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krok68 [10]
2 years ago
15

A sample of 0.200 moles of nitrogen occupies 0.400 L. Under the same conditions, what number of moles occupies 1.200 L

Chemistry
1 answer:
IRISSAK [1]2 years ago
7 0

The number of mole of nitrogen that occupies 1.2 L under the same condition is 0.6 mole

<h3>Data obtained from the question </h3>
  • Initial mole (n₁) = 0.2 mole
  • Initial volume (V₁) = 0.4 L
  • Final volume (V₂) = 1.2 L
  • Final mole (n₂) =?

<h3>How to determine the final mole </h3>

The final mole can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

Divide both side n

PV / n = RT

Divide both side by P

V / n = RT / P

RT / P = constant

V / n = constant

Thus,

V₁ / n₁ = V₂ / n₂

0.4 / 0.2 = 1.2 / n₂

2 = 1.2 / n₂

Cross multiply

2 × n₂ = 1.2

Divide both side by 2

n₂ = 1.2 / 2

n₂ = 0.6 mole

Learn more about ideal gas equation:

brainly.com/question/4147359

#SPJ1

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6 0
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The enthalpy of vaporization of Bromine is 15.4 kJ/mol. What is the energy change when 80.2 g of Br2 condenses to a liquid at 59
Aleksandr-060686 [28]

The enthalpy of vaporization of Bromine is 15.4 kJ/mol. -7.7 kJ is the energy change when 80.2 g of Br₂ condenses to a liquid at 59.5°C.

<h3>What is Enthalpy of Vaporization ?</h3>

The amount of enthalpy or energy that must be added to a liquid substance into gas substance is called Enthalpy of Vaporization. It is also known as Latent heat of vaporization.

<h3>How to find the energy change from enthalpy of vaporization ?</h3>

To calculate the energy use this expression:

Q = n \Delta H_{\text{vapo.}

where,

Q = Energy change

n = number of moles

\Delta H_{\text{Vapo.}} = Molar enthalpy of vaporization

Now find the number of moles

Number of moles (n) = \frac{\text{Given Mass}}{\text{Molar mass}}

                                   = \frac{80.2\ g }{159.8\ g/mol}

                                   = 0.5 mol

Now put the values in above formula we get

Q = - n \Delta H_{\text{vapo.}         [Negative sign is used because Br₂ condensed here]

   = - (0.5 mol × 15.4 kJ/mol)

   = - 7.7 kJ

Thus from the above conclusion we can say that The enthalpy of vaporization of Bromine is 15.4 kJ/mol. -7.7 kJ is the energy change when 80.2 g of Br₂ condenses to a liquid at 59.5°C.

Learn more about the Enthalpy of Vaporization here: brainly.com/question/13776849

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8 0
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