Answer:
47.8 moles of H₂O.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
2H₂ + O₂ —> 2H₂O
From the balanced equation above,
1 mole of O₂ reacted to produce 2 moles of H₂O
Finally, we shall determine the number of mole of water, H₂O, produced by the reaction of 23.9 moles of O₂. This can be obtained as follow:
From the balanced equation above,
1 mole of O₂ reacted to produce 2 moles of H₂O.
Therefore, 23.9 moles of O₂ will react to produce = 23.9 × 2 = 47.8 moles of H₂O.
Thus, 47.8 moles of H₂O were obtained from the reaction.
Answer:
P(H₂) = 0.8533 atm
Explanation:
n(CO) = 0.220 mole
n(H₂) = 0.350 mole
n(He) = 0.640 mole
_______________
∑ n = 1.210 moles
mole fraction => X(H₂) = 0.350/1.210 = 0.2892
Dalton's Law of Partial Pressures => P(H₂) = X(H₂)·P(ttl) = 0.2892(2.95 atm) = 0.8533 atm
The answer to your question is,
C. Look over their answers to the lab questions and check for errors.
-Mabel <3
Answer:
The body with 2.7 
has a larger volume
Explanation:
There is a missespelling in the question. The units of density cannot be g, they usually are
In order to answer this question, we need to use the formula of the density of a body:
For body A:
Mass (M) = 5.0 g
Density (D) = 2.7
2.7 = 5g * 1/V
V1 = 5g / (2.7 )
V1 = 1.85 
For Body B:
Mass (M) = 5.0 g
Density (D) = 8.4
8.4 = 5g * 1/V
V2 = 5g / (8.4 )
V2 = 0.59
So V1 is bigger than V2
