A sample of gas is at STP and occupies 37.2 mL. If the temperature is increased to 32.0^circ C and the entire sample is transferred to a 14.1 mL container, what will be the gas pressure (in atm) inside the container? square disappointed Formula 1 point

To solve this problem, we can use the ideal gas law equation:<br /><br />PV = nRT<br /><br />Where:<br />P = pressure<br />V = volume<br />n = number of moles<br />R = ideal gas constant<br />T = temperature<br /><br />Given information:<br />- Initial volume (V1) = 37.2 mL<br />- Initial temperature (T1) = 0°C (STP)<br />- Final volume (V2) = 14.1 mL<br />- Final temperature (T2) = 32.0°C<br /><br />Step 1: Convert the temperatures to Kelvin.<br />T1 = 0°C + 273.15 = 273.15 K<br />T2 = 32.0°C + 273.15 = 305.15 K<br /><br />Step 2: Use the ideal gas law equation to find the initial number of moles (n1).<br />PV = nRT<br />n1 = (P1V1) / (RT1)<br />n1 = (1 atm × 37.2 mL) / (0.0821 L·atm/mol·K × 273.15 K)<br />n1 = 1.56 mol<br /><br />Step 3: Use the ideal gas law equation to find the final pressure (P2).<br />PV = nRT<br />P2 = (nRT2) / V2<br />P2 = (1.56 mol × 0.0821 L·atm/mol·K × 305.15 K) / 14.1 mL<br />P2 = 2.34 atm<br /><br />Therefore, the gas pressure inside the 14.1 mL container at 32.0°C will be 2.34 atm.