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3 years ago

6

Covalent bonds can be single, double, or triple.

1 answer:

DaniilM [7]3 years ago

3 0

Im pretty sure the answer would be 2. Bc that’s how many is shared between O2

You might be interested in

What is the volume of 8.45 grams of carbon dioxide at a pressure of 589 mmHg and a temperature of 10 c

frez [133]

This is a PV=nRT problem, commonly known as ideal gas. For this, we simply need to take what we know and plug it into the equation

Pressure x Volume = moles x ideal gas constant x tempature.

We know our pressure is 589mmHg so we can plug that in. The volume is unknown.

Then, we need to convert 8.45g of CO2 to moles. That is the grams to moles stoichiometry problem. I will not solve the problem for you, however I can set it up for you:

8.45gCO2 1 mole CO2
-------------- x --------------
1 44.01g CO2

At this point, we now have 589 x X= moles.
The ideal gas constant for mmHg should have been given to you, it is 62.4.

Then, we need to convert from celcius to kelvin. To do this, we simply add 273 to 10, since 273 is the standard unit for kelvin.

Now that we have all of our units, we can plug them into the PV=nRT formula, and solve. We are finding the V, so therefore to find it, the P (pressure) needs to equal the nRT. We would multiple nRT together to get an answer, and divide by the pressure to get the missing unit. To make sure you got the right answer, multiply P and V together to see if it equals nRT. And don't forget to round to the least number of sig figs! Hope I could be of help!

8 0

4 years ago

If water (p=998 kg/m3, u = 10-3 Pa.s) flows through a 50 m Pa.s) determine the velocity of carbon tetrac me the velocity of carb

babymother [125]

Explanation:

As it is given that both have same dynamic characteristics.

Therefore, $Re_{water}$ = $Re_{CCl_{4}}$

$\frac{\rho_{water} \times \nu_{water} \times D_{water}}{\mu_{water}}$ = $\frac{\rho_{CCl_{4}} \times \nu_{CCl_{4}} \times D_{CCl_{4}}}{\mu_{CCl_{4}}}$

Hence, putting the given values into the above formula as follows.

$\frac{998 kg/m^{3} \times 2 m/s \times 50 mm}{10^{-3}Pa.s}$ = $\frac{1590 kg/m^{3}} \times \nu_{CCl_{4}} \times 60 mm}{0.958 \times 10^{-3}}$

$\nu_{CCl_{4}}$ = 1.002 m/s

Thus, we can conclude that the velocity of carbon tetrachloride in the given conditions is 1.002 m/s.

4 0

3 years ago

Draw the product you expect from the reaction of (s)-3-iodohexane with ch3co2-. be sure to show stereochemistry.

Rasek [7]

This will give substituted product which will be by SN2 mechanism

so here we will get product with inverted geometry

In SN2 mechanism the nucleophile attacks from back side and we always get product with inverted geometry

This is known as Walden inversion.

8 0

3 years ago

Alum used in cooking is potassium aluminum sulfate hydrate, KAl(SO4)2. XH2O. To find the value of X, you can heat the sample of

kolbaska11 [484]

Answer:

The answer is given below in the picture

Explanation:please check it

6 0

4 years ago

In a particular experiment, 2.50-g samples of each reagent are reacted. The theoretical yield of lithium nitride is ________ g.

Neporo4naja [7]

Answer:

4.18 g

Explanation:

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Given: For Li

Given mass = 2.50 g

Molar mass of Li = 6.94 g/mol

<u>Moles of Li = 2.50 g / 6.94 g/mol = 0.3602 moles</u>

Given: For $N_2$

Given mass = 2.50 g

Molar mass of $N_2$ = 28.02 g/mol

<u>Moles of $N_2$ = 2.50 g / 28.02 g/mol = 0.08924 moles</u>

According to the given reaction:

$6Li+N_2\rightarrow 2Li_3N$

6 moles of Li react with 1 mole of $N_2$

1 mole of Li react with 1/6 mole of $N_2$

0.3602 mole of Li react with $\frac {1}{6}\times 0.3602$ mole of $N_2$

Moles of $N_2$ that will react = 0.06 moles

Available moles of $N_2$ = 0.08924 moles

$N_2$ is in large excess. (0.08924 > 0.06)

Limiting reagent is the one which is present in small amount. Thus,

Li is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

6 moles of Li gives 2 mole of $Li_3N$

1 mole of Li gives 2/6 mole of $Li_3N$

0.3602 mole of Li react with $\frac {2}{6}\times 0.3602$ mole of $Li_3N$

Moles of $Li_3N$ = 0.12

Molar mass of $Li_3N$ = 34.83 g/mol

Mass of $Li_3N$ = Moles × Molar mass = 0.12 × 34.83 g = 4.18 g

<u>Theoretical yield = 4.18 g</u>

5 0

3 years ago