Answer : The correct option is, 13.7 mole
Solution : Given,
Moles of = 27.4 moles
The given balanced chemical reaction is,
From the balanced chemical reaction, we conclude that
As, 2 moles of react with 1 moles of
So, 27.4 moles of react with
moles of
Therefore, the number of moles of oxygen required are, 13.7 moles
The equilibrium constant for the reaction is 0.00662
Explanation:
The balanced chemical equation is :
2NO2(g)⇌2NO(g)+O2(g
At t=t 1-2x ⇔ 2x + x moles
The ideal gas law equation will be used here
PV=nRT
here n= =
= density
P = density is 0.525g/L, temperature= 608.15 K, P = 0.750 atm
putting the values in reaction
0.75 =
M = 34.61
to calculate the Kc
Kc=
x M NO2 +
M NO+
M O2
Putting the values as molecular weight of NO2, NO,O2
34.61=
x= 0.33
Kc=
putting the values in the above equation
Kc = 0.00662
Answer : 50.69 mg of ascorbic acid does not meet the daily requirement.
Solution : Given,
Molar mass of Ascorbic acid = 176 g/mole
Moles of Ascorbic acid =
Formula used :
or,
Now put all the given values in this formula, we get the mass of ascorbic acid.
Conversion :
As per question, a healthy adult’s daily requirement of vitamin C is 70-90 mg. But calculate mass of vitamin C is 50.69 mg. So, 50.69 mg of ascorbic acid does not meet the daily requirement.
Answer:
a)
b)
Explanation:
Equation of reaction:
Initial pressure 3 1 0
Pressure change 2P 1P 2P
Total pressure = (3-2P) + (1-P) + (2P)
Total Pressure = 3.75 atm
(3-2P) + (1-P) + (2P) = 3.75
4 - P = 3.75
P = 4 - 3.75
P = 0.25 atm
Let us calculate the pressure of each of the components of the reaction:
Pressure of XO2 = 3 - 2P = 3 - 2(0.25)
Pressure of XO2 =2.5 atm
Pressure of O2 = 1 - P = 1 -0.25
Pressure of O2 = 0.75 atm
Pressure of XO3 = 2P = 2 * 0.25
Pressure of XO3 = 0.5 atm
From the reaction, equilibrium constant can be calculated using the formula:
Standard free energy:
b) value of k−1 at 27 °C, i.e. 300K