A chemical process occurs at constant temperature and pressure within the cylinder. Reaction 8.0 L 4.0 L

A Moving to another question will save this response. Question 6 "Calculate the total pressure of mixture of 1.32g of nitrogen gas, 1.33g of hydrogen gas, and 1.66g of chloring gas mixed in a sealed 4.8L container at 17.1°C"

Use ideal gas law

Calculate the number of molecules of an ideal gas in a 8.2 Liter of a container at -73°C and 0.50 atm.     0.25     1.5 x 1023     -4.1 x 1023     7.5 x 1023     4.2 x 10-25

A mixture contains 5.00 g each of N2, O2, CO2 and Ne gases. Calculate the volume of this mixture at STP. Calculate the partial pressure of each gas in the mixture at STP.

To determine the molecular weight of an unknown chlorate. a sample of the chlorate was decomposed by heating and the oxygen gas produced was collected over water.563mL of oxygen were collected. The gas collected and the water were both at a temperature of 24°C. The total pressure of the room was 0.996 atm. If the vapor pressure of water at 24°C is 25.8 torr, howmany moles of gas were collected?R = 0.08206* L*atm/ mol*K

what is the easiest procedure?

A 3.0L sample of gas at 1.0 atm and 0.0℃ is heated to 85℃. Calculate the final volume. The pressure remains constant.

using Ideal gas law. volume =) TOL Temperature => 273k Pressure = 1 atm moles =>> ?

For the following set of pressure/volume data, calculate the new volume of the gas sample after the pressure change is made. Assume that the temperature and the amount of gas remain constant. V = 115 mL at 738 mm Hg %3D V = ? mL at 781 mm Hg Volume mL %3D