What is the pressure of 0.500mol of gas at 12.2 L and 273K

P = 0.92 atm

Explanation:

Given data:

Pressure of gas = ?

Number of moles = 0.500 mol

Volume of gas = 12.2 L

Temperature of gas = 273 K

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will put the values.

P = nRT/v

P = 0.500 mol × 0.0821 atm.L/ mol.K   ×273 K/ 12.2 L

P = 11.2 /12.2 L

P = 0.92 atm

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.

i just learnt this recently but i need to look through my notes again