Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose a can contains a residual amount of gas at a pressure of 750mmHg and a temperature of 23∘C. What would the pressure be if the can were heated to 1220∘C?

I think I am over thinking this? help!!!

PV=kT, so P/T is constant

Figure the increase in T (as a factor), and apply that same factor to P to keep the ratio constant.

To solve this problem, we can use the ideal gas law, which states that PV = nRT, where:

P = pressure of the gas
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant
T = temperature of the gas in Kelvin

In this case, we are given the initial pressure (P1), temperature (T1), and we need to find the final pressure (P2) when the temperature is increased to a certain value (T2).

First, let's convert the temperatures to Kelvin by adding 273.15 to each value:
T1 = 23°C + 273.15 = 296.15 K
T2 = 1220°C + 273.15 = 1493.15 K

Now, let's solve for P2 using the following relationship:

P1/T1 = P2/T2

Substituting the given values, we have:
750 mmHg / 296.15 K = P2 / 1493.15 K

To find P2, we can cross-multiply and solve for it:
750 mmHg * 1493.15 K = P2 * 296.15 K

By multiplying these values and dividing by 296.15, we can find the value of P2:
P2 = (750 mmHg * 1493.15 K) / 296.15 K

Calculating this expression, we get:
P2 ≈ 3790 mmHg

Therefore, if the can were heated to 1220°C, the pressure inside the can would be approximately 3790 mmHg.