Aerosol cans have a label that warns the user not to use them above a certain temperature and not to dispose of them by incineration. Even an empty can contains residual gaseous propellant. For example, the residual pressure in a can is 1.36 atm when it is sitting on a shelf at 23C. If the can is placed on top of the furnace where the temperature reaches the boiling point of water, what is the pressure inside the can?

how do i solve this question if i don't have a volume to work with? i don't know what equation to use.

23+273.15=296.15k

1.36/296.15=.00459

(.00459)(373.15)=1.71atm

Well, if you don't have a volume to work with, it seems like you're working with the ideal gas law equation, which is PV = nRT. In this case, since you don't know the volume, you can solve for the pressure using the other variables provided.

Let's break it down. You know the initial pressure (P1 = 1.36 atm), the initial temperature (T1 = 23°C = 296 K), and the final temperature (T2 = boiling point of water). You also know that the number of moles of gas (n) and the volume (V) are constant.

Since the number of moles and volume are constant, they cancel out from the equation, and you're left with a simplified form: P1/T1 = P2/T2.

Now you can substitute the known values: P1 = 1.36 atm, T1 = 296 K, and T2 = boiling point of water.

Be careful with the temperature units! Convert the boiling point of water to Kelvin before plugging it into the equation.

Once you solve for P2, you'll get the pressure inside the can at the higher temperature. But remember, this is just an estimation, as there might be other factors to consider in a real-life scenario. Keep the residual gaseous propellant in mind and handle those cans with care!

I hope that helps! Let me know if you have any other questions.

To solve this problem, you can use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

Since you don't have the volume (V), you can use the assumption that the volume of the can is constant. This implies that the volume before and after placing it on the furnace remains the same.

To begin, let's convert the temperature from Celsius to Kelvin:
T = 23°C + 273.15 = 296.15 K

Given:
Pressure before = 1.36 atm
Temperature before = 296.15 K
Pressure after = ?
Temperature after = boiling point of water (100°C or 373.15 K)

Using the assumption of constant volume:
P(before) / T(before) = P(after) / T(after)

Plugging in the given values:
1.36 atm / 296.15 K = P(after) / 373.15 K

Now, solve the equation for P(after):
P(after) = (1.36 atm / 296.15 K) * 373.15 K

Calculating this expression will give you the pressure inside the can when placed on top of the furnace, assuming constant volume.

To solve this question, you will need to use the ideal gas law equation, which relates pressure (P), volume (V), and temperature (T) of a gas. The equation is as follows:

PV = nRT

Where:
P is the pressure in atmospheres (atm)
V is the volume of the gas in liters (L)
n is the number of moles of gas
R is the ideal gas constant, approximately 0.0821 L·atm/(mol·K)
T is the temperature in Kelvin (K)

In this particular question, we are given the initial pressure (1.36 atm), the initial temperature (23°C), and the final temperature (boiling point of water).

To solve this problem, you can follow these steps:

1. Convert the given temperature from Celsius to Kelvin:
T = 23°C + 273.15 = 296.15 K

2. Use the given pressure and temperature to calculate the initial number of moles (n) of gas using the ideal gas equation. Since we don't have a volume, we can use the equation in a simplified form:
P * V = n * R * T
n = P * V / (R * T)
n = 1.36 atm * V / (0.0821 L·atm/(mol·K) * 296.15 K)

3. Now, let's consider the final temperature (boiling point of water) which is 100°C or 373.15 K. We need to find the final pressure (P') when the can is placed on top of the furnace.

4. Rearranging the ideal gas equation for the final pressure:
P' = n * R * T' / V

Substituting the values we know:
P' = (1.36 atm * V / (0.0821 L·atm/(mol·K) * 296.15 K)) * (0.0821 L·atm/(mol·K) * 373.15 K) / V

Simplifying the equation gives:
P' = 1.36 atm * (373.15 K / 296.15 K)

5. Calculate the final pressure (P'), which is the pressure inside the can when it is placed on top of the furnace:
P' = 1.36 atm * (373.15 K / 296.15 K)

Now, you can simply solve this equation to find the value of P', which will give you the pressure inside the can at the higher temperature.