Question

Compute the root-mean-square speed of a nitrogen molecule at 23.6°C. The molar mass of nitrogen molecules...

Compute the root-mean-square speed of a nitrogen molecule at 23.6°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3 kg/mol. At what temperatures will the root-mean-square speed be (b) 1/4 times that value and (c) 4 times that value?

Homework Answers

Answer #2

T = 273 + 23.6 = 296.6 K

M = 28x10^-3 kg/mol

Vrms = = 514 m/s

b)

As V is proportional to square root of absolute temperature, it will be 1/4th if temperature is made 1/16th

T2 = 296.6/16 = 18.53 K

c)

It will be 4 times if temp is made 16 times

T3 = 296.6 x16 = 4745.6 K

answered by: anonymous
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Compute the root-mean-square speed of a nitrogen molecule at 60.1°C. The molar mass of nitrogen molecules...
Compute the root-mean-square speed of a nitrogen molecule at 60.1°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3 kg/mol. At what temperatures will the root-mean-square speed be (b) 1/3 times that value and (c) 4 times that value?
(a) Compute the root-mean-square speed of a nitrogen molecule at 99.1°C. The molar mass of nitrogen...
(a) Compute the root-mean-square speed of a nitrogen molecule at 99.1°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3 kg/mol. At what temperatures will the root-mean-square speed be (b) 1/3 times that value and (c) 2 times that value?
Compute the root-mean-square speed of He molecules in a sample of helium gas at a temperature...
Compute the root-mean-square speed of He molecules in a sample of helium gas at a temperature of 168°C. Compute the root-mean-square speed of N2 molecules in a sample of nitrogen gas at a temperature of 28°C. Arrange the following molecules in order of increasing average molecular speed. All are at the same temperature. methane, argon, sulfur dioxide, neon Enter formulas in the boxes below: 1 = slowest, 4 = fastest Arrange the following molecules in order of increasing average molecular...
Calculate the most probable speed, average speed, and root mean square speed of oxygen gas molecules....
Calculate the most probable speed, average speed, and root mean square speed of oxygen gas molecules. Molar mass of oxygen is 0.032 kg/mol.
Consider a gas of nitrogen molecules at 20°C with a particle density of 2.7 ×1019 molecules/cm3....
Consider a gas of nitrogen molecules at 20°C with a particle density of 2.7 ×1019 molecules/cm3. The molar mass of nitrogen molecules is 28 g/mol.(a) What is the rms speed of the nitrogen molecules?(b) At what temperature will the rms speed be half that value?(c) What is the average translational kinetic energy of these molecules at 20°C? (d) The mean free path of the nitrogen molecules is 0.80×10−5 cm. What is the molecular radius of a nitrogen molecule?
The root mean square speed of O2 molecules at 29°C is about 0.485 km/s. What is...
The root mean square speed of O2 molecules at 29°C is about 0.485 km/s. What is the root mean square speed (in km/s) of a H2 molecule at 29°C? ____km/s
Q26. At what temperature does the root-mean-square speed of H2 equal the escape speed from the...
Q26. At what temperature does the root-mean-square speed of H2 equal the escape speed from the Moon? The mass of H2 molecule is 3.32x10-27kg. (A) -30°C (B) 28°C (C) 179°C (D) 450°C (E) 1027°C Q27. A container holds a mixture of 1 mol of monoatomic gas and 2 mol of diatomic gas at room temperature. What is the molar specific heat of the mixture? (A) 12.5 J/mol×K (B) 18.0 J/mol×K (C) 20.8 J/mol×K (D) 23.5 J/mol×K (E) 29.1 J/mol×K
The rms (root-mean-square) speed of a diatomic hydrogen molecule at 50∘C is 2000 m/s. Note that...
The rms (root-mean-square) speed of a diatomic hydrogen molecule at 50∘C is 2000 m/s. Note that 1.0 mol of diatomic hydrogen at 50∘C has a total translational kinetic energy of 4000 J. Part B The total translational kinetic energy of 1.0 mole of diatomic oxygen at 50∘C is: Choose the correct total translational kinetic energy. View Available Hint(s) Choose the correct total translational kinetic energy. (16)(4000J)=64000J (4)(4000J)=16000J 4000J (14)(4000J)=1000J (116)(4000J)=150J none of the above Part C The temperature of the...
1(a) Effusion refers to the process that gas molecules are escaped from a container through a...
1(a) Effusion refers to the process that gas molecules are escaped from a container through a small pin hole. The rate of escape is determined by their root-room-square speed urms. Effusion is used enrich radioactive uranium 235U from the non-radioactive 238U element. Explain how this is possible. (b) If the rate of effusion of A is four times the rate of B, how does the molar mass of A related to molar mass B? (c ) If an unknown gas...
According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the...
According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be the highest at 200C? A) Cl2 B) H2O C) SF6 D) HCl E) None. The molecules of all gases have the same root-mean-square speed at any given temperature