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yawa3891 [41]
3 years ago
15

When the temperature of a gas in a rigid container decreases, the particles of the gas move slower and experience fewer collisio

ns with each other and the container walls. Because of this, it is sometimes necessary to add more air to automobile tires in the winter.Which gas law applies in this situation?
Chemistry
2 answers:
4vir4ik [10]3 years ago
6 0
When the temperature of a gas within a rigid container decreases, the particles on average move more slowly and do not collide with one another or the container walls as often. It is the the ideal gas law that applies in this situation and states that a decrease in the temperature of a gas also results in a decrease in the pressure. Thus, automobile tyres which have a colder gas in the winter sometimes need additional air to provide suffiicient pressure. 
notsponge [240]3 years ago
6 0

Answer:

Gay Lusaac's law: The pressure Temperature Law

Explanation:

First off, it is important to understand that the fewer collisions experienced by the particles with each other and the walls of the container is referring to the pressure.

SO, form the question, we can tell that temperature and pressure are directly proportional to each other. As temperature increases, the particles move faster which in turn leads to increased pressure.

After that has been established, we look up the gas laws and find the pone that gives a temperature-pressure relationship and this is the Gay-Lussac's Law: The Pressure Temperature Law. This law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature. As the pressure goes up, the temperature also goes up, and vice-versa.

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24.6 ℃

<h3>Explanation</h3>

Hydrochloric acid and sodium hydroxide reacts by the following equation:

\text{HCl} \; (aq) + \text{NaOH} \; (aq) \to \text{NaCl} \; (aq) + \text{H}_2\text{O} \; (aq)

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Both the solution and the calorimeter absorb energy released in this neutralization reaction. Their temperature change is dependent on the heat capacity <em>C</em> of the two objects, combined.

The question has given the heat capacity of the calorimeter directly.

The heat capacity (the one without mass in the unit) of water is to be calculated from its mass and <em>specific</em> heat.

The calorimeter contains 1.00 liters or 1.00 \times 10^{3} \; \text{ml} of the 1.0 gram per milliliter solution. Accordingly, it would have a mass of 1.00 \times 10^{3} \; \text{g}.

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The calorimeter-solution system thus has a heat capacity of 4.634 \times 10^{3} \; \text{J} \cdot \text{K}^{-1}, meaning that its temperature would rise by 1 degree celsius on the absorption of 4.634 × 10³ joules of energy. 1.405 \times 10^{4} \; \text{J} are available from the reaction. Thus, the temperature of the system shall have risen by 3.03 degrees celsius to 24.6 degrees celsius by the end of the reaction.

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