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3 years ago

What is the mass of 0.28 moles of iron

Chemistry

2 answers:

Xelga [282]3 years ago

4 0

1 mole has mass = 56 g

0.28 mol has mass = 56 x 0.28 = 15.68 g

Hope this helps!

Greeley [361]3 years ago

4 0

<h2>Answer:</h2>

Given data:

Number of moles of iron = 0.28 M

Mass of iron = ?

Solution:

Formula : Mass of iron = Number of moles of iron * Molecular mass of iron

Putting values in above formula:

Mass of iron = 0.28 * 55.84 = 15.63

Mass of iron = 15.63

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Which of the following is not a step in the conversion 1.3 Dam cubed to liters

lisabon 2012 [21]

A is the answer, and put the choices

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4 years ago

Show your calculation by uploading a picture. Calculate the molar mass of ammonia, NH3

Cloud [144]

Answer:

17.04 g/mol

Explanation:

Molar Mass of NH₃

we know that

Nitrogen has 14.01 gram/mol

And Hydrogen has 1.01 gram/mol

but we have 3 Hydrogens So we multiply

1.01 by 3 i.e., 3.03

Now, add

14.01

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17.04

So, The molar mass of ammonia, NH₃ is

17.04 g/mol

-TheUnknownScientist

5 0

3 years ago

A gaseous mixture composed of 20% CH4, 30% C2H4, 35% C2H2, and 15% C2H20. What is the average molecular weight of the mixture? a

Semenov [28]

Answer: The correct answer is Option d.

Explanation:

We are given:

Mass percentage of $CH_4$ = 20 %

So, mole fraction of $CH_4$ = 0.2

Mass percentage of $C_2H_4$ = 30 %

So, mole fraction of $C_2H_4$ = 0.3

Mass percentage of $C_2H_2$ = 35 %

So, mole fraction of $C_2H_2$ = 0.35

Mass percentage of $C_2H_2O$ = 15 %

So, mole fraction of $C_2H_2O$ = 0.15

We know that:

Molar mass of $CH_4$ = 16 g/mol

Molar mass of $C_2H_4$ = 28 g/mol

Molar mass of $C_2H_2$ = 26 g/mol

Molar mass of $C_2H_2O$ = 48 g/mol

To calculate the average molecular mass of the mixture, we use the equation:

$\text{Average molecular weight of mixture}=\frac{_{i=1}^n\sum{\chi_im_i}}{n_i}$

where,

$\chi_i$ = mole fractions of i-th species

$m_i$ = molar masses of i-th species

$n_i$ = number of observations

Putting values in above equation:

$\text{Average molecular weight}=\frac{(\chi_{CH_4}\times M_{CH_4})+(\chi_{C_2H_4}\times M_{C_2H_4})+(\chi_{C_2H_2}\times M_{C_2H_2})+(\chi_{C_2H_2O}\times M_{C_2H_2O})}{4}$

$\text{Average molecular weight of mixture}=\frac{(0.20\times 16)+(0.30\times 28)+(0.35\times 26)+(0.15\times 42)}{4}\\\\\text{Average molecular weight of mixture}=6.75$

Hence, the correct answer is Option d.

3 0

3 years ago

A flexible container at an initial volume of 6.13 L contains 2.51 mol of gas. More gas is then added to the container until it r

aleksley [76]

Answer:

2.12 moles of gas were added.

Explanation:

We can solve this problem by using Avogadro's law, which states that at constant temperature and pressure:

V₁n₂=V₂n₁

Where in this case:

V₁ = 6.13 L

n₂ = ?

V₂ = 11.3 L

n₁ = 2.51 mol

We input the data:

6.13 L * n₂ = 11.3 L * 2.51 mol

n₂ = 4.63

As 4.63 moles is the final number of moles, the number of moles added is:

4.63 - 2.51 = 2.12 moles

5 0

3 years ago

For each row in the table below, decide whether the pair of elements will form a molecular or ionic compound. If they will, then

Olin [163]

Answer:

$\begin{array}{cccll}\textbf{Element 1} & \textbf{ Element 2} &\textbf{Compound?} &\textbf{Formula} &\textbf{Type}\\\text{Ar}&\text{Xe} &\text{No} &\text{None}&\text{Neither}\\\text{F}& \text{Cs} &\text{Yes} &\text{CsF} &\text{Ionic}\\\text{N} &\text{Br} &\text{Yes} & \text{NBr}_{3}&\text{molecular} \\\end{array}$

Explanation:

You look at the type of atom and their electronegativity difference.

If ΔEN <1.6, covalent; if ΔEN >1.6, ionic

Ar/Xe: Noble gases; no reaction

F/Cs: Non-metal + metal; ΔEN = |3.98 – 0.79| = 3.19; Ionic

N/Br: Two nonmetals; ΔEN = |3.04 - 2.98| = 0.

4 0

3 years ago