Can anyone help me do this crossword puzzle?

NemiM [27]

102 grams of ammonia is formed when 3 moles of nitrogen and 6.7 moles of hydrogen reacts.

Explanation:

The equation given is of Haeber's process in which the nitrogen is limiting factor in the ammonia formation and hydrogen if in excess gets delimited.

We know that 1 mole of Nitrogen gives 2 moles of ammonia.

We have 3 moles of nitrogen here,

So, 6 moles of ammonia will be form

so from the formula

no of moles=mass/atomic mass

mass= no. of moles*atomic mass

= 6*17

= 102 grams of ammonia will be formed.

So, 6 moles or 102 grams of ammonia is formed when 3 mole of nitrogen and 6.7 mole of hydrogen reacts.

7 0

3 years ago

What Is scientific theory

sveticcg [70]

Answer:

is an explanation of an aspect of the natural world that can be repeatedly tested and verified in accordance with the scientific method, using accepted protocols of observation, measurement, and evaluation of results

8 0

3 years ago

Why are the atoms of the group 8 elements unreactive??

anygoal [31]

Answer:

because that is the last group the ones before it are more reactive im sorry if this not what you were looking for.

3 0

3 years ago

When a 3.00 grams sample of a compound containing only c, h, and o was completely burned, 1.17 grams of h2o and 2.87 grams of co

SVEN [57.7K]

Answer:- $CH_2O_2$

Solution:- From given masses of carbon dioxide and water we could calculate the moles that helps to calculate the moles of C and H.

Molar mass of carbon dioxide = 44 gram per mol

molar mass of water = 18.02 gram per mol

From given info, combustion of compound gives 1.17 grams of water and 2.87 grams of carbon dioxide. Let's calculate the moles of these:

$1.17gH_2O(\frac{1mol}{18.02g})$

= $0.0649molH_2O$

Similarly, $2.87gCO_2(\frac{1mol}{44g})$

= $0.0652molCO_2$

One mol of water has two moles of H. So, the moles of H would be two times the moles of water as calculated above.

So, moles of H = 2* 0.0649 = 0.1298 mol

One mol of carbon dioxide contains one mol of C. So, the moles of C would be equal to the moles of carbon dioxide calculated above.

moles of C = 0.0652 mol

Let's convert the moles of H and C to grams so that we could calculate the amount of oxygen present in the sample as:

grams of H in sample = 1.008 x 0.1298 = 0.1308 g

grams of C in sample = 12*0.0652 = 0.7824 g

If we subtract the sum of the masses of C and H from sample mass then it would give as the mass of oxygen since the sample has only C, H and O.

mass of O in sample = 3.00g - (0.1308 g + 0.7824 g)

= 3.00 g - 0.9132 g

= 2.0868 g

Let's convert these grams of oxygen to moles on dividing by it's atomic mass as:

$2.0868gO(\frac{1mol}{15.999g})$

= 0.130 mol O

Now, we have the moles of all the three atoms and we know that an empirical formula is the simplest whole number ratio of the moles of atoms. So, let's calculate the ratio. For this, we divide the moles of each by the least one of them.Looking at the moles, the least value is for carbon. So, let's divide the moles of each by the moles of C as:

C = $\frac{0.0652}{0.0652}$ = 1

H = $\frac{0.1298}{0.0652}$ = 2

O = $\frac{0.130}{0.0652}$ = 2

The ratio of C, H and O is 1:2:2. So, the simplest formula of the compound is $CH_2O_2$ .

3 0

3 years ago

Using the combined gas law, if the volume of a gas at 155kPa changes from 22L to 10L. What is the new pressure if the temperatur

Deffense [45]

Answer:

The answer to your question is P2 = 342 kPa

Explanation:

Data

Pressure 1 = P1 = 155 kPa

Volume 1 = V1 = 22 l

Pressure 2 = P2 = ?

Volume 2 = V2 = 10 l

Temperature = constant

Process

1.- Write the equation of the combined gas law

P1V1/T1 = P2V2/ T2

Cancel T1 and T2 because they measure the same

P1V1 = P2V2

-Solve for P2

P2 = P1V1/V2

2.- Substitution

P2 = (155 x 22) / 10

3.- Simplification

P2 = 3410 / 10

4.- Result

P2 = 342 kPa

5 0

3 years ago