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 correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)