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iren [92.7K]
2 years ago
8

Continuing from the last question, what is the new pressure inside the container? Hint: Did we use up all of the reactants?

Chemistry
1 answer:
Leya [2.2K]2 years ago
7 0

If all the reactors are used, the pressure inside the flask will most likely increase to 4 atm.

<h3>What is atmospheric pressure?</h3>

Atmospheric pressure is a force per unit area exerted by the air in the atmosphere on the Earth's surface. The value of atmospheric pressure above sea level is 1013.25 hPa.

<h3>What influences the variation of atmospheric pressure?</h3>

The atmospheric pressure varies from different meteorological factors such as:

  • Decreases with altitude.
  • It varies according to latitude, the lowest atmospheric pressure at sea level is reached in the equatorial latitudes.
  • The equatorial zone has high atmospheric pressures for dynamic reasons derived from the Earth's rotation.

According to the above, if all the reactors are used at atmospheric pressure, it will most likely increase.

Note: This question is incomplete because some information is missing. However I can answer it based on my prior knowledge.

Learn more about atmospheric pressure in: brainly.com/question/1393320

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Two solutions, initially at 24.60 °C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J/°C). When a 100.0 mL volume of 0.100
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Answer:

ΔH = -59.6kJ/mol

Explanation:

The reaction that occurs between Ag⁺ and Cl⁻ ions is:

Ag⁺ + Cl⁻ → AgCl(s) + ΔH

To find ΔH we need to obtain moles of reaction and heat released in the reaction because ΔH is defined as heat released per mole of reaction.

<em>Moles of reaction:</em>

Moles of Ag⁺ and Cl⁻ added are:

Ag⁺: 0.100L * (0.100mol / L) = 0.01moles

Cl⁻: 0.100L * (0.200mol / L) 0 0.02 moles

That means limiting reactant is Ag⁺ and moles of reaction are 0.01 moles

<em>Heat released:</em>

To find heat released we must use coffe cup calorimeter equation:

Q = C*m*ΔT

<em>Where C is specific heat of solution (4.18J/g°C), m is the mass of solution (200g because there are 100 + 100mL = 200mL and density of solution is 1g/mL) and ΔT is change in temperature (25.30°C - 24.60°C = 0.70°C).</em>

Replacing:

Q = C*m*ΔT

Q = 4.18J/g°C * 200g * 0.70°C

Q = 585,2J

Is total heat released.

The calorimeter absorbs:

15.5J / °C * 0.7°C = 10.85

Thus, when 0.01 moles reacts, 585.2J + 10.85  = 596.05J are released (Heat released is heat abosrbed by calorimeter + Heat absorbed by water) and ΔH is:

ΔH = 596.05J / 0.01 moles =

ΔH = 59605J / mol =

<h3>ΔH = -59.6kJ/mol</h3>

<em>As heat is released, ΔH < 0.</em>

6 0
3 years ago
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