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3 years ago

what temperature will 215 mL of a gas at 20°C and 1 atm pressure attain when it is subject to 1.5 atm of pressure?

Chemistry

1 answer:

romanna [79]3 years ago

8 0

Given:

Volume of gas = 215 ml

Initial temperature T1 = 20C = 20 +273 = 293 K

Initial pressure P1 = 1 atm

Final pressure P2 = 1.5 atm

To determine:

The final temperature T2

Explanation:

Based on Gay-Lussac's Law:

P α T

Therefore we have the relation:

P1/T1 = P2/T2

T2 = P2T1/P1 = 1.5 *293/1 = 439.5 K

Converting from Kelvin to degrees C we have:

T2 = 439.5 - 273 = 166.5 C

Ans: The final temperature is 439.5 K or 166.5 C

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3 years ago

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3 years ago

1. How many ATOMS of carbon are present in 7.48 grams of carbon monoxide ?

Salsk061 [2.6K]

Answer:

The answer is 1.61 × 10²³ atoms

Explanation:

To determine number of atoms, we will use the formula below

Number of atoms = number of moles (n) × avogadro's constant (6.02 x 10²³)

n was not provided, hence we will solve for n

n = mass/ molar mass

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3 0

3 years ago

an unknown molecule is found to consist of 24.2% carbon by mass, 4.0% hydrogen by mass and the remaining mass is due to chlorine

Paha777 [63]

Answer:

C3 H6 Cl 3

Explanation:

C -24.2%

H - 4.0%

Cl - (100-24.2 - 4.0)=73.8 %

We can take 100g of the substance, then we have

C -24.2 g

H - 4.0 g

Cl - 73.8 g

Find the moles of these elements

C -24.2 g/12.0 g/mol =2.0 mol

H - 4.0 g/1.0 g/mol = 4. 0 mol

Cl - 73.8 g/ 35.5 g/mol = 2.1 mol

Ratio of these elements gives simplest formula of the substance

C : H : Cl = 2 : 4 : 2 = 1 : 2 : 1

CH2Cl

Molar mass (CH2Cl) = 1*12.0 +2*1.0 + 1*35.5 = 49.5 g/mol

Real molar mass = 150 g/mol

real molar mass/ Molar mass (CH2Cl) = 150 /49.5=3

So, Real formula should be C3 H6 Cl 3.

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3 years ago

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matrenka [14]

Answer:

Yes.

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2 years ago