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Liono4ka [1.6K]
3 years ago
5

What is the temperature of 0.500 moles of a gas that is stored in a 2.50 L container under 13.0 atm of pressure?

Chemistry
1 answer:
faust18 [17]3 years ago
3 0
<h2>Answer:</h2>

Moles of a gas = 0.500

Volume = 2.50 L

Pressure = 13. atm

Temperature = ?

Solution:

Formula:

                       PV = n RT

Putting the values in formula:

 T = PV/nR = 13 * 2.5 / 0.5 *  0.082057

   =  32.5/0.041 = 792.68 K

                    T = 792.68 K

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Data Table 3: Polystyrene Test Tube, 12x75mm
Lera25 [3.4K]

Answer:

Experiment 8 E Data Table 3 fl Data Table 4 fl Data Table 5 fl Data Table 6 Data Table 3: Polystyrene Test Tube, 12x75mm Volume of water at room temperature (V1 in mL) Volume of gas in polystyrene tube at boil (V2 in mL) Temperature of gas at boil inside polystyrene tube (°C) Volume of gas in polystyrenetube at room temperature (V3 in mL) Temperature of gas.

Explanation:

Hope this helps

Mark as Brainliest please

4 0
3 years ago
34 atoms of carbon (C) react with 22 molecules of hydrogen gas (H2). How many molecules of methane (CH4) will be formed, and wha
kolbaska11 [484]

Answer:

11 molecules of CH4.

23 atoms of C is the leftover.

Explanation:

Hello!

In this case, for the formation of methane:

C+2H_2\rightarrow CH_4

We can see there is an excess of carbon based on their stoichiometry, because the needed amount of hydrogen gas molecules would be:

molecules _{H_2}=34atomC*\frac{2molec\ H_2}{1atomC} =68molec\ H_2

Thus, the formed molecules of methane are computed below:

molec\ CH_4=22molec\ H_2 *\frac{1molec\ CH_4}{2molmolec\ H_2} \\\\molec\ CH_4=11molec\ CH_4

In such a way, the leftover of carbon atoms are:

atoms \ C^{left over}=34-22molec\ H_2*\frac{1atoms C}{2molec\ H_2} \\\\atoms \ C^{left over}=23 atoms C

Best regards!

4 0
3 years ago
Covalent bonding (with an electronegativity difference below 0.5) results when fluorine bonds with
Hitman42 [59]

Answer:

flourine

Explanation:

7 0
3 years ago
Is wind energy consistent or inconsistent
LuckyWell [14K]
Inconsistent as it can vary from time to time.
5 0
3 years ago
A 475 cm3 sample of gas at standard temperature and pressure is allowed to expand until it occupies a
Andrej [43]

The final temperature : 345 K

<h3> Further explanation </h3>

Given

475 cm³ initial volume

600 cm³ final volume

Required

The final temperature

Solution

At standard temperature and pressure , T = 273 K and 1 atm

Charles's Law  :

When the gas pressure is kept constant, the gas volume is proportional to the temperature  

V₁/T₁=V₂/T₂

Input the value :

T₂=(V₂T₁)/V₁

T₂=(600 x 273)/475

T₂=345 K

4 0
3 years ago
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