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.

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

what are the statements