Imagine that you have a 7.00L gas tank and a 4.50L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 105atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time?

i just need to know how to get the temperature, do i assume it is the standard 273K?

You still feel compelled to use different screen names? It's still confusing to us.

Yes, 273 will work. Any T will work if you use the same one for both calculations.

Imagine that you have a 5.00L gas tank and a 3.50L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 105atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases.

To determine the pressure at which you should fill the acetylene tank, you need to consider 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 this case, you want to find the pressure for which both the oxygen and acetylene tanks will run out of gas at the same time.

Assuming that the temperature is the standard 273K (0°C or 32°F), you can calculate the number of moles of gas in each tank using the ideal gas law equation. Let's assume the initial pressure in the oxygen tank is 105 atm and the initial pressure in the acetylene tank is P (unknown).

First, calculate the number of moles of oxygen using the ideal gas law:
n_oxygen = (P_oxygen * V_oxygen) / (R * T)
n_oxygen = (105 atm * 7.00 L) / (R * 273 K)

Then, calculate the number of moles of acetylene using the same equation:
n_acetylene = (P_acetylene * V_acetylene) / (R * T)
n_acetylene = (P * 4.50 L) / (R * 273 K)

Since you want both tanks to run out of gas at the same time, the number of moles of each gas should be equal. Therefore, n_oxygen = n_acetylene.

Now, you can set up an equation to solve for the unknown pressure P:
(105 atm * 7.00 L) / (R * 273 K) = (P * 4.50 L) / (R * 273 K)

You can cancel out the common factors, R and 273 K:
(105 atm * 7.00 L) = P * 4.50 L

Divide both sides of the equation by 4.50 L:
P = (105 atm * 7.00 L) / 4.50 L

Simplifying the expression:
P = 163.33 atm

Therefore, to run out of both gases at the same time, you should fill the acetylene tank to a pressure of approximately 163.33 atm (assuming the temperature is 273 K or 0°C).

Note: Please be cautious while working with gases, as they can be hazardous. Always follow proper safety guidelines and consult relevant resources for specific instructions.