11.48-gram of
are needed to produce 6.75 Liters of
gas measured at 1.3 atm pressure and 298 K
<h3>What is an ideal gas equation?</h3>
The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
First, calculate the moles of the gas using the gas law,
PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.
Given data:
P= 1.3 atm
V= 6.75 Liters
n=?
R= 
T=298 K
Putting value in the given equation:


Moles = 0.3588 moles
Now,


Mass= 11.48 gram
Hence, 11.48-gram of
are needed to produce 6.75 Liters of
gas measured at 1.3 atm pressure and 298 K
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The system is not at equilibrium.
The reaction will proceed to the right to attain the equilibrium.
Let's consider the following reaction.
2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)
The pressure equilibrium constant (Kp) is 60.6. To determine if the system is at equilibrium when the pressure of each component is 1.75 atm, we have to calculate the reaction quotient (Q) and compare it with Kp.
Q = [NO]².[Br₂] / [NOBr]²
Q = (1.75)².(1.75) / (1.75)²
Q = 1.75
Since Q ≠ Kp, the system is not at equilibrium.
Since Q < Kp, the reaction will proceed to the right to attain the equilibrium.
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1. 80 Kj
2. 120-80= 40 Kj
3. 120-20= 100Kj
4. 20-80= -60Kj
5. +60 Kj
6. Exothermic because 4 is negative
<u>Answer:</u> The mass of the nitrous oxide gas produced is 0.011 kg.
<u>Explanation:</u>
To calculate the mass of the gas, we use the formula:

We are given:
Specific density of the gas = 
Mass of the gas = ? kg
Volume of the gas =
(Conversion Factor:
)
Putting values in above equation, we get:


Hence, the mass of the nitrous oxide gas produced is 0.011 kg.