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3 years ago

Consider the equation below. N2 + 3H2 -> 2NH3 What is the mole ratio of hydrogen to ammonia?

Chemistry

2 answers:

kumpel [21]3 years ago

7 0

Answer:

3:2

Explanation:

Crank3 years ago

4 0

The answer is: C. 3 : 2.

Balanced chemical reaction: 3H₂ + N₂ → 2NH₃.

From chemical reaction: n(H₂) : n(NH₃) = 3 : 2.

Coefficients with the lowest ratio indicate the relative amounts of substances in a reaction.

Coefficient in fron of hydrogen is 3 and coefficient in fron ammonia is 2.

Coefficients are important to prove the law of conservation of mass.

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When 3.24 g of a nonelectrolyte solute is dissolved in water to make 955 mL of solution at 22 °C, the solution exerts an osmotic

attashe74 [19]

Answer:

The molar concentration is 0.0529 M

We have 0.0505 moles solute

The molar mass of the solute is 64.16 g/mol

Explanation:

Step 1: Data given

Mass of the nonelectrolyte solute = 3.24 grams

Volume of water = 955 mL

Temperature = 22 °C = 295 K

Osmotic pressure = 973 torr = 973 / 760 = 1.28026 atm

Step 2: Calculate mass water

Mass water = 955 mL * 1g/mL

Mass water = 955 grams = 0.955 kg

Step 3: Calculate the molar concentration

π = i*M*R*T

⇒with π = the osmotic pressure = 1.28026 atm

⇒with i = the van't Hoff factor = 1

⇒with M = the molar concentration

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 295 K

M = 1.28026 / (0.08206*295)

M = 0.0529 M

Step 4: Calculate moles solute

Molar concentration = moles / volume

Moles solute = Molar concentration * volume

Moles solute = 0.0529 M * 0.955 L

Moles solute = 0.0505 moles

Step 5: Calculate molar mass

Molar mass = mass / moles

Molar mass = 3.24 grams / 0.0505 moles

Molar mass = 64.16 g/mol

The molar concentration is 0.0529 M

We have 0.0505 moles solute

The molar mass of the solute is 64.16 g/mol

4 0

3 years ago

You are on a field trip to a nearby lake for biology class and want to perform a quick analysis of the water’s approximate pH le

vitfil [10]

The easiest way to approximate ph level is through the ph paper measurement system because using pH paper would be best for doing a quick measurement in the field. It does not essentially need to be calibrated or standardized and the papers make available an instant estimate.

8 0

3 years ago

What mass of HCl (in Kg) is required to create 8.80 Liters of hydrogen gas?

tiny-mole [99]

The important thing to notice here is that the reaction takes place at STP conditions, which are defined as a pressure of
100 kPa
and a temperature of
0
∘
C
.
Moreover, at STP one mole of any ideal gas occupies exactly
22.7 L
- this is known as the molar volume of a gas at STP.
Since all the gases are at the same conditions for pressure and temperature, the mole ratios become volume ratios.
To prove this, use the ideal gas law equation to write the number of moles of hydrogen gas and of chlorine gas as
P
V
=
n
R
T
⇒
n
=
P
V
R
T
For hydrogen, you would have
n
hydrogen
=
P
⋅
V
hydrogen
R
T
and for chlorine you have
n
chlorine
=
P
⋅
V
chlorine
R
T
Thus, the mole ratio between hydrogen and chlorine will be
n
hydrogen
n
chlorine
=
P
V
hydronge
R
T
⋅
R
T
P
⋅
V
chlorine
=
V
hydrogen
V
chlorine
The same principle applies to the mole ratio that exists between hydrogen and hydrogen chloride.
So, the balanced chemical equation for this reaction is
H
2(g]
+
Cl
2(g]
→
2
HCl
(g]
Notice that you have a
1
:
2
mole ratio between hydrogen gas and hydrogen chloride.
This means that the reaction will produce twice as many moles as you the number of moles of hydrogen gas that reacts.
Use the volume ratio to find what volume of hydrogen chloride will be produced by the reaction
4.9
L H
2
⋅
2
L HCl
1
L H
2
=
9.8 L HCl
Now use the molar volume to find how many moles you'd get in this volume of gas at STP
9.8
L HCl
⋅
1 mole HCl
22.7
L HCl
=
0.4317 moles HCl
Finally, use hydrogen chloride's molar mass to find how many grams would contain this many moles
0.4317
moles HCl
⋅
36.461 g
1
mole HCl
=
15.74 g
Rounded to two sig figs, the answer will be
m
HCl
=
16 g

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3 years ago

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klemol [59]

the answer is Nitrogen.

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vlada-n [284]

I think it is the bottom left :)

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3 years ago