Answer : The volume of the balloon at the new location is, 591.3 L
Explanation :
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
where,
= initial pressure of gas = 0.995 atm
= final pressure of gas = 0.720 atm
= initial volume of gas = 500 L
= final volume of gas = ?
= initial temperature of gas = 
= final temperature of gas = 
Now put all the given values in the above equation, we get:
Therefore, the volume of the balloon at the new location is, 591.3 L
Answer:
The reaction is not at the equilibrium, we have more products than reactants.
Explanation:
Step 1: Data given
Temperature = 400 °C
When Q=K, this means the system is at equilibrium. There will not be a shift to either the left or the right.
When Q<K,it means we have more reactants than products. The system will, as reaction, make more products, this will cause the equilibrium to move to the right.
When Q>K,it means we have more products than reactants. The system will, as reaction, make less products and more reactants, this will cause the equilibrium to move to the left.
[NO] = 0.01 M
[N2] = 0.001 M
[O2] = 0.001 M
Kc = 0.0156
Step 2: The balanced equation
N2 (g) + O2 (g) ⇆ 2NO (g) + Cl2 (g)
Step 3: Calculate Q
Q = [NO]²/[N2][O2]
Q = 0.01²/(0.01*0.001)
Q = 10
Q>>Kc
This means we have more products than reactants. The system will, as reaction, make less products and more reactants, this will cause the equilibrium to move to the left.
The reaction is not at the equilibrium, we have more products than reactants.
Answer:
grams O₂ = 134 grams
Explanation:
PV = nRT => n = PV/RT
P = 8.15atm
V = 12.2 Liters
R = 0.08206L·atm/mol·K
T = 16.0°C + 273 = 289K
n = (8.15atm)(12.2L)/(0.08206L·atm/mol·K)(289K) = 4.2 moles O₂
grams O₂ = 4.2 moles O₂ x 32g/mol = 134 grams O₂
Answer:
101.56 of H₂O
Explanation:
The balanced equation for the reaction is given below:
CH₄ + 2O₂ —> CO₂ + 2H₂O
Next, we shall determine the mass of CH₄ that reacted and the mass of H₂O produced from the balanced equation. This is illustrated below:
Molar mass of CH₄ = 12 + (4×1.01)
= 12 + 4.04
= 16.04 g/mol
Mass of CH₄ from the balanced equation = 1 × 16.04 = 16.04 g
Molar mass of H₂O = (2×1.01) + 16
= 2.02 + 16
= 18.02 g/mol
Mass of H₂O from the balanced equation = 2 × 18.02 = 36.04g
SUMMARY:
From the balanced equation above,
16.04 g of CH₄ reacted to produce 36.04 g of H₂O.
Finally, we shall determine the mass of water, H₂O produced by the reaction of 45.2 g of methane, CH₄. This can be obtained as illustrated below:
From the balanced equation above,
16.04 g of CH₄ reacted to produce 36.04 g of H₂O.
Therefore 45.2 g of CH₄ will react to produce = (45.2 × 36.04)/16.04 = 101.56 g of H₂O.
Thus, 101.56 of H₂O were obtained.
