Calculate the temperature, in K, of 2.20 moles of gas occupying 4.10 L at 2.82 atm.

64 k

Explanation:

To figure this out you need to start with the ideal gas equation:

P

⋅

V

=

n

⋅

R

⋅

T

You have P (3.30 atm), V (3.5 l), n (2.20 moles) and you can look up the gas constant, R (0.082057 (latm)/(molK)).

We simply rearrange the ideal gas equation to get T by itself:

T

=

P

⋅

V

n

⋅

R

Then simply plug in the values you were given, making sure that the units are in liters, atmospheres, and moles (which they are, in this case):

T

=

3.30

atm

⋅

3.5

l

2.20

moles

⋅

0.082057

(l*atm)/(mol*K)

=

63.9799

K

Since volume was only given to 2 significant figures, we can only report 2 significant figures for our

64 K.

3 hours because it is a decent distance.

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.