Multiple Choice 20 points A container holds 50.0 ml of nitrogen at 25 degrees Celslus and a pressure of 736 mm Hg what will be its volume if the temperature increases to 60 degrees Celslus? 25.0 mL 55.9 mL 20.8 mL 70.0 mL

To solve this problem, we can use the ideal gas law, which states that the pressure, volume, and temperature of a gas are related by the equation:<br /><br />PV = nRT<br /><br />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 Kelvin.<br /><br />First, we need to convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature:<br /><br />T1 = 25°C + 273.15 = 298.15 K<br />T2 = 60°C + 273.15 = 333.15 K<br /><br />Next, we can use the ideal gas law to find the volume of the gas at the new temperature:<br /><br />V1 = nRT1/P<br />V2 = nRT2/P<br /><br />Since the number of moles and the pressure remain constant, we can simplify the equation to:<br /><br />V1/T1 = V2/T2<br /><br />Substituting the given values, we get:<br /><br />50.0 mL / 298.15 K = V2 / 333.15 K<br /><br />Solving for V2, we get:<br /><br />V2 = 50.0 mL * 333.15 K / 298.15 K = 55.9 mL<br /><br />Therefore, the volume of the gas at 60°C will be 55.9 mL.