a tank of helium gas used to inflate toy baloons is a pressure of 15.5 x 10 Pa and a temp of 293 k. The tank's volume is 0.020 m. How are a baloon would it fill at 1.00 atmosphere and 323 k

169m^3

To solve this problem, we'll use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant (8.31 J/(mol·K))
T = temperature

Step 1: Convert the pressure from 1.00 atm to Pascals (Pa).
1 atm = 101325 Pa, so 1.00 atm = 101325 Pa.

Step 2: Calculate the number of moles of gas in the tank at the initial conditions.
Using the ideal gas law equation, we can rearrange it to solve for n:
n = PV / RT

n = (15.5 x 10 Pa) * (0.020 m) / ((8.31 J/(mol·K)) * 293 K)

Step 3: Calculate the number of moles of gas at the final conditions.
Since the number of moles remains constant, n is the same at both initial and final conditions.

Step 4: Calculate the volume of the balloon at the final conditions using the ideal gas law.
Rearrange the ideal gas law equation to solve for V:
V = nRT / P

V = (n * (8.31 J/(mol·K)) * 323 K) / (101325 Pa)

Step 5: Calculate the number of balloons that can be filled with the volume of the balloon at the final conditions.
Divide the volume of the tank by the volume of a single balloon.
Number of balloons = (Volume of tank) / (Volume of a single balloon)

Please note that you need to provide the volume of a single balloon in order to calculate the final number of balloons that can be filled.

To determine how many balloons the tank of helium gas would fill, we can use the ideal gas law equation, which relates the pressure, volume, temperature, and the number of moles of gas.

The ideal gas law equation is expressed as:

PV = nRT

Where:
P is the pressure of the gas,
V is the volume of the gas,
n is the number of moles of gas,
R is the ideal gas constant, and
T is the temperature of the gas in Kelvin.

We are given:
P1 = 15.5 x 10^5 Pa (pressure in the tank)
V1 = 0.020 m^3 (volume of the tank)
T1 = 293 K (temperature of the tank)

We want to find the number of balloons the tank would fill at a different set of conditions:
P2 = 1.00 atm (pressure for filling the balloons)
T2 = 323 K (temperature for filling the balloons)

First, let's calculate the number of moles of helium gas in the tank using the initial conditions:

n = PV / RT

n1 = (15.5 x 10^5 Pa) * (0.020 m^3) / (8.314 J/(mol·K) * 293 K)

Now, we can use the number of moles of gas to find the number of balloons it would fill at the new conditions using the ideal gas law:

n2 = P2V2 / RT2

We are given:
P2 = 1.00 atm = 1.013 x 10^5 Pa (converting atm to Pa)
V2 = unknown (volume of a balloon)
T2 = 323 K (temperature for filling the balloons)

n2 = (1.013 x 10^5 Pa) * V2 / (8.314 J/(mol·K) * 323 K)

Since we are looking for the number of balloons the tank can fill, we need to compare the number of moles of helium gas in the tank (n1) to the number of moles required to fill one balloon (n2).

To determine the volume of one balloon (V2), we can rearrange the formula for n2:

V2 = (n2 * 8.314 J/(mol·K) * 323 K) / (1.013 x 10^5 Pa)

Finally, we can substitute the values of n1 and V2 in the equation to find the number of balloons the tank would fill:

Number of balloons = n1 / (V2 * Avogadro's number)

Avogadro's number is approximately equal to 6.022 x 10^23.

So, by plugging in the values and following these calculations, we can determine the number of balloons the tank would fill at the given conditions.

how many moles?

n=PV/RT in the tank.

outside the tank

Outside the tank volume= nRT/P

You didn't say how much volume each balloon had.