A sample of hydrogen gas occupies a volume of 8.64 L at 50.0°C and 0.450 atm. If it is desired to decrease the volume of the gas sample to 6.15 L, while increasing its pressure to 0.577 atm, the temperature of the gas sample at the new volume and pressure must be ______ °C.

A sample of methane occupied 18.95 L at 41.03 °C. When the volume changed to 11.60 L at 16.59 °C, the pressure was 2.044 atm. Calculate the original pressure (atm). Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Convert temperature(s) to K, and enter with proper s.f. If the term doesn't apply in this problem enter 0. Enter a question mark for the variable being calculated. Do not leave any blank empty. P1 =  V1 =  T1= n1= P2= V2= T2= n2=   Rearrange the gas law equation needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressures = P1, P2; volumes = V1, V2; temperatures = T1, T2, moles = n1, n2…

You have a 3.00-liter container filled with N₂ at 25 °C and 3.35 atm pressure connected to a 2.00-liter container filled with Ar at 25 °C and 2.75 atm pressure. A stopcock connecting the containers is opened and the gases are allowed to equilibrate between the two containers. What is the final pressure (in atm) in the two containers if the temperature remains at 25 °C? Assume ideal behavior.

A 15.9 mL sample of liquid ethanol (C₂H5OH, density = 0.789 g/mL) was injected into a 10.0 L cylinder containing O₂ at a pressure of 4.50 atm and a temperature of 25 °C. The cylinder was heated to 125 °C and a spark was used to ignite the ethanol, which was completely combusted. What was the final total pressure in the cylinder (in atm) after the reaction, while it was still at 125 °C?

A sample of helium gas occupies a volume of 8.14 L at 57.0°C and 1.09 atm. If it is desired to increase the volume of the gas sample to 10.8 L, while decreasing its pressure to 0.730 atm, the temperature of the gas sample at the new volume and pressure must be (blank) °C.

A quantity of N2 gas originally held at 5.25 atm in a 1.00 L container at 26 °C is transferred to a 12.5 L container at 20 °C. A quantity of O, originally at 5.25 atm and 26 °C in a 5.00 L container is transferred to the same container. What is the total pressure of the mixture in the new container?

The gas in a 1,528 mL balloon at sea level has a pressure of 762 mmHg, and 21.1 ℃. If the balloon rises to an altitude where its pressure is 135 mmHg and its temperature is -22.5 ℃, what is the volume (in L) of the balloon at the higher altitude?

For many purposes we can treat ammonia (NH3). as an ideal gas at temperatures above its boiling point of -33. °C. Suppose the pressure on a 6.0 m³ sample of ammonia gas at -14.0°C is doubled. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. yes no пос x10 X

.) A sample of nitrogen gas initially occupies a volume of 27.5 L at a temperature of 22.5 \deg C and a pressure of 3.25 atm. Calculate the sample's temperature (in \deg C) after the volume of the sample increases to 98.6 L and its pressure decreases to 1.75 atm. 1.

What temperature (in °C) did an ideal gas shift to if it was initially at -15.5 °C at 4.62 atm and 35.0 L and the pressure was changed to 8.31 atm and the volume changed to 25.0 L?