<u>Answer:</u> The partial pressure of oxygen is 160 mmHg
<u>Explanation:</u>
We are given:
Percent of oxygen in air = 21 %
Mole fraction of oxygen in air = 
To calculate the partial pressure of oxygen, we use the equation given by Raoult's law, which is:

where,
= partial pressure of oxygen = ?
= total pressure of air = 760 mmHg
= mole fraction of oxygen = 0.21
Putting values in above equation, we get:

Hence, the partial pressure of oxygen is 160 mmHg
Answer:
A)P5010
Explanation:
Penta- means 5 and deca/deco- means 10
ANSWER: C. Simple machine
Balanced equation is
HBr + NaOH ----> NaBr + H2O
Using molar masses
80.912 g HBr reacts with 39.997 g of Naoh to give 18.007 g water
so 1 gram of NaOH reacts with 2.023 g of HBR
and 5.7 reacts with 11.531 g HBr so we have excess HBr in this reaction
Mass of water produced = (5.7 * 18.007 / 39.997 = 2.6 g to 2 sig figs