Argon-40 can be used to measure the age of rocks. A volcan

arsen [322]

Answer:

3.77 mg of K-40 decayed into Ar-40.

Data:

1) K-40, Ca-40, Ar-40: all three have the same atomic mass

2) 90% of the potassium-40 will decay into calcium-40

3) 10% of the potassium-40 will decay into argon-40.

4) K-40 inside the rock = 0.81 mg

5) Ar-40 trapped = 0.377 mg

Soltuion:

1) 0.377 mg of Ar-40 is the 10% of the mass of the K-40 that decayed

=> x * 10% = 0.377 mg => x * 0.1 = 0.377mg

=> x = 0.377 mg / 0.1 = 3.77 mg

That means that 3.77 mg of K-40 decayed into Ar-40. And this is the answer to the question.

Additionaly, you can analyze the content of all K-40 and Ca-40, to understand better the case.

2) The mass of the K-40 that decayed into Ca-40 is 9 times (ratio 9:1) the amount that decayed into Ar-40 =>

mass of K-40 that decayed into Ca-40 = 9 * 0.377 = 3.393 mg

3) Total amount of K-40 that decayed = amount that decayed into Ar-40 + amount that decayed into Ca-40 = 0.377mg + 3.393mg = 3.77 mg

4) Original amount of K-40 = amount of K-40 that decayed + amount of K-40 present in the rock = 3.77mg + 0.81 mg = 4.58 mg

5) amount of K-40 that decayed into Ar-40 as percent

% = [3.77 mg / 4.58mg] * 100 = 82.31 %.

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4 years ago

The partial pressures of the gases in a mixture are 0.255 atm 0, 3.24 atm Ny,

katovenus [111]

<h3>Answer:</h3>

4.945 atm

<h3>Explanation:</h3>

Based on Dalton's law of Partial pressure, the total pressure of a mixture of gases is equivalent to the sum of individual partial pressures of the gases in the mixture.

That is;

$Pt = P1+P2+P3+P4+............+ Pn$

In this case;

Partial pressure of Oxygen, P(O) = 0.255 atm

Partial pressure of N, P(N) = 3.24 atm

Partial pressure of Ar, P(Ar) = 1.45 atm

Therefore;

P(total) = P(O) + P(N) + P(Ar)

= 0.255 atm + 3.24 atm + 1.45 atm

= 4.945 atm

Therefore, the total pressure of the mixture is 4.945 atm

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3 years ago

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The empirical formula for this would be FeS

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3 years ago

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The equation is x/25=3.2
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3 years ago