<span>Boyles law states that the volume of a gas is proportional to the moles of the gas when pressure and temperature are kept constant. </span>
Answer: (a) There are 0.428 moles present in 12 g of molecule.
(b) There are 2 moles present in particles of oxygen.
Explanation:
(a). The mass of nitrogen molecule is given as 12 g.
As the molar mass of is 28 g/mol so its number of moles are calculated as follows.
So, there are 0.428 moles present in 12 g of molecule.
(b). According to the mole concept, 1 mole of every substance contains atoms.
Therefore, moles present in particles are calculated as follows.
So, there are 2 moles present in particles of oxygen.
Answer:
Option A. It has stayed the same.
Explanation:
To answer the question given above, we assumed:
Initial volume (V₁) = V
Initial temperature (T₁) = T
Initial pressure (P₁) = P
From the question given above, the following data were:
Final volume (V₂) = 2V
Final temperature (T₂) = 2T
Final pressure (P₂) =?
The final pressure of the gas can be obtained as follow:
P₁V₁/T₁ = P₂V₂/T₂
PV/T = P₂ × 2V / 2T
Cross multiply
P₂ × 2V × T = PV × 2T
Divide both side by 2V × T
P₂ = PV × 2T / 2V × T
P₂ = P
Thus, the final pressure is the same as the initial pressure.
Option A gives the correct answer to the question.
Answer:
Kc = [CH₄] / [H₂]²
Kp = [CH₄] / [H₂]² * (0.082*T)^-1
Explanation:
Equilibrium constant, Kc, is defined as the ratio of the concentrations of the products over the reactants. Also, each concentration of product of reactant is powered to its coefficient.
<em>Pure solids and liquids are not taken into account in an equilibrium</em>
Thus, for the reaction:
C(s)+ 2H₂(g) ⇌ CH₄(g)
Equilibrium constant is:
<h3>Kc = [CH₄] / [H₂]²</h3>
Now, using the formula:
Kp = Kc* (RT)^Δn
<em>Where R is gas constant (0.082atmL/molK), T is the temperature of the reaction and Δn is difference in coefficients of gas products - coefficients of gas reactants (1 - 2= -1)</em>
Replacing:
<h3>Kp = [CH₄] / [H₂]² * (0.082*T)^-1</h3>
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