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Dafna1 [17]
3 years ago
15

The number of moles in 250 L of He gas at STP is ________ mol, Round to a whole number,

Chemistry
1 answer:
7nadin3 [17]3 years ago
7 0

Answer: The number of moles in 250.0 L of He at STP is 11.0 mole.

Explanation:

  • It is known that 1.0 mole of a gas at STP conditions will occupy 22.7 L.
  • To show this information: STP means that T = 0.0 °C = 273.15 K and P = 1.0 kPa =  (100/101.325) = 0.9869 atm.
  • From the ideal gas law: PV = nRT.
  • Where, P is the pressure in atm <em>(P = 1.0 atm at STP).</em>
  • V is the volume in L.
  • n is the number of moles (n = 1.0 mole).
  • R is the general gas constant (R = 0.0821 L.atm/mol.K).
  • T is the temperature in K (T = 273.15 K at STP).
  • and now we can get the volume of 1.0 mole at STP: V = nRT/P
  • V = (1.0 mole x 0.0821 L.atm/mol.K x 273.15 K) / (0.9869 atm) = 22.7 L.
  • Now, we can get the number of moles of 250.0 L of He at STP:

<em>Using cross multiplication:</em>

1.0 mole → 22.7 L

??? mole → 250.0 L

  • The number of moles in 250.0 L of He at STP = (250.0 L x 1.0 mole) / (22.7 L) = 11.01 mole ≅ 11.0 mole.
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Fantom [35]

Answer:

Diatomic molecules consist of two atoms that are chemically bonded. The two atoms can be the same or different chemical elements. As for whether or not they are compounds, there is not technically an answer. This is because all compounds are molecules, but not all molecules are compounds. For example diatomic molecules that comprise the chemical compounds nitric acid, carbon monoxide, and hydrogen chloride are made up of two different elements.  As you can see, most diatomic molecules are not made up of the same kind of elements and not every diatomic molecule comprises a chemical compound.

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Explanation:

4 0
2 years ago
Determine the final temperature of sample with a specific heat of 1.1 J/g°C and a mass of 385 g if it starts out at a temperatur
Assoli18 [71]

Answer:

T2 =21.52°C

Explanation:

Given data:

Specific heat capacity of sample = 1.1 J/g.°C

Mass of sample = 385 g

Initial temperature = 19.5°C

Heat absorbed = 885 J

Solution:

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = Final temperature - initial temperature

885J = 385 g× 1.1 J/g.°C×(T2 - 19.5°C )

885 J = 423.5 J/°C× (T2 - 19.5°C )

885 J / 423.5 J/°C = (T2 - 19.5°C )

2.02°C = (T2 - 19.5°C )

T2 = 2.02°C + 19.5°C

T2 =21.52°C

8 0
3 years ago
The amount of a chemical solution is measured to be 2 liters.
irinina [24]
2 liters may be 1.5 to 1.9 rounded up to 2 or 2.1 or 2.4 rounded down to 2.

2 - 1.5 = 0.5

percent error = (absolute error / quantity) * 100

percent error = 0.5/2 * 100% = 0.25 * 100% = 25%

Choice C. 25%.
3 0
2 years ago
How many moles of oxygen are needed to react with 87 grams of aluminum
labwork [276]

Answer:

2.4 moles of oxygen are needed to react with 87 g of aluminium.

Explanation:

Chemical equation:

4Al(s)  + 3O₂(l)   → 2AlO₃(s)

Given data:

Mass of aluminium = 87 g

Moles of oxygen needed = ?

Solution:

Moles of aluminium:

Number of moles of aluminium= Mass/ molar mass

Number of moles of aluminium= 87 g/ 27 g/mol

Number of moles of aluminium= 3.2 mol

Now we will compare the moles of aluminium with oxygen.

                              Al         :         O₂

                               4          :         3

                               3.2       :         3/4×3.2 = 2.4 mol

2.4 moles of oxygen are needed to react with 87 g of aluminium.

5 0
2 years ago
A gas sample has a temperature of 22c with an unknown volume. The same gas has a volume of 456 mL when the temperature is 86c wi
Mkey [24]

The initial volume is 116.65 mL

<u>Explanation:</u>

<u />

Given:

Temperature, T₁ = 22°C

T₂ = 86°C

Volume, V₂ = 456 m

V₁ = ?

According to Charle's law:

\frac{V_1}{T_1} = \frac{V_2}{T_2}

Substituting the values:

\frac{V_1}{22} =\frac{456}{86} \\\\V_1 = \frac{456 X 22}{86} \\\\V_1 = 116.65 mL

Therefore, the initial volume is 116.65 mL

3 0
3 years ago
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