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labwork [276]
3 years ago
15

What do the news and science have in common?

Chemistry
1 answer:
Artemon [7]3 years ago
7 0

Answer: B

Drift-net fishing has many effects, and when the net is put in the water, coral reefs and other oceanic/aquatic plants can be destroyed.

The answer to the question is option B.

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Among the following which solution is the most acidic?
Vika [28.1K]

i think it c i dont know if im right tho.

8 0
3 years ago
Compare endothermic and exothermic reactions and give examples of each. In an endothermic reaction would we expect the temperatu
Ivanshal [37]

Exothermic gives off heat/energy and endothermic takes in heat/energy. Exothermic example: a candle flame

Endothermic example: baking bread

In Exothermic, you can expect the surrounding temp. to rise, and in Endothermic you can expect the surrounding temperature to fall.

Hope this helps

3 0
3 years ago
Please help it’s a test due in five minutes! I’ll give 10 points
barxatty [35]

Answer: negative acellaration or mass.

Explanation:

the first reason why is that i got that quistion right. and when objects are unbalanced it gives negative acellaration

3 0
3 years ago
In Part A, we saw that the theoretical yield of aluminum oxide is 0.800 mol . Calculate the percent yield if the actual yield of
MAVERICK [17]
Percent Yield is the actual practical yield of a certain chemical reaction. It is always less than the theoretical yield calculated due to human handling and error.

Percent Yield = (Actual yield / theoretical yiield) * 100 = (0.456 / 0.800) * 100 = 57%

The yield here is small which means a bad handling and high error.
6 0
4 years ago
Read 2 more answers
A vessel of volume 100 cm3 contains 0.25 mol o2 and 0.034 mol co2 at 10.0c. Calculate the partial pressure of each component and
Artyom0805 [142]

Answer: The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.

Explanation:

According to the ideal gas equation:'

PV=nRT

P = Pressure of the gas = ?

V= Volume of the gas = 100cm^3=0.1L 1L=1000cm^3

T= Temperature of the gas = 10°C = 373 K      

R= Gas constant = 0.0821 atmL/K mol

n=  moles of gas= 0.25 +0.034 = 0.284 moles

P=\frac{nRT}{V}=\frac{0.284\times 0.0821\times 373}{0.1}=87atm

x_{O_2} = mole fraction of oxygen=\frac{\text {moles of }O_2}{\text {moles of }O_2+\text{moles of }CO_2}=\frac{0.25}{0.25+0.034}=0.88,  

x_{CO_2} =mole fraction of carbon dioxide=\frac{\text {moles of }CO_2}{\text {moles of }O_2+\text{moles of }CO_2}=\frac{0.034}{0.25+0.034}=0.12

partial pressure of oxygen = p_{O_2}=x_{O_2}\times P=0.88\times 87=76.56atm

partial pressure of carbon dioxide= p_{CO_2}=x_{CO_2}\times P=0.12\times 87=10.44atmatm

The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.

8 0
3 years ago
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