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When the amount of gas in a container is increased, the volume increases. Lussac's law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.
Answer: gas molecules will hit the container walls more frequently and with greater force
Explanation:
According to the postulates of kinetic molecular theory:
1. The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls.
2. The average kinetic energy of the gas molecules is proportional to the kelvin temperature of the gas.
When the temperature is increased, so the average kinetic energy and the rms speed also increase. This means that the gas molecules will hit the container walls more frequently and with greater force because they are all moving faster. This increase the pressure.
A firework exploding is a chemical change as soon as you light the fuse the combustion reacts with the gunpowder.
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