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zysi [14]
3 years ago
12

Maintaining constant pressure, the volume of a gas is increased from 12,0 L

Chemistry
1 answer:
kow [346]3 years ago
3 0

Answer:

790 K

Explanation:

Step 1: Given data

  • Initial volume of the gas (V₁): 12.0 L
  • Initial temperature of the gas (T₁): 23.0 °C
  • Final volume of the gas (V₂): 32.0 L

Step 2: Convert 23.0 °C to Kelvin

We will use the following expression.

K = °C + 273.15 = 23.0 + 273.15 = 296.2 K

Step 3: Calculate the final temperature of the gas

Assuming constant pressure and ideal behavior, we can calculate the final temperature of the gas using Charles' law.

T₁/V₁ = T₂/V₂

T₂ = T₁ × V₂/V₁

T₂ = 296.2 K × 32.0 L/12.0 L = 790 K

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A sample of 23.2 g of nitrogen gas is reacted with
slavikrds [6]

Answer:

1.66 moles.

Explanation:

We'll begin by calculating the number of mole in 23.2 g of nitrogen gas, N2.

This is illustrated below:

Molar mass of N2 = 2x14 = 28 g/mol

Mass of N2 = 23.2 g

Mole of N2 =.?

Mole = mass /Molar mass

Mole of N2 = 23.2/28

Mole of N2 = 0.83 mole

Next, we shall determine the number of mole in 23.2 g of Hydrogen gas, H2.

This is illustrated below:

Molar mass of H2 = 2x1 = 2 g/mol

Mass of H2 = 23.2 g

Mole of H2 =?

Mole = mass /Molar mass

Mole of H2 = 23.2/2

Mole of H2 = 11.6 moles

Next, the balanced equation for the reaction. This is given below:

N2 + 3H2 —> 2NH3

From the balanced equation above,

1 mole of N2 reacted with 3 moles of H2 to produce 2 moles of NH3.

Next, we shall determine the limiting reactant. This can be obtained as follow:

From the balanced equation above,

1 mole of N2 reacted with 3 moles of H2.

Therefore, 0.83 moles will react with = (0.83 x 3) = 2.49 moles of H2.

From the calculations made above, we can see that only 2.49 moles out of 11.6 moles of H2 is required to react completely with 0.83 mole of N2.

Therefore, N2 is the limiting reactant.

Finally, we shall determine the maximum amount of NH3 produced from the reaction.

In this case, we shall use the limiting reactant because it will give the maximum yield of NH3 since all of it is consumed in the reaction.

The limiting reactant is N2 and the maximum amount of NH3 produced can be obtained as follow:

From the balanced equation above,

1 mole of N2 reacted to produce 2 moles of NH3.

Therefore, 0.83 mole of N2 will react to produce = (0.83 x 2) = 1.66 moles of NH3.

Therefore, the maximum amount of NH3 produced from the reaction is 1.66 moles.

5 0
3 years ago
1. Which of the following is a correctly written thermochemical equation?
WITCHER [35]

Explanation:

1. Thermochemical equation is balance stoichiometric chemical equation written with the phases of the reactants and products in the brackets along with the enthalpy change of the reaction.

The given correct thermochemical reactions are:

Fe(s)+O_2(g)\rightarrow Fe_2O_3(s),\Delta H = 3,926 kJ


C_3H_8(g)+5O_2 (g)\rightarrow 3CO_2 (g)+4H_2O(l),\Delta H= 2,220 kJ/mol

2. Phase change affect the value of the enthalpy change of the thermochemical equation. This is because change in phase is accompanied by change in energy. For example:

H_2O(s)\rightarrow H_2O(g),\Delta H_{s}=51.1 kJ/mol

H_2O(l)\rightarrow H_2O(g),\Delta H_{v}=40.65 kJ/mol

In both reaction phase of water is changing with change in energy of enthalpy of reaction.

7 0
3 years ago
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How does the use of synthetic oil impact the natural resource from which they are derived?
omeli [17]
Its destructing the nature
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3 years ago
Which organism is a tertiary consumer?<br> clownfish<br> brittle star<br> killer whale<br> octopus
vlada-n [284]

Answer:

killer whale

Explanation:

7 0
3 years ago
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An average bushel of apples has a mass of 10 kg and contains 5 dozen apples.
Alina [70]

Answer:

Average mass of 6 apple  = 1 kg

Explanation:

Given:

Average mass of 5 dozen apple = 10 kg

Find:

Average mass of 6 apple

Computation:

Average mass of 6 apple  = [Average mass of 1 apple] x [6 apple]

Average mass of 6 apple  = [10/(12 x 5)] x [6]

Average mass of 6 apple  = 1 kg

3 0
3 years ago
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