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Verdich [7]
1 year ago
14

When the temperature of a 3. 0-l sample of a gas is dropped from 200°c to 100°c, what will be the final volume of the gas sample

?.
Chemistry
1 answer:
ipn [44]1 year ago
4 0

P1V1T1=P2V2T2 Add 273 to convert degrees Celsius to Kelvin:

∴200×25/298=250×V2/273, ∴V2=200×25×273/298×250, ∴V2=18.32L

<h3>Where is the volume equation?</h3>

The basic formula for volume is length, breadth, and height, as opposed to length, width, and height for the area of a rectangular shape. The calculation is unaffected by how you refer to the various dimensions; for instance, you can use "depth" instead of "height."

<h3>What is chemistry using volume units?</h3>

Volume, which is measured in cubic units, is the 3-dimensional space occupied by matter or encircled by a surface. The cubic meter (m3), a derived unit, is the SI unit of volume.

to know more about volume and temperature here:

brainly.com/question/12050285

#SPJ4

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What happens when nitrogen and hydrogen comes in contact at high temperature and pressure in presence of iron powder and molybde
Sidana [21]

Answer:

<h2>Ammonia Gas</h2>

Explanation:

It result in formation of ammonia gas.

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It forms ammonia gas.

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3 years ago
12-How many elements are in the mixture pictured below?<br> A-7<br> O B-4<br> C-3<br> D-2
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4 0
3 years ago
Read 2 more answers
When methanol, CH 3 OH , is burned in the presence of oxygen gas, O 2 , a large amount of heat energy is released. For this reas
luda_lava [24]

<u>Answer:</u> The mass of methanol that must be burned is 24.34 grams

<u>Explanation:</u>

We are given:

Amount of heat produced = 581 kJ

For the given chemical equation:

CH_3OH(g)+\frac{3}{2}O_2(g)\rightarrow CO_2(g)+2H_2O(l);\Delta H=-764kJ

By Stoichiometry of the reaction:

When 764 kJ of heat is produced, the amount of methanol reacted is 1 mole

So, when 581 kJ of heat will be produced, the amount of methanol reacted will be = \frac{1}{764}\times 581=0.7605mol

To calculate mass for given number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of methanol = 0.7605 moles

Molar mass of methanol = 32 g/mol

Putting values in above equation, we get:

0.7605mol=\frac{\text{Mass of methanol}}{32g/mol}\\\\\text{Mass of methanol}=(0.7605mol\times 32g/mol)=24.34g

Hence, the mass of methanol that must be burned is 24.34 grams

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3 years ago
What is the oxidation number of S2O3
Liono4ka [1.6K]
I think S = 3. Not S=6
5 0
3 years ago
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