At STP 1 mol of gas occupies 22.4 L. So what we have to do is find the new volume of gas under the conditions you describe.
STP
====
V = 22.4 L
P = 1 Atm
T = 0 + 273 = 273
Given conditions
===========
V1 = ???
P1 = 1.5 atm
T1 = 264 oK
V*P/T = V1*P1/T1
22.4 * 1 / 273 = V1 * 1.5 / 264
V1 = 22.4 * 1 * 264/(273 * 1.5)
V1 = 14.44 L
Now we need to find out the molar mass of H2S
2*1 + 32 = 34
1 mole of H2S has a mass of 34 grams / mol
The density is mass / Volume
d = 34/ 14.44 = 2.35 grams /L
ok jennifer lopez... start with these 2 equations...
(1).. PV = nRT
(2).. n = mass / mw
substitute and rearranging...
PV = (mass / mw) RT
(mass / V) = mw x P / (RT)
since density = mass / V...
density = mw x P / (RT)
solving...
density = (34.08g/mol) x (1.5atm) / ((0.08206 Latm/molK) x (264K))
density = 2.4 g/L
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At STP 1 mol of gas occupies 22.4 L. So what we have to do is find the new volume of gas under the conditions you describe.
STP
====
V = 22.4 L
P = 1 Atm
T = 0 + 273 = 273
Given conditions
===========
V1 = ???
P1 = 1.5 atm
T1 = 264 oK
V*P/T = V1*P1/T1
22.4 * 1 / 273 = V1 * 1.5 / 264
V1 = 22.4 * 1 * 264/(273 * 1.5)
V1 = 14.44 L
Now we need to find out the molar mass of H2S
2*1 + 32 = 34
1 mole of H2S has a mass of 34 grams / mol
The density is mass / Volume
d = 34/ 14.44 = 2.35 grams /L
ok jennifer lopez... start with these 2 equations...
(1).. PV = nRT
(2).. n = mass / mw
substitute and rearranging...
PV = (mass / mw) RT
(mass / V) = mw x P / (RT)
since density = mass / V...
density = mw x P / (RT)
solving...
density = (34.08g/mol) x (1.5atm) / ((0.08206 Latm/molK) x (264K))
density = 2.4 g/L