A sample of gas at 1015.7 mmHg, occupying a volume of 14.66 L, and at a temperature of 21.31 °C is transferred to a container of 9.78 L with a pressure of 71.36 kPa. What is the new temperature in °C? Provide your answer with TWO decimals.

For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C.   Suppose the temperature of a sample of ammonia gas is raised from −12.0°C to 21.0°C, and at the same time the pressure is changed. If the initial pressure was 2.5atmand the volume decreased by 45.0%, what is the final pressure? Round your answer to the correct number of significant digits.       atm

A gas sample originally occupies 436 mL at 24 °C. When the volume is expanded to 612 mL and the temperature is increased to 97 °C, the pressure becomes 526 mm Hg. What was the original pressure?

Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1100. torr. key carbon hydrogen dlo nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr O2 torr

A mass of 7.16 g carbon monoxide is reacted with 6.84 g hydrogen to form methanol. CO(g) + 2 H₂(g) → CH3OH(g) The reaction is performed in a 5.00 L flask at 85.0 °C and proceeds to completion. What is the partial pressure (in mmHg) of each of the three species following completion of the reaction? What is the total pressure in the flask? mmHg mmHg CO H₂ CH3OH Total Submit Submit Answer mmHg mmHg Show Approach Show Tutor Steps Try Another Version 2 item attempts remaining

For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is lowered from 23.0°C⁢ to −19.0°C, and at the same time the pressure is changed. If the initial pressure was 6.3atm and the volume increased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits.

A 34.0 L metal cylinder stores a sample of gas at 26 °C under 1.42 atm. The temperature of the storage unit rises to 96 °C, causing the gas to decompose and doubling the number of moles in the cylinder.

A gas sample originally was held at a volume of 4.39 L at 42.5 °C and a pressure of 748 torr. In order to reduce its volume to 3.29 L, at constant pressure, this gas must be cooled to °C. Record your answer to the nearest degree Celsius.

A 8.00 L tank at 11.8 °C is filled with 7.85 g of carbon dioxide gas and 3.51 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: 0 x10 carbon dioxide partial pressure: atm mole fraction: 0 boron trifluoride partial pressure: atm Total pressure in tank: atm

A cylinder is filled with 10.0L of gas and a piston is put into it. The initial pressure of the gas is measured to be 281.kPa . The piston is now pushed down, compressing the gas, until the gas has a final volume of 1.90L . Calculate the final pressure of the gas. Be sure your answer has the correct number of significant digits.