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Art [367]
3 years ago
14

Commercial manufacturers produce nitric acid (HNO3) by the Ostwald process. The process requires three steps:

Chemistry
1 answer:
Shkiper50 [21]3 years ago
5 0

Answer:

this doesnt make sence ezxplain the subject

Explanation:

You might be interested in
A gas has a volume of 5.00 L at 0°C. What final temperature, in degrees Celsius, is needed to change the volume of the gas to ea
Diano4ka-milaya [45]

Answer:

A = -213.09°C

B = 15014.85 °C

C = -268.37°C

Explanation:

Given data:

Initial volume of gas = 5.00 L

Initial temperature = 0°C  (273 K)

Final volume = 1100 mL, 280 L, 87.5 mL

Final temperature = ?

Solution:

Formula:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Conversion of mL into L.

Final volume = 1100 mL/1000 = 1.1 L

Final volume =  87.5 mL/1000 = 0.0875 L

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

T₂ = V₂T₁ / V₁

T₂ = 1.1 L × 273 K / 5.00 L

T₂ = 300.3 L.K / 5.00 K

T₂ = 60.06 K

60.06 K - 273 = -213.09°C

2)

V₁/T₁ = V₂/T₂

T₂ = V₂T₁ / V₁

T₂ = 280 L × 273 K / 5.00 L

T₂ = 76440 L.K / 5.00 K

T₂ = 15288 K

15288 K - 273 = 15014.85 °C

3)

V₁/T₁ = V₂/T₂

T₂ = V₂T₁ / V₁

T₂ = 0.0875 L × 273 K / 5.00 L

T₂ = 23.8875 L.K / 5.00 K

T₂ = 4.78 K

4.78 K - 273 = -268.37°C

4 0
2 years ago
A + B = AB
Ahat [919]

The greatest amount of AB would be produced if the equilibrium constant of the reaction is equal to 1.0 \;X \;10^5. Hence, option D is correct.

<h3>What is an equilibrium constant?</h3>

A number that expresses the relationship between the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature.

The equilibrium constant expression is a mathematical relationship that shows how the concentrations of the products vary with the concentration of the reactants.

If the value of K is greater than 1, the products in the reaction are favoured. If the value of K is less than 1, the reactants in the reaction are favoured.

Hence, option D is correct.

Learn more about the equilibrium constant here:

brainly.com/question/10038290

#SPJ1

7 0
2 years ago
You put two open cans of soda on the table. You took one can from the refrigerator and the other from your car. When you open th
sladkih [1.3K]
The correct answer from the choices given is the last option. The can from the <span> car will lose the carbon more quickly because there are fewer solute–solvent collisions. The can in the car has a lower temperature than the one in the refrigerator. At low temperature, the solubility of carbon dioxide in the liquid decrease therefore particles would tend to be in the vapor phase and escape from the liquid.</span>
6 0
3 years ago
Wich of these equations are balanced? a) H2SO4+2AL---&gt;AL2(SO4) b)2KCL+Pb(NO3)2---&gt;2KNO3+PbCL2
Zolol [24]

The answer is b since on a it says H2 but on the right side there is no H idk if you forgot to put H there so im guessing b. Have a good day

4 0
2 years ago
When 12 moles of methanol (ch3oh) and 24 moles of oxygen gas react according to the chemical equation below, what is the limitin
Nataliya [291]
The balanced reaction equation for the reaction between CH₃OH and O₂ is 
                        2CH₃OH(l) + 3O₂(g) → 2CO₂(g) + 4H₂O(l)
Initial moles        12                24
Reacted moles   12                18
Final moles          -                   6              12               24
 
The stoichiometric ratio between CH₃OH and O₂ is 2 : 3
Hence,
   reacted moles of O₂ = reacted moles of CH₃OH x (3/2)
                                      = 12 mol x 3 / 2  
                                      = 18 mol

All of CH₃OH moles react with O₂.

Hence, the limiting agent is CH₃OH. 

Excess reagent is O₂.
Amount of moles of excess reagent left = 24 - 18 mol = 6 mol
                                            
5 0
3 years ago
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