Under which conditions of temperature and pressure would helium behave most like an ideal gas?

2 answers:

8 0

At conditions 50 K and 20 kPa of temperature and pressure would helium behave most like an ideal gas. The answer is number 1. This is because the temperature is so low and the pressure is low too.

xenn [34]3 years ago

5 0

Answer : The correct option is, (3) 750 K and 20 kPa

Explanation :

The conditions for ideal gas are :

Ideal gas are those gas that has no intermolecular attractions.

Ideal gas are those gas that have negligible volume.

The ideal gas equation is,

$PV=nRT$

The conditions for real gas are :

Real gas are those gas that have intermolecular attractions.

Real gas are those gas that have volume.

The real gas equation is,

$(P+\frac{an^2}{V^2})(V-nb)=nRT$

A real gas behave ideally at high temperature and low pressure condition.

From the given options, option (3) have high temperature and low pressure is the correct option.

Hence, at 750 K and 20 kPa conditions of temperature and pressure does a sample of helium behave most like an ideal gas.

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Nitrogen dioxide gas is dark brown in color and remains in equilibrium with dinitrogen tetroxide gas, which is colorless.

sukhopar [10]

Answer:

This reaction is exothermic because the system shifted to the left on heating.

Explanation:

2NO₂ (g) ⇌ N₂O₄(g)

Reactant => NO₂ (dark brown in color)

Product => N₂O₄ (colorless)

From the question given above, we were told that when the reaction at equilibrium was moved from room temperature to a higher temperature, the mixture turned dark brown in color.

This simply means that the reaction does not like heat. Hence the reaction is exothermic reaction.

Also, we can see that when the temperature was increased, the reaction turned dark brown in color indicating that the increase in the temperature favors the backward reaction (i.e the equilibrium shift to the left) as NO₂ which is the reactant is dark brown in color. This again indicates that the reaction is exothermic because an increase in the temperature of an exothermic reaction will shift the equilibrium position to the left.

Therefore, we can conclude that:

The reaction is exothermic because the system shifted to the left on heating.

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3 years ago

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Aleks [24]

Answer:

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Explanation:

hope it helps!

7 0

2 years ago