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2 years ago

Compare how entropy changes for the following two systems

Chemistry

1 answer:

bazaltina [42]2 years ago

3 0

Remember the fact

Randomness follows the order

Gas>Liquid>Solid

#System A

As solid particles are dissolved in water their randomness increases so entropy increases

#System B

Gas is converted to liquid so entropy decreases as randomness decreases

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Use the combined gas law to calculate the "corrected" volume of hydrogen at STP

solong [7]

Answer:

We will derive the combined gas equation from the law of Gases

Boyle's law

P∝1/V

PV=Constant

Charles law

V∝T

Avogadro's Law

V∝n

By combining these three equations we get the combined gas equation

PV=nRT

V=nRT/P

If n=1 mole

V=RT/P

By putting the value of R, T, and P in the above equation we can calculate the volume of the gas at STP.

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4 years ago

When using the process of evaporation to separate a mixture, what is left behind

brilliants [131]

Answer:

When a solution is heated, the solvent evaporates, leaving behind the dissolved solids as residue. When a solution containing dissolved solutes is heated, the solvent will evaporate. Only the solute will remain in the evaporating dish.

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3 years ago

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3 years ago

Read 2 more answers

How many grams of CO2 are produced from 6.7 L of O2 gas at STP?

Tasya [4]

<h3>Answer:</h3>

13 g CO₂

<h3>General Formulas and Concepts:</h3>

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table
Moles
STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

<u>Stoichiometry</u>

Using Dimensional Analysis

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<h3>Explanation:</h3>

<u>Step 1: Define</u>

<em>Identify variables</em>

[Given] 6.7 L O₂

[Solve] g O₂

<u>Step 2: Identify Conversions</u>

[STP] 22.4 L = 1 mol

[PT] Molar Mass of O: 16.00 g/mol

[PT] Molar Mass of C: 12.01 g/mol

Molar Mass of CO₂: 12.01 + 2(16.00) = 44.01 g/mol

<u>Step 3: Convert</u>

[DA] Set up: $\displaystyle 6.7 \ L \ O_2(\frac{1 \ mol \ O_2}{22.4 \ L \ O_2})(\frac{44.01 \ g \ O_2}{1 \ mol \ O_2})$
[DA] Divide/Multiply [Cancel out units]: $\displaystyle 13.1637 \ g \ O_2$