A student wanted to check if the volume of a gas would double after doubling its temperature in °C at constant pressure. A 10.0 L volume of methane gas, CH4, was heated from 25°C to 50°C at constant pressure. What is the final volume of the gas?

If the temperature of a 11.0 mL sample of N₂ gas is increased from 25.0 °C to 75.0 °C as its pressure remains constant, what will be its new volume in milliliters?

A hot air balloon is filled with 1.23 × 10° L of an ideal gas on a cool morning (11 °C). The air is heated to 111 °C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. volume: L

A sample of carbon dioxide gas at a pressure of 1.17 atm and a temperature of 27.4 °C, occupies a volume of 621 mL. If the gas is allowed to expand at constant temperature until its pressure is 0.771 atm, the volume of the gas sample will be ____mL?   A sample of argon gas at a pressure of 0.866 atm and a temperature of 30.0 °C, occupies a volume of 852 mL. If the gas is allowed to expand at constant temperature until its pressure is 0.603 atm, the volume of the gas sample will be _____mL?

5) Consider the reaction below. Co(g) + 2H¿(g) → CH,OH(g) 1.5 L of hydrogen gas and 3.5 L of carbon monoxide gas, both at 45 °C and 1.28 atm are in separate containers separated by a value. When the value is opened the two gases mix and react, according to the above reaction. a) Please determine the limiting reagent and the theoretical yield. b) If the percent yield is 67.3%, what is the concentration of the product in the final reaction mixture? c) What is the partial pressure of the product in the final reaction mixture?

A mixture of neon and methane gases at a total pressure of 882 mm Hg contains neon at a partial pressure of 420 mm Hg. If the gas mixture contains 3.60 grams of neon, how many grams of methane are present?g CH4

A prototype sports ball for a new game is precisely inflated to a pressure of 7.3 psi at 25 degrees C. The ball is spherical with an inner bladder diameter of 22.8 cm. It is filled with air (Mw=28.97 g/mol). Not Avogadro’s number is 6.022 x 10^23 atom/mol. A. Calculate the number of moles of air in the ball at the specified temperature and pressure. Consider the air in the ball to follow the ideal gas law. PV=nRT   Where P is the absolute pressure of the air in atm, V is the volume of the ball, T is the absolute temperature in K, and R is the ideal gas constant.   B. How many oxygen atoms compose the air in the ball? Assume that the mole fraction of N2 in the air is 0.79 and the remainder of the air is 02(oxygen).

2a

For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of -196. °C. Suppose the temperature of a sample of nitrogen gas is raised from -20.0 °C to 12.0 °C, and at the same time the pressure is changed. If the initial pressure was 3.0 atm and the volume decreased by 60.0%, what is the final pressure? Round your answer to the correct number of significant digits. atm 0 x5 ? D Submit Assignment Continue 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Terms of Use | Privacy Center | Accessibility 9:27 AM 75°F Cloudy ^ ADE40 5/23/202 Bi insert delete home end prt sc esc Type here to search 1 F2 @ 2 F3 # 3 F4 $ 4 D F5 % 5 O F6 T A 6 ** F7 Y 8 & 7 F8 U * 8 F9 F10 9 ) U P

A hot air balloon is filled with 1.39 × 10° L of an ideal gas on a cool morning (11 °C). The air is heated to 113 °C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. volume: L