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3 years ago

Help please!!!!!!!!!

Chemistry

1 answer:

Hatshy [7]3 years ago

3 0

Answer:

D. Element

Explanation:

Fe is an element. It isn't more than one element chemically combined (compound), it isn't a charged particle (ion), and it isn't the smallest possible unit of multiple atoms combined together (molecule).

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What is the formula of acceleration?

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Answer:

The formula of acceleration is final velocity-initial velocity÷time taken

Explanation:

v-u/t

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3 years ago

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A sample of an unknown compound is vaporized at 150.°C . The gas produced has a volume of 960.mL at a pressure of 1.00atm , and

IrinaK [193]

Answer:

34.02 g.

Explanation:

Hello!

In this case, since the gas behaves ideally, we can use the following equation to compute the moles at the specified conditions:

$PV=nRT\\\\n=\frac{1.00atm*0.960L}{0.08206\frac{atm*L}{mol*K}*(150+273)K} =0.0277mol\\\\$

Now, since the molar mass of a compound is computed by dividing the mass over mass, we obtain the following molar mass:

$MM=\frac{0.941g}{0.0277mol} \\\\MM=34.02g/mol$

So probably, the gas may be H₂S.

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3 years ago

The Moon is smaller than Earth. Why does the Moon have less gravity than Earth?

ipn [44]

C is the answer the moon has less mass than earth

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3 years ago

The ion MnOis often used to analyze for the Fe2+ content of an aqueous solution by using the (unbalanced) reaction Mno+Fe2+ + Fe

dusya [7]

Answer:

B) 0.230 M

Explanation:

The first step is to <u>balance the reaction</u> between the Ferrous ion and the permanganate ion:

$5~Fe^+^2~+~MnO_4^-^1~+~8H^+~->~5Fe^+^3~+~Mn^+^2~+4H_2O$

Then we have to <u>calculate the moles</u> of $MnO_4^-$ :

$M~=~\frac{mol}{L}$

$mol~=~M*L$

$mol~=~0.033~M*0.0633L=~0.002088~mol~MnO_4^-$

Then using the <u>molar ratio</u> we can find the moles of $Fe^+^2$ :

$0.002088~mol~MnO_4^-\frac{5~mol~Fe^+^2}{1~mol~MnO_4^-}=0.01044~mol~Fe^+^2$

Finally we can calculate the molarity:

$M=\frac{0.01044~mol~Fe^+^2}{0.0455~L}=0.230~M$

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3 years ago

How many moles in 4.93 x 10E23 atoms of silver?

leva [86]

<h3>Answer:</h3>

0.819 mol Ag

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

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

4.93 × 10²³ atoms Ag

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

Avogadro's Number

<u>Step 3: Convert</u>

Set up: $\displaystyle 4.93 \cdot 10^{23} \ atoms \ Ag(\frac{1 \ mol \ Ag}{6.022 \cdot 10^{23} \ atoms \ Ag})$
Divide: $\displaystyle 0.818665 \ mol \ Ag$

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

0.818665 mol Ag ≈ 0.819 mol Ag

8 0

3 years ago