All categories

3 years ago

Balance the equation first.

Chemistry

1 answer:

topjm [15]3 years ago

7 0

Answer:

Therefore, 12 moles of hydrogen makes 8 moles of ammonia.

Using the proportions of the amount of the molecules, we can convert from any reagent or product to any other reagent or product. In the context of this reaction, for every mole of N2 and every 3 moles of H2 we obtain 2 moles of NH3.

Explanation:

;)’ hola

You might be interested in

Students investigate forces and how they affect objects. They use a small car and wooden blocks to carry out their investigation

Umnica [9.8K]

Answer:

increase the number of blocks

increase the number of students pulling the cart

increase the number of blocks and increase the number of students pulling the cart

decrease the number of blocks

decrease the number of students pulling the cart

decrease the number of blocks and decrease the number of students pulling the cart

(ANSWER CHOICES)

Explanation:

7 0

3 years ago

Brown bears live in thick forests. Recently, many forests have been cut down to build homes. What will happen to the bears that

nlexa [21]

They will not have a home and will die

3 0

4 years ago

Read 2 more answers

How do i draw the 3D orbital diagram for formyl chloride

Paha777 [63]

Answer:

jjjjjj*shhhhh is not good enough

Explanation:

jjjhjjjjjj

7 0

3 years ago

determine the empirical and molecular formula of a compound composed of 18.24 g carbon, 0.51 g hydrogen, and 16.91 g fluorine an

Vika [28.1K]

Answer: The empirical formula for the given compound is $C_3HF_2$ and molecular formula for the given compound is $C_{24}H_8F_{16}$

Explanation : Given,

Mass of C = 18.24 g

Mass of H = 0.51 g

Mass of F = 16.91 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{18.24g}{12g/mole}=1.52moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.51g}{1g/mole}=0.51moles$

Moles of Fluorine = $\frac{\text{Given mass of Fluorine}}{\text{Molar mass of Fluorine}}=\frac{16.91g}{19g/mole}=0.89moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.51 moles.

For Carbon = $\frac{1.52}{0.51}=2.98\approx 3$

For Hydrogen = $\frac{0.51}{0.51}=1$

For Fluorine = $\frac{0.89}{0.51}=1.74\approx 2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : F = 3 : 1 : 2

The empirical formula for the given compound is $C_3H_1F_2=C_3HF_2$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

We are given:

Molar mass = 562.0 g/mol

Mass of empirical formula = 3(12) + 1(1) + 2(19) = 75 g/eq

Putting values in above equation, we get:

$n=\frac{562.0}{75}=7.49\approx 8$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_3HF_2=(C_3HF_2)_n=(C_3HF_2)_8=C_{24}H_8F_{16}$

Thus, the molecular formula for the given compound is $C_{24}H_8F_{16}$

8 0

3 years ago

A storm that stays longer over coasts is a more dangerous storm. Is this statement true or false?

11Alexandr11 [23.1K]

Answer:

I think it is true, but I am not to sure.

5 0

3 years ago

Read 2 more answers