Answer:
118.776 mmHg
Explanation:
The equation of the reaction is;
C4H10(g) + 13/2 O2(g) ------> 4CO2(g) + 5H20(g)
Now the mole ratio according to the balanced reaction equation is;
1 : 6.5 : 4 : 5
Hence, the total number of moles present = 1 + 6.5 + 4 + 5 = 16.5 moles
Mole fraction of water vapour = 5/16.5 = 0.303
We also know that;
Partial pressure= mole fraction * total pressure
Partial pressure of H20(g) = 0.303 * 392 mmHg = 118.776 mmHg
86 atoms have more electrons than Germanium
Molecular weight of N2
gram Atomic weight of N is 14 g.
gram Molecular weight = 14 g×2
= 28 g
Liter concepts
1 liter of gas always occupies 1 gram molecular weight .
Application of the concept
5.75 liter gives 0.257g
1 mole will occupy 28 g
0.257 will occupy 28 g × 0.257
= 7.196 g
The mass of the gas is 7.196 g.
Hope it helps you
For equal moles of gas, temperature can be calculated from ideal gas equation as follows:
P×V=n×R×T ...... (1)
Initial volume, temperature and pressure of gas is 3.25 L, 297.5 K and 2.4 atm respectively.
2.4 atm ×3.25 L=n×R×297.5 K
Rearranging,
n\times R=0.0262 atm L/K
Similarly at final pressure and volume from equation (1),
1.5 atm ×4.25 L=n×R×T
Putting the value of n×R in above equation,
1.5 atm ×4.25 L=0.0262 (atm L/K)×T
Thus, T=243.32 K
