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Luden [163]
3 years ago
7

Look at the following reaction. How could you increase the production of 2NH3(g)? N2(g) + 3H2(g) 2NH3(g) Increase the volume of

the reaction vessel. Increase the pressure of the system. Decrease the pressure of the system. Remove N2(g) from the system.
Chemistry
2 answers:
Zolol [24]3 years ago
5 0
The correct option is B. To increase the production of ammonia, you have to increase the pressure of the system. Increase in pressure will result in increased production of ammonia because this will drive the chemical reaction forward.
ivolga24 [154]3 years ago
3 0

Answer: Option (b) is the correct answer.

Explanation:

When we apply pressure or increase the pressure then molecules of the gas come closer to each other. As a result, forces of attraction will increase which will lead to increase in production of the product.

Therefore, in the given reaction the production can be increased by increasing the pressure of the system.

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-2(bx-5)=16 slove for b<br>​
Papessa [141]

Explanation:

SADMEP

-2(bx-5) = 16 distribute

-2bx +10 = 16 subtracte

-10 -10

-2bx = 6

divide by -2x (on both sides)

b = -3x

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2 years ago
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A saturated solution of Barium Chloride at 30’C contains 150.0g water. How much additional Barium Chloride can be dissolved by h
oksian1 [2.3K]
Wouldn't it be just dubble the amount witch would be 300.0g water
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2 years ago
A gas has a pressure of 326 mm Hg at 20 degrees Celsius. What is the temperature at 52.4 k Pa?
jonny [76]

Answer:

it's is math that you can answer with your sister and your mother

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2 years ago
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The force of attraction that holds two atoms together is called a "chemical bond". True or false? if false, what is the right an
Annette [7]
1: False; electrical force 2:true



3 0
3 years ago
At 650 K, the reaction MgCO3(s)⇌MgO(s)+CO2(g)MgCO3(s)⇌MgO(s)+CO2(g) has Kp=0.026Kp=0.026. A 10.0-L container at 650 K has 1.0 g
Ray Of Light [21]

Answer:

0.4076 g

Explanation:

Kp is the equilibrium constant based on pressure and depends only on gas substances. For a generic reaction

aA + bB ⇄ cC + dD

Kp = \frac{(pC)^c*(pD)^d}{(pA)^a*(pB)^b}, where pX is the pressure of X in equilibrium.

For the reaction Kp = pCO₂

pCO₂ = 0.026 atm

The system is in equilibrium at the beginning. The compression occurs at a constant temperature, so using Boyle's law

P1V1 = P2V2

0.026*10 = P2*0.1

P2 = 2.6 atm

The reaction will reach again the equilibrium, and pCO₂ = 0.026 atm, then the rest will form MgCO₃, which will be 2.6 - 0.026 = 2.574 atm.

By the ideal gas law:

PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm*L/mol*K), and T is the temperature.

2.574*0.1 = n*0.082*650

53.3n = 0.2574

n = 4.83x10⁻³ mol

The stoichiometry of the reaction is 1 mol of MgCO₃ for 1 mol of CO₂, so it will form 4.83x10⁻³ mol of MgCO₃  .

The molar mass is:

MgCO₃: 24 g/mol of Mg + 12 g/mol of C + 3*16 g/mol of O = 84 g/mol

The mass formed is the molar mass multiplied by the number of moles:

m = 84x4.83x10⁻³

m = 0.4076 g

3 0
2 years ago
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