How many moles are in 1.2 x 10 ^ 3 grams of ammonia

Answers

Answer 1

Answer: Molar mass ammonia:

NH₃ = 17.031 g/mol

$n = (m)/(M)$

$n = (1.2*10^3 g)/(17.031 g/mol)$

$n = 70.459$ moles

hope this helps!

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Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of the hydrogen that combines with 1.00g of each compound is 1.4 x 10^-1g, 2.4x10^-1 g and 2.40x10^-2 respectively. Show how these data illustrate the law of multiple proportions.

Answers

The law of multiple proportions, states that when two elements combine to form more than one compound, the mass of one element, which combines with a fixed mass of the other element, will always be ratios of whole numbers. You divide each by the smallest, and you should get the right kind of ratio. We do as follows:

H in N2H4 = 1.4x10^-1
1.4x10^-1 / 2.4x10^-2 = 6

H in NH3 = 2.4x10^-1
2.4x10^-1 / 2.4x10^-2 = 10

H in HN3 = 2.4x10^-2
2.4x10^-2 / 2.4x10^-2 = 1

Hello there.
Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of the hydrogen that combines with 1.00g of each compound is 1.4 x 10^-1g, 2.4x10^-1 g and 2.40x10^-2 respectively. Show how these data illustrate the law of multiple proportions.

H in HN3 = 2.4x10^-2
2.4x10^-2 / 2.4x10^-2 = 1

If 4.00 g of NaCl react with 10.00 g of AgNO3, what is the excess reactant?

Answers

Answer : The excess reagent is, $NaCl$

Explanation :

First we have to calculate the moles of $NaCl$ and $AgNO_3$ .

$\text{Moles of }NaCl=\frac{\text{Mass of }NaCl}{\text{Molar mass of }NaCl}=(4g)/(58.4g/mole)=0.068moles$

$\text{Moles of }AgNO_3=\frac{\text{Mass of }AgNO_3}{\text{Molar mass of }AgNO_3}=(10g)/(169.9g/mole)=0.058moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$NaCl+AgNO_3\rightarrow AgCl+NaNO_3$

From the balanced reaction we conclude that

As, 1 mole of $NaCl$ react with 1 mole of $AgNO_3$

So, 0.068 moles of $NaCl$ react with 0.068 moles of $AgNO_3$

From this we conclude that, the moles of $AgNO_3$ are less than the NaCl. So, $AgNO_3$ is a limiting reagent because it limits the formation of products and $NaCl$ is an excess reagent.

Hence, the excess reagent is, $NaCl$

The reaction formula of this is NaCl + AgNO3 = NaNO3 + AgCl. The mole number of NaCl is 4/58.5=0.068 mol. The mole number of AgNO3 is 10/170=0.059 mol. So the NaCl is excess.

NEED HELP AS SOON AS POSSIBLE!7. How many atoms are present in a 6.00 g sample of silver?
a. 1.07 x 10^-1 atoms
b. 6.47 x 10^2 atoms
c. 3.35 x 10^22 atoms
d. 3.61 x 10^24 atoms

8. How many atoms are present in 2.0 x 10^6 mol of carbon?
a. 3.3 x 10^-18 atoms
b. 4.0 x 10^-17 atoms
c. 1.0 x 10^29 atoms
d. 1.2 x 10^30 atoms

9. what mass is present in sample of AgNO3 containing 3.14 x 10^19 formula units?
a. 5.21 x 10^-5 g
b. 8.86 x 10^-3 g
c. 1.13 x 10^2 g
d. 1.92 x 10^4 g

10. How many molecules are present in 36.6 L of SO2 gas at STP?
a. 1.36 x 10^-21 molecules
b. 1.63 x 10^0 molecules
c. 1.54 x 10^22 molecules
d. 9.84 x 10^23 molecules

Answers

I got :
  7) C
  8) D
  9) B
10) D

The decimal difference in my calculations may be due to my rounding off or my use of the exact values in some cases.
Note: Mr - Molar Mass
L - Avogadro's Constant

Which subatomic particle(s) are found in the nucleus of the atom?. Enter the subatomic particle or particles separated by commas.

Answers

The subatomic particles found in the nucleus of the atom are:

Protons, Neutrons

The subatomic particles found inside the nucleons of the atoms are also referred to as the "nucleons". The nucleons are the protons, which are positively charged, and neutrons, which are neutral. The negatively charged subatomic particles, electrons, are found outside the nucleus.

Which of the following materials is not considered to be a semiconductor? germanium tin silicon aluminum

Answers

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Aluminium is not considered to be a semiconductor.

What type of reaction takes place when the melting of a solid occurs?

Answers

Thats a chemical reaction. I think

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