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Why does increasing the temperature of a solid make it melt? Increasing the temperature increases molecular vibrations until attractive forces can no longer hold the molecules in one place. … Cooling slows molecular motion until attractive forces between molecules can hold them in place.
As temperature increases, molecules gain energy and move faster and faster. Therefore, the greater the temperature, the higher the probability that molecules will be moving with the necessary activation energy for a reaction to occur upon collision.
The temperature of the gas is proportional to the average kinetic energy of the gas molecules. The particles moving faster collide with the container walls frequently with greater force. This causes the force on the walls of the container to increase and so the pressure increases.
The combined gas law states that the pressure of a gas is inversely related to the volume and directly related to the temperature. If temperature is held constant, the equation is reduced to Boyle’s law. Therefore, if you decrease the pressure of a fixed amount of gas, its volume will increase.
Decreasing temperature decreases the kinetic energy of gas particles and applying pressure decreases the space between particles which in turn strengthens the attractive forces between particles. These changes force the gas to liquefy and change its state to liquid.
According to Kinetic Molecular Theory, an increase in temperature will increase the average kinetic energy of the molecules. As the particles move faster, they will likely hit the edge of the container more often.
With the increase in temperature the kinetic energy of the particles increases and starts moving faster. The kinetic energy of the particles is more in gases and least in solids.
Temperature has a direct effect on whether a substance exists as a solid, liquid or gas. Generally, increasing the temperature turns solids into liquids and liquids into gases; reducing it turns gases into liquids and liquids into solids.
When heat transfer is involved, use this formula: change in temperature = Q / cm to calculate the change in temperature from a specific amount of heat added. Q represents the heat added, c is the specific heat capacity of the substance you’re heating, and m is the mass of the substance you’re heating.
An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision (Figure. 17.5 “Temperature and Reaction Rate”).
An increase in the temperature of a system favors the direction of the reaction that absorbs heat, the endothermic direction. Absorption of heat in this case is a relief of the stress provided by the temperature increase. For the Haber-Bosch process, an increase in temperature favors the reverse reaction.
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