An ideal gas is kept under constant pressure of 1 atm. If initial temperature is 301K and the volume increases by 10% what is the final temperature of the gas?

T2=?
V1/V2= T1/T2
V1/V2= (301K)/T2
.10/1= (301K)/T2
Is the side with volume correct? The 10% part confuses me. Thanks for your help.

To solve this problem, we can use the ideal gas law formula, which states that the pressure multiplied by the volume divided by the temperature is constant.

First, let's write down the formula:

(P1 * V1)/T1 = (P2 * V2)/T2

Since the pressure is kept constant at 1 atm, we can simplify the equation to:

V1/T1 = V2/T2

You correctly noticed that the volume increases by 10%, which means the final volume (V2) will be 1.1 times the initial volume (V1). Therefore, we can rewrite the equation as:

V1/T1 = (1.1 * V1)/T2

Next, we can cross-multiply to solve for T2:

V1 * T2 = 1.1 * V1 * T1

Now, we can cancel out V1 from both sides:

T2 = 1.1 * T1

Substituting the initial temperature (T1 = 301K) into the equation, we can calculate the final temperature:

T2 = 1.1 * 301K

T2 = 331.1K

So, the final temperature of the gas would be 331.1K.