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Anna11 [10]
3 years ago
8

Name three of the most sensitive parts of your body (Appropriate parts. Ex: finger, wrist, shoulder, etc.)

Chemistry
1 answer:
yKpoI14uk [10]3 years ago
3 0
Inner thigh, eyes, brain
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How many liters of hydrogen gas is formed from the complete reaction of 15.9 g c? assume that the hydrogen gas is collected at a
ololo11 [35]
C + H2O -> H2 + CO
n(C) = 15.9/12 = 1.325 (mol)
=> n(H2) = 1.325 mol
We have:
PV = nRT
=> V = (nRT)/P
(R = 22.4/273 = 0.082)
V = (1.325 x 0.082 x 360)/1 = 39.114 (L)
7 0
3 years ago
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Which model of an atom is correctly labeled?
Andreas93 [3]

Answer:

B

DUH

The nucleus is made up of the protons (which have a positive charge) and neutrons and surrounded by a cloud of electrons ( which have a negative charge ).

8 0
3 years ago
Differences and similarities between Clastic, Chemical, and Organic sedimentary rock.
8090 [49]
Clastic are made from small pieces of other rocks, sedimentary rocks.
Chemical are formed when minerals becomes undersaturated, precipitate forming a limestone.
organic sedimentary rock are made of fossils
 
7 0
2 years ago
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What is the mass of 8.12 × 1023 molecules of CO2 gas? (Atomic mass of carbon = 12.011 u; oxygen = 15.999 u.)
Elza [17]

Answer:

8306.76

Explanation:

you just calcuate 8.12 x 1023 and that will give you the answer

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6 0
3 years ago
You are a NASCAR pit crew member. Your employer is leading the race with 20 laps to go. He just finished a pit stop and has 5.0
jek_recluse [69]

Answer:

Since there are 3500 g of fuel left in the tank, and he needs only 1687.5 g to complete 20 laps, he has enough fuel to complete the race. I will tell the driver that he does not need to make another pit stop as he has enough fuel to complete the race.

Explanation:

Density = mass / volume

Density of fuel = 700 g/ 1 gal

Therefore, the mass of fuel in 1 gallon = 700 g

The driver has 5.0 gallons of fuel in the tank.

The mass of 5.0 gallons of fuel = 5 × 700 = 3500 g of fuel

Equation of the combustion of fuel, C₅H₁₂ is given below:

C₅H₁₂ + 8 O₂ ---> 6 H₂O + 5 CO₂

1 mole C₅H₁₂ requires 8 moles of O₂

1 mole of C₅H₁₂ has a mass = 72 g

8 moles of O₂ has a mass = 256 g

Therefore, 300 g of O₂ will require 300 × (72/256) g of C₅H₁₂ = 84.375 g of C₅H₁₂

84.375 g of fuel is used by the car per lap;

20 laps will require 20 × 84.375 g of fuel = 1687.5 g of fuel.

Since there are 3500 g of fuel left in the tank, and he needs only 1687.5 g to complete 20 laps, he has enough fuel to complete the race. I will tell the driver that he does not need to make another pit stop as he has enough fuel to complete the race.

7 0
3 years ago
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