if there are 6.25 L of Hydrogen gas at a pressure of 1.95 ATM and a temperature of 243 K, how many grams of hy

Question

5.If there are 6.25 L of Hydrogen gas at a pressure of 1.95 ATM and a temperature of 243 K, how many grams of hydrogen are there?

Answer 1

Hi:
U have to use the universal gas law which is:pv=nRT
where: p=pressure
v-volume
R= 8.31J/mole/K(universal) or
R=0.8214
T= temperature
n= number of moles

U have only one unknown in this equation ater you find n slove for mass using this equation:
mass= rmm * moles

so we have:
Step one: pv=nRT
P=1.95,V=6.25,R=0.8214,T=243K

pv=nRT
Substituting the above values solve for n:

Step two : take the value of n and find the mass of hydrogen you need!
MASS=MOLES * RMM
MOLES =X(u found in step one)
RMM OF HYDROGEN= CHECK A PERIODIC TABLE
MULTIPLY IT
AND UR PROBLEM IS SLOVE
lOVE sanam

Answer 2

PV = nRT
P = pressure
V = Volume
n = number of moles
R = constant = .08214
T = temperature in Kelvin

solve for n and multiply it by atomic mass of Hydrogen. Then do your own homework.