Determine the pressure change when a constant volume of gas at 1 .00 atm is heated from 293K to 303K. 1.5 atm 303 atm 1.03 atm 293 atm

## Step 1<br />The problem involves the application of Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature, provided the volume is kept constant. This can be mathematically represented as:<br />### \( \frac{P1}{T1} = \frac{P2}{T2} \)<br />where \( P1 \) and \( T1 \) are the initial pressure and temperature, and \( P2 \) and \( T2 \) are the final pressure and temperature.<br /><br />## Step 2<br />In this problem, the initial pressure \( P1 \) is 1.00 atm, the initial temperature \( T1 \) is 293 K, the final temperature \( T2 \) is 303 K, and we are asked to find the final pressure \( P2 \).<br /><br />## Step 3<br />We can rearrange the Gay-Lussac's Law formula to solve for \( P2 \):<br />### \( P2 = P1 \times \frac{T2}{T1} \)<br /><br />## Step 4<br />Substitute the given values into the formula:<br />### \( P2 = 1.00 \, \text{atm} \times \frac{303 \, \text{K}}{293 \, \text{K}} \)<br /><br />## Step 5<br />Calculate the value of \( P2 \), which is approximately 1.03 atm.