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2 years ago

Complete this example: A 0.67 molal solution was

Chemistry

1 answer:

Lynna [10]2 years ago

3 0

Answer:

A then C

Explanation:

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To obtain gasoline from crude oil.

11111nata11111 [884]

Answer:

pumped from ground, then carbon atoms linked together in chains of different lengths

Explanation:

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3 years ago

I need someone to help me with this. PLEASE, I'M BEGGING YOU

musickatia [10]

Answer:

D. 25%

Explanation:

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3 years ago

If a precipitation reaction occurs, what will be the products of the unbalanced

levacccp [35]

Answer:

${ \sf{B. \: AgCl _{(s)} + NaNO _{3(aq)}}}$

Explanation:

Silver chloride precipitates out because it has a low value of Ksp.

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3 years ago

Please please please please help

Pavel [41]

Answer:

Atomic #: 82

Mass #: 206

Charge: 4+

# of protons: 82

# of electrons: 78

# of neutrons: 124

Explanation:

Atomic #: look at the bottom left #, it's always the atomic #.

Mass #: look at the top left # it's always the mass #.

Charge: they give you the charge which is shown on the upper right of the element.

# of protons: is the atomic #

# of electrons: also the atomic # minus 4 bc the charge is a positive 4, indicating that some electrons 'left'.

# of neutrons: 206 (mass # is protons + neutrons) minus 82 (atomic#) which is 124.

6 0

3 years ago

What is the empirical formula? A compound is used to treat iron deficiency in people. It contains 36.76% iron, 21.11% sulfur, an

Mandarinka [93]

Answer: The empirical formula of the compound is $Fe_1S_1O_4$

Explanation:

Empirical formula is defined formula which is simplest integer ratio of number of atoms of different elements present in the compound.

Percentage of iron in a compound = 36.76 %

Percentage of sulfur in a compound = 21.11 %

Percentage of oxygen in a compound = 42.13 %

Consider in 100 g of the compound:

Mass of iron in 100 g of compound = 36.76 g

Mass of iron in 100 g of compound = 21.11 g

Mass of iron in 100 g of compound = 42.13 g

Now calculate the number of moles each element:

Moles of iron= $\frac{36.76 g}{55.84 g/mol}=0.658 mol$

Moles of sulfur= $\frac{21.11 g}{32.06 g/mol}=0.658 mol$

Moles of oxygen= $\frac{42.13 g}{16 g/mol}=2.633 mol$

Divide the moles of each element by the smallest number of moles to calculated the ratio of the elements to each other

For Iron element = $\frac{0.658 mol}{0.658 mol}=1$

For sulfur element = $\frac{0.658 mol}{0.658 mol}=1$

For oxygen element = $\frac{2.633 mol}{0.658 mol}=4.001\approx 4$

So, the empirical formula of the compound is $Fe_1S_1O_4$

4 0

3 years ago

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