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3 years ago

Maintaining constant pressure, the volume of a gas is increased from 12,0 L

Chemistry

1 answer:

kow [346]3 years ago

3 0

Answer:

790 K

Explanation:

Step 1: Given data

Initial volume of the gas (V₁): 12.0 L

Initial temperature of the gas (T₁): 23.0 °C

Final volume of the gas (V₂): 32.0 L

Step 2: Convert 23.0 °C to Kelvin

We will use the following expression.

K = °C + 273.15 = 23.0 + 273.15 = 296.2 K

Step 3: Calculate the final temperature of the gas

Assuming constant pressure and ideal behavior, we can calculate the final temperature of the gas using Charles' law.

T₁/V₁ = T₂/V₂

T₂ = T₁ × V₂/V₁

T₂ = 296.2 K × 32.0 L/12.0 L = 790 K

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3. What is the atomic mass of phosphorous if phosphorous-29 has a percent abundance of 35.5%, phosphorous-30 has a percent abund

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The atomic mass of phosphorus is 29.864 amu.

Explanation:

Given data:

Atomic mass of phosphorus = ?

Percent abundance of P-29 = 35.5%

percent abundance of P-30 = 42.6%

Percent abundance of P-31 = 21.9%

Solution:

Average atomic mass = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) + (abundance of 3rd isotope × its atomic mass / 100

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The atomic mass of phosphorus is 29.864 amu.

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2. A solvent used in cleaning is found to contain only the elements carbon, hydrogen, and chlorine. When a

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mass of C = 0.238 g

mass of H =0.00989 g

mass of Cl = 1.05 g

Explanation:

Determine the masses of carbon, hydrogen, and chlorine in the original sample of the solvent.

First we need to calculate the molar mass of carbon dioxide (CO₂) and water (H₂O)

molar mass of CO₂ = molar mass of C × 1 + molar mass of O × 2

molar mass of CO₂ = 12 × 1 + 16 × 2 = 44 g/mole

molar mass of H₂O = molar mass of H × 2 + molar mass of O × 1

molar mass of H₂O = 1 × 2 + 16 × 1 = 18 g/mole

Now, to find the mass of carbon and hydrogen in the original sample of solvent, we devise the following reasoning:

if 44 g of CO₂ contains 12 g of C

then 0.872 g of CO₂ contains X g of C

X = (0.872 × 12) / 44 = 0.238 g of C

if 18 g of H₂O contains 2 g of H

then 0.089 g of H₂O contains Y g of H

Y = (0.089 × 2) / 18 = 0.00989 g of H

And now, we can find the mass of chlorine:

mass of sample = mass of C + mass of H + mass of Cl

mass of Cl = mass of sample - mass of C - mass of H

mass of Cl = 1.30 - 0.238 - 0.00989

mass of Cl = 1.05 g

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