a 13.5L tank is filled with H2 to a pressure of 2x10^2atm. How many balloons (each 2L) can be inflated to a pressure of 1 atm from the tank?assume there is no temp change and tank cant be emptied below 1 atm of pressure

PV = nRT will give you n = number of mols H2 in the tank originally.

Redo PV = nRT and substitute 1 for P and calcualte n = number of mols at the end (since P can't go below 1 atm).

Now use PV = nRT to calculate the mols used to fill a single balloon.

You should be able to determine how many balloons can be filled with the total mols you have.

Post your work if you get stuck.

To solve this problem, we can use the ideal gas law:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, let's calculate the number of moles of H2 gas in the tank.

Given:
Volume of the tank (V1) = 13.5 L
Pressure in the tank (P1) = 2x10^2 atm

We can rearrange the ideal gas law to solve for moles (n):

n = (P1 * V1) / (R * T)

As it is mentioned that there is no temperature change, we can disregard the 'T' value.

Using the ideal gas constant (R = 0.0821 L·atm/(mol·K)), we can calculate the number of moles:

n = (2x10^2 atm * 13.5 L) / (0.0821 L·atm/(mol·K))

n ≈ 164.752 moles

Now, let's calculate the number of balloons that can be inflated.

Given:
Volume of each balloon (V2) = 2 L
Pressure needed for each balloon (P2) = 1 atm

Similar to the previous calculation, we can use the ideal gas law to solve for the number of moles (n):

n = (P2 * V2) / (R * T)

Disregarding temperature as mentioned, we can use the same ideal gas constant (R = 0.0821 L·atm/(mol·K)):

n = (1 atm * 2 L) / (0.0821 L·atm/(mol·K))

n ≈ 0.1217 moles

Now, we can calculate the number of balloons that can be inflated by dividing the total number of moles available by the number of moles needed for each balloon:

Number of balloons = (Total moles) / (Moles per balloon)

Number of balloons = 164.752 moles / 0.1217 moles

Number of balloons ≈ 1353.99

Therefore, approximately 1353 balloons (each with a volume of 2L) can be inflated to a pressure of 1 atm from the given tank.

To solve this problem, we can use the Ideal Gas Law equation, which states PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature (assuming temperature is constant).

Given:
Initial pressure (P1) = 2×10^2 atm
Initial volume (V1) = 13.5 L
Final pressure (P2) = 1 atm
Final volume (V2) = 2 L

We need to find the number of moles of hydrogen gas in the tank (n1) and the number of moles in each balloon (n2), and then calculate how many balloons can be inflated.

Step 1: Calculate the initial number of moles in the tank.
Using the Ideal Gas Law equation (PV = nRT), we rearrange it to find the number of moles (n).

n1 = (P1 * V1) / (R * T)

Since the temperature is constant in this problem, we can assume R and T will cancel out. The value of R is 0.0821 (atm L / mol K).

n1 = (2×10^2 atm * 13.5 L) / (0.0821 atm L / mol K)
n1 ≈ 275.30 mol

Therefore, the initial number of moles of hydrogen gas in the tank is approximately 275.30 mol.

Step 2: Calculate the final number of moles in each balloon.
Since the pressure in each balloon is 1 atm and the volume is 2 L, we can use the Ideal Gas Law equation again to find the number of moles (n2) in each balloon.

n2 = (P2 * V2) / (R * T)
n2 = (1 atm * 2 L) / (0.0821 atm L / mol K)
n2 ≈ 0.024 mol

Therefore, the final number of moles of hydrogen gas in each balloon is approximately 0.024 mol.

Step 3: Calculate the number of balloons that can be inflated.
To find the number of balloons that can be inflated, divide the initial number of moles in the tank (n1) by the final number of moles in each balloon (n2).

Number of balloons = n1 / n2
Number of balloons ≈ 275.30 mol / 0.024 mol
Number of balloons ≈ 11,470

Therefore, approximately 11,470 balloons can be inflated with the given conditions.

Note: It's important to consider that the Ideal Gas Law assumes ideal gas behavior, and in practice, real gases may deviate slightly from ideal behavior.