Chemistry Question: Pressure Change at Different Temperatures

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In summary, a hydrogen cylinder holding gas at 3.67 atm and 25° C in a laboratory will experience a decrease in pressure when placed in a showroom with a temperature of 7° C. To calculate this change, you can use the gas laws, such as Charles law, Boyle's Law, the combined gas law, or the ideal gas law, by listing all known values and determining which equation to use based on the types of values given.
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hemihead_dave
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A hydrogen cylinder holds gas at 3.67 atm in a laboratory where the temperature is 25° C. To what will the pressure change when the cylinder is placed in a showroom where the temperature drops to 7° C?

I am having trouble calculating this question. Unsure what equation I need to use. Can anyone help?
 
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  • #2
What gas laws do you know?

You should use post template, now I have to ask questions that you should answer in your first post.
 
  • #3
I know Charles law, Boyle's Law, the combined gas law and the ideal gas law PV=nRT
 
  • #4
Begin by listing all of your known values. Just a straight forward before and after listfor each type of measurment (volumes, mass, pressure, temperatures, etc etc) that is given.
Then take a look at those formulas and see which equations utilize those types of values.
 

FAQ: Chemistry Question: Pressure Change at Different Temperatures

How does pressure change at different temperatures?

The relationship between pressure and temperature is described by the ideal gas law, which states that pressure and temperature are directly proportional. This means that as temperature increases, so does pressure, and vice versa. This is because at higher temperatures, gas molecules have more energy and move around more, causing them to collide with the walls of their container more frequently and with greater force, resulting in an increase in pressure.

How do you calculate pressure change at different temperatures?

To calculate pressure change at different temperatures, you can use the ideal gas law equation: PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin. By rearranging the equation to solve for pressure, you can plug in the values for volume, number of moles, gas constant, and temperature to calculate the pressure at a specific temperature.

How does pressure change when temperature decreases?

As stated by the ideal gas law, pressure and temperature are directly proportional. This means that as temperature decreases, so does pressure. This is because at lower temperatures, gas molecules have less energy and move around less, resulting in fewer collisions with the walls of their container and a decrease in pressure.

What is the effect of pressure change on chemical reactions?

Pressure can affect the rate and direction of chemical reactions. Increasing pressure usually results in an increase in the rate of a reaction, as it increases the frequency of collisions between reactant molecules. However, this is not always the case as some reactions may be endothermic and require an increase in pressure to occur in the reverse direction. Additionally, pressure can also affect the equilibrium position of a reaction, where a decrease in pressure can shift the equilibrium towards the side with fewer gas moles.

How is pressure change related to phase changes?

The pressure of a substance can also affect its phase changes. For example, at a constant temperature, increasing pressure can cause a substance to transition from a gas to a liquid, and then to a solid. This is because increasing pressure forces gas molecules closer together, reducing the space between them and causing them to condense into a liquid. Further increasing pressure can cause the liquid to solidify. On the other hand, decreasing pressure can cause a substance to undergo a phase change from solid to liquid to gas.

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