Is this how you would draw Lewis structure for NO2?

In Part B, we determined the water hardness of a water sample by combining the water sample with a 10.00 mL sample of calcium ch

Verizon [17]

Answer:

The definition is defined throughout the clarification section beneath, and according to the particular circumstance.

Explanation:

Although water samples were supplemented with purified water, the amount of EDTA has would be smaller.
Since there are fewer ions throughout purified water, most of the ions are eliminated throughout distillation, less utilized EDTA.
Complex calcium formation including EDTA will be less complex. Samples used throughout the starting include several Ca⁺², Mg²⁺ ions that have not been found in pure water, causing fewer EDTA volume to enter the final stages.

8 0

3 years ago

acetylene gas c2h2 undergoes combustion to produce carbon dioxide and water vapor How many grams of water are produced by the sa

ella [17]

<u>Answer:</u> The amount of water produced in the given reaction is $0.692x$ grams.

<u>Explanation:</u>

Let us assume that the initial amount of acetylene gas given be 'x' grams. Now, to calculate the number of moles, we will use the formula:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

Given mass of acetylene = x grams

Molar mass of acetylene = 26 g/mol

Putting values in above equation, we get:

$\text{Number of moles of acetylene}=\frac{xg}{26g/mol}=\frac{x}{26}mol$

The reaction of combustion of acetylene is given by the equation:

$2C_2H_2+5O_2\rightarrow 4CO_2+2H_2O$

By Stoichiometry of the reaction:

2 moles of acetylene produces 2 moles of water.

So, $\frac{x}{26}$ moles of acetylene will produce = $\frac{2}{2}\times \frac{x}{26}=\frac{x}{26}$ moles of water.

Now, to calculate the amount of water produced, we use equation 1:

Molar mass of water = 18 g/mol

Moles of water = $\frac{x}{26}mol$

Putting values in equation 1, we get:

$\frac{x}{26}mol=\frac{\text{Mass of water}}{18g/mol}$

$\text{Mass of water}=\frac{x}{26}\times 18=0.692x$ grams

8 0

3 years ago

What is the correct formula that would result from the combination of the two ionic species?

DerKrebs [107]

Answer:

2K+ + NO-2 -> K2NO

Explanation:

Message me for extra explanation.

snap- parkguy786

5 0

3 years ago

How many moles of gas would you have if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature

seraphim [82]

Answer: There are 3.2 moles of gas if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature.

Explanation:

Given: Volume = 38.0 L

Pressure = 1430 mm Hg (1 mm Hg = 0.00131579 atm) = 1.9 atm

Temperature = 273.15 K

Using ideal gas equation, the moles of gas will be calculated as follows.

$PV = nRT\\$

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T =temperature

Substitute the values into above formula as follows.

$PV = nRT\\1.9 atm \times 38.0 L = n \times 0.0821 L atm/mol K \times 273.15 K\\n = \frac{1.9 atm \times 38.0 L}{0.0821 L atm/mol K \times 273.15 K}\\= 3.2 mol$

Thus, we can conclude that there are 3.2 moles of gas if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature.

5 0

3 years ago

What volume of 15.7 M H2SO4 is required to prepare 12.0 L of 0.156 M sulfuric acid?

kirza4 [7]

The volume of 15.7 M H2SO4 is required to prepare 12.0 L of 0.156 M sulfuric acid is 0.12 L

<h3>Data obtained from the question</h3>

From the question given above, the following data were obtained:

Molarity of stock solution (M₁) = 15.7 M
Volume of diluted solution (V₂) = 12 L
Molarity of diluted solution (M₂) = 0.156 M
Volume of stock solution needed (V₁) = ?

<h3>How to determine the volume of the stock solution needed</h3>

The volume of the stock solution needed can be obtained by using the dilution formula as shown below:

M₁V₁ = M₂V₂

15.7 × V₁ = 0.156 × 12

15.7 × V₁ = 1.872

Divide both side by 15.7

V₁ = 1.872 / 15.7

V₁ = 0.12 L

Thus, the volume of the stock solution needed to prepare the solution is 0.12 L

Learn more about dilution:

brainly.com/question/15022582

#SPJ1

4 0

1 year ago