Consider equimolar samples of different ideal gases at the same volume and temperature. Gas A has a higher molar mass than gas B. 1. Compare the pressure
a. A > B
b. A= B
c. A < B

2. Compare the speed.

a. A > B
b. A= B
c. A < B

I don't understand the question

Explanation:

1. c

2. c

1. b. A = B

2. c. A < B

Explanation:

Consider equimolar samples of different ideal gases at the same volume and temperature. (nA = nB)

Gas A has a higher molar mass than gas B. (MA > MB)

1. We can calculate the pressure using the ideal gas equation.

P = n × R × T / V

Since n, T and V are equal, the pressure of both gases are equal as well.

2. We can calculate the root-mean-square of the velocity using the following expression.

v(rms) = √(3RT/M)

There is an inverse relationship between speed and molar mass. Since A has a higher molar mass, it has a lower speed.

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.