Butane - ethane - methane - propane: What do these hydrocarbons have in common? A) The same number of carbons present. B) They a
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Answer : The partial pressure of at equilibrium are, 1.133, 2.009, 0.574 bar respectively. The total pressure at equilibrium is, 3.716 bar
Solution : Given,
Initial pressure of = 1.42 bar
Initial pressure of = 2.87 bar
= 0.036
The given equilibrium reaction is,
Initially 1.42 2.87 0
At equilibrium (1.42-x) (2.87-3x) 2x
The expression of will be,
Now put all the values of partial pressure, we get
By solving the term x, we get
From the values of 'x' we conclude that, x = 3.889 can not more than initial partial pressures. So, the value of 'x' which is equal to 3.889 is not consider.
Thus, the partial pressure of at equilibrium = 2x = 2 × 0.287 = 0.574 bar
The partial pressure of at equilibrium = (1.42-x) = (1.42-0.287) = 1.133 bar
The partial pressure of at equilibrium = (2.87-3x) = [2.87-3(0.287)] = 2.009 bar
The total pressure at equilibrium = Partial pressure of + Partial pressure of
+ Partial pressure of
The total pressure at equilibrium = 1.133 + 2.009 + 0.574 = 3.716 bar
Given equation :
Given information = 2.47 grams KNO2 and excess KMnO4 and we need to find grams of water (H2O).
Since KMnO4 is in excess, so grams of water(H2O) can be calculated using grams of KNO2 with the help of stoichiometry.
To find grams of water(H2O) from grams of KNO2 , we need to follow three steps.
Step 1. Convert 2.47 grams of KNO2 to moles of KNO2.
Molar mass of KNO2 = 85.10 g/mol
Moles = 0.0290 mol KNO2
Step 2. Convert moles of KNO2 to moles of H2O using mole ratio.
Mole ratio are the coefficient present in front of the compound in the balanced equation.
Mole ratio of KNO2 : H2O is 5 : 3 (5 coefficient of KNO2 and 3 coefficient of H2O)
Mole = 0.0174 mol H2O
Step 3. Convert mole of H2O to grams of H2O
Grams = Moles X molar mass
Molar mass of H2O = 18.00 g/mol
Grams of water = 0.313 grams H2O
Summary : The above three steps can also be done in a singe setup as shown below.
In the above setup similar units get cancelled out and we will get grams of H2O as 0.313 grams water (H2O)
Answer:- 1.90 atm
Solution:- It is based on combined gas law equation, PV = nRT
In this equation, P is pressure, V is volume, n is moles of gas, R is universal gas constant and T is kelvin temperature.
If we divide both sides by V then:
We know that, molarity is moles per liter. So, in the above equation we could replace by molarity, M of the gas. The equation becomes:
P = MRT
T = 20 + 273 = 293 K
M =
Let's plug in the values in the equation:
P =
P = 1.90 atm
So, the pressure of the gas is 1.90 atm.