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How many grams are in 4.5 x 10^22 molecules of Ba(NO2)2

NNADVOKAT [17]

Answer:

17 g Ba(NO₂)₂

General Formulas and Concepts:

Chemistry

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

Explanation:

Step 1: Define

4.5 × 10²² molecules Ba(NO₂)₂

Step 2: Define conversion

Molar Mass of Ba - 137.33 g/mol

Molar Mass of N - 14.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of Ba(NO₂)₂ - 137.33 + 2(14.01) + 4(16.00) = 229.35 g/mol

Step 3: Dimensional Analysis

$4.5 \cdot 10^{22} \ mc \ Ba(NO_2)_2(\frac{1 \ mol \ Ba(NO_2)_2}{6.022 \cdot 10^{23} \ mc \ Ba(NO_2)_2} )(\frac{229.35 \ g \ Ba(NO_2)_2}{1 \ mol \ Ba(NO_2)_2} )$

= 17.1384 g Ba(NO₂)₂

Step 4: Check

We are given 2 sig figs. Follow sig fig rules.

17.1384 g Ba(NO₂)₂ ≈ 17 g Ba(NO₂)₂

7 0

3 years ago

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Lostsunrise [7]

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4 0

4 years ago

Which material has a greater density, lead or feathers?

algol13

Lead has a higher density

5 0

3 years ago

Write the net ionic equation for any precipitation reaction that may be predicted when aqueous solutions of calcium iodide and c

Hitman42 [59]

Answer: The net ionic equation is written below.

Explanation:

Net ionic equation of any reaction does not include any spectator ions.

Spectator ions are defined as the ions which does not get involved in a chemical equation. They are found on both the sides of the chemical reaction when it is present in ionic form.

The chemical equation for the reaction of calcium iodide and chromium (III) sulfate is given as:

$3CaI_2(aq.)+Cr_2(SO_4)_3(aq.)\rightarrow 3CaSO_4(s)+2CrI_3(aq.)$

Ionic form of the above equation follows:

$3Ca^{2+}(aq.)+6I^{-}(aq.)+2Cr^{3+}(aq.)+3SO_4^{2-}(aq.)\rightarrow 3CaSO_4(s)+2Cr^{3+}(aq.)+6I^-(aq.)$

As, chromium and iodide ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

$3Ca^{2+}(aq.)+3SO_4^{2-}(aq.)\rightarrow 3CaSO_4(s)$

Hence, the net ionic equation is written above.

8 0

3 years ago

If you evaporated 125 mL of a 3.5 M solution of iron(II) nitrite, how many moles of iron(II) nitrite would you recover?

Verizon [17]

Considering the definition of molarity, 0.4375 moles of iron(II) nitrite you would recover.

In order to find the moles of the solid that can be recovered from this solution, you need to use the definition of molarity.

<h3>Definition of molarity</h3>

Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.

The molarity of a solution is calculated by dividing the moles of solute by the volume of the solution:

$Molarity=\frac{number of moles}{volume}$