<u>Answer: </u>The mass of water produced is 44.28 g
<u>Explanation:</u>
We are given:
Volume of oxygen gas = 27.50 L
At STP conditions:
22.4 L of volume is occupied by 1 mole of a substance
27.50 L of oxygen gas will be occupied by = 
The chemical equation for the formation of water follows:
By the stoichiometry of the reaction:
If 1 mole of oxygen gas produces 2 moles of water
So, 1.23 moles of oxygen gas will produce = 
of water
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
......(1)
Molar mass of water = 18 g/mol
Plugging values in equation 1:
Hence, the mass of water produced is 44.28 g
Answer: The answer would be B. 171 square feet
Explanation:
I took the test and got it right / Hope it helps!:)
The new volume of the bag : 747.43 ml
<h3>Further explanation</h3>
Charles's Law
When the gas pressure is kept constant, the gas volume is proportional to the temperature
V₁=250 ml
T₁=19+273=292 K
T₂=600+273=873 K
Answer:
the equilibrium partial pressure of BrCl is pBC = 784.52 torr
Explanation:
Since
Br₂(g) + Cl₂(g) ⇌ 2BrCl(g) , Kp=1.112 at 150 K
denoting BC as BrCl , B as Br₂ , C as Cl₂, p as partial pressure , then
Kp = pBC²/[pB*pC]
solving for pBC
pBC = √(Kp*pB*pC)
replacing values
pBC = √(Kp*pB*pC) = √(1.112*751 torr*737 torr) = 784.52 torr
pBC = 784.52 torr
then the equilibrium partial pressure of BrCl is pBC = 784.52 torr
