Question

What are the three ways that we can decrease the pressure of a gas inside a container?

A. List three ways.

B. Using the macro/micro tables show how each of these two sus decreases pressure. Indicate whether each quantity increases, decreases, or remains the same. What does decreasing the temperature if a gas do on the molecular level? Why does it decrease the pressure?

Answer 1

Three Ways to Increase the Pressure of a Gas

1 .Increment the measure of gas. This is spoken to by the "n" in the condition. Including more particles of a gas builds the quantity of impacts between the atoms and the dividers of the holder. This raises weight.

2. Increment the temperature of the gas. This is spoken to by "T" in the condition. Expanding temperature adds vitality to the gas particles, expanding their movement and, once more, expanding impacts.

3. Reduction the volume of the gas. This is the "V" in the condition. By their extremely nature, gases can be packed, so if similar gas can be put into a littler compartment, it will apply a higher weight. The gas atoms will be constrained nearer to each other, expanding crashes (power) and weight.

More gas is available in an answer with a lower temperature contrasted with an answer with a higher temperature. ... Expanded temperature causes an expansion in dynamic vitality. The higher active vitality causes more movement in particles which break intermolecular bonds and escape from arrangement.

Rather than atoms in a fluid or strong, those in a gas can move unreservedly in the space in which you bind them. They fly about, once in a while crashing into each other and with the compartment dividers. The aggregate weight they apply on the holder dividers relies upon the measure of vitality they have. They get vitality from the warmth in their environment, so if the temperature goes up, so does the weight. Truth be told, the two amounts are connected by the perfect gas law.

How Pressure Varies With Temperature

For whatever length of time that the volume and mass of the gas are consistent, the connection amongst weight and temperature moves toward becoming P = KT, where K is a steady got from the volume, number of moles of gas and the perfect gas consistent. In the event that you put a gas that satisfies perfect gas conditions into a compartment with inflexible dividers so the volume can't change, seal the holder and measure the weight on the holder dividers, you will see it diminish as you bring down the temperature. Since this relationship is direct, you simply require two readings of temperature and strain to draw a line from which you can extrapolate the weight of the gas at any given temperature.

This straight relationship separates at low temperatures when the blemished flexibility of the gas particles ends up sufficiently imperative to influence comes about, however the weight will in any case diminish as you bring down the temperature. The relationship will likewise be nonlinear if the gas particles are sufficiently extensive to block characterizing the gas as perfect.