Calculate the root mean square velocity, in m/s, of Cl₂ at -23.0°C. Assume ideal gas behavior.

Calculate the root mean square (rms) average speed of the atoms in a sample of neon gas at  0.15 atm and  −95.°C. Round your answer to  3 significant digits.

Calculate the root mean square (rms) average speed of the atoms in a sample of xenon gas at  0.13 atm  and −95.°C. Round your answer to  3  significant digits.

Nitrogen gas and hydrogen gas combine to produce ammonia gas (NH3). What volume of hydrogen gas at 25C and 735mm Hg is required for the complete reaction of 10.0g of nitrogen?

Calculate the root-mean-square velocity, in m/s, for a neon atom at 12.1°C. The universal gas constant, R=8.314 J/mol-K.

Consider a sample of nitrogen gas, N2, in which the constituent molecules have a root-mean-square speed of 690 m/s. The atomic mass of N is 14 u. What is the temperature of the gas?

A 2.39 L volume of hydrogen measured at −154°C is warmed to 100.°C. Calculate the volume (in L) of the gas at the higher temperature, assuming no change in pressure.

Determine the root mean square velocity of chlorine molecules at 25.0 C in m/s.