Answer:
Explanation:
Considering,
Using ideal gas equation as:
where,
P is the pressure = 760 mmHg
V is the volume = 100.0 mL = 0.1 L
m is the mass of the gas = 0.193 g
M is the molar mass of the gas = ?
Temperature = 17 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (17 + 273.15) K = 290.15 K
R is Gas constant having value = 62.36367 L. mmHg/K. mol
Applying the values as:-
M = 45.95 g/mol
This mass corresponds to . Hence, the gas must be
.
<u>Answer:</u> The value of for the given chemical equation is 0.0457.
<u>Explanation:</u>
Given values:
Initial moles of = 0.700 moles
Volume of conatiner = 3.50 L
The given chemical equation follows:
I: 0.700
C: -2x +2x x
E: 0.700-2x 2x x
Equilibrium moles of = x = 0.180 moles
Equilibrium moles of = 2x =
Equilibrium moles of = 0.700 - 2x =
Molarity is calculated by using the equation:
So,
The expression of for above equation follows:
Plugging values in above expression:
Hence, the value of for the given chemical equation is 0.0457.