Master Boyle's Law Calculations

Boyle's Law: A 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure? Use the equation: $P_1V_1 = P_2V_2$. Insert the values and denote V2 as x: (740.0 mmHg) (2.00 L) = (760.0 mmHg) (x). Multiply the left side and divide (by 760.0 mmHg) to solve for x. V2= ______.

Boyle's Law: A 5.00 L of a gas is at 1.08 atm. What pressure is obtained when the volume is 10.0L? Use the equation: $P_1V_1 = P_2V_2$. Insert the values and denote P2 as x: (1.08 atm) (5.00 L) = (x) (10.0 L). Multiply the left side and divide (by 760.0 mmHg) to solve for x. P2 = ______.

Boyle's Law: A gas sample occupies a volume of 2.5 L at a pressure of 1.5 atm. What would be the volume of the gas if its pressure is reduced to 1 atm at the same temperature? Use the equation: $P_1V_1 = P_2V_2$. Insert the values and denote V2 as x: (1.5 atm) (2.5 L) = (1 atm) (x). Multiply the left side and divide (by 1 atm) to solve for x. V2 = ______.

Boyle's Law: The gas inside a balloon has a volume of 15.0 L at a pressure of 2.0 atm. Calculate the pressure of the gas if its volume is compressed to 10.0 L at the same temperature? Use the equation: $P_1V_1 = P_2V_2$. Insert the values and denote P2 as x: (2.0 atm) (15.0 L) = (x) (10.0 L). Multiply the left side and divide (by 10.0 L) to solve for x. P2 = ______.

Charles' Law: A gas sample has a volume of 2.0 L at a temperature of 25°C. What would be the volume of the gas at 50°C, assuming pressure remains constant? Use the equation: $V_1 / T_1 = V_2 / T_2$. Insert the values and denote V2 as x: (2.0 L) / (25°C + 273) = (x) / (50°C + 273). Multiply the left side and solve for x. V2 = ______.