Charles's Law Calculations 1. A container holds 50 mL of nitrogen at 25^circ C and a pressure of 736 mm Hg. What will be its volume if the temperature increases by 10^circ C i 2. A sample of oxygen occupies a volume of 160cm^3 at 91^circ C What will be the volume of oxygen when the temperature drops to 0^circ C i 3. A sample of hydrogen gas has an initial temperature of 50^circ C When the temperature is lowered to -5^circ C the volume of hydrogen becomes 212cm^3 What was the initial volume of the hydrogen gas? 4. 568cm^3 of chlorine at 25^circ C will occupy what volume at -25^circ C while the pressure remains constant? (V_(1))/(T_(1))=(V_(2))/(T_(2))

1. To solve this problem, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature, provided the pressure and the amount of gas remain constant. The formula for Charles's Law is: where is the initial volume, is the initial temperature, is the final volume, and is the final temperature.Given: We need to find .First, we need to convert the temperatures from Celsius to Kelvin by adding 273.15: Now, we can plug the values into the formula and solve for : Therefore, the volume of nitrogen will be approximately 51.8 mL when the temperature increases by .2. Given: We need to find .First, we need to convert the temperatures from Celsius to Kelvin: Now, we can plug the values into the formula and solve for : Therefore, the volume of oxygen will be approximately 117.6 cm when the temperature drops to .3. Given: We need to find .First, we need to convert the temperatures from Celsius to Kelvin: Now, we can plug the values into the formula and solve for : Therefore, the initial volume of the hydrogen gas was approximately 256.8 cm .4. Given: We need to find .First, we need to convert the temperatures from Celsius to Kelvin: Now, we can