Which of the following statements is false? an increase in temperature will
a. increase the molecular weight of the gas.
b. increase the velocity of the gas molecules.
c. increase the number of collisions per second.
d. increase the average kinetic energy of the molecules.
e. increase the root-mean-square velocity of the molecules.

- what is the order of increasing rate of effusion for the following gases? ar, co2, he, n2

- place the following gases in order of increasing speed at the same temperature. n2, h2, cl2, co2, ar

the false statements are a, and e (not sure about e but think a is false)

P=4184.36 torr

Explanation:

For this problem we can use the idea gas law,

where P is pressure, V is volume, n is moles of substance, R is the constant, and T is temperature, We will need to manipulate it and a couple values so that we can get our answer in torr. To do this, let's rearrange the equation to solve for P.

Next, let's convert T (32) to kelvin. To do this, add 273 to the value.

Next, let's convert 28g of N2 to moles of N2. To do this, divide 28 by the molar mass of N2 (28.02)

moles of N2

Next, we need to find out what value of R we need to use. Because you want your answer in torr, we will need to use the value of

Now that we have all of our values, let's plug them into the equation (I'll be excluding units for simplicity but they cancel out to leave units of torr in the answer)

P=4184.36 torr

Very briefly, I don't know what your periodic table looks like, but mine has nitrogen's molar mass as 14.01. If you have a different mass of nitrogen, this pretty drastically impacts the value. For example, if your nitrogen's molar mass was rounded to 14.0 (making N2 28g) then it would be one mole instead of .99 moles, raising the answer to 4228.70 torr. If you have any different values just plug them in in their proper spots. A similar concept applies to the Kelvin conversion.