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2 years ago

How exactly are synthetic paint brushes made? Nylon?

Chemistry

1 answer:

oksian1 [2.3K]2 years ago

6 0

Answer:

<h2>Synthetic brushes <em>are typically made from nylon bristles. Other times, they're made </em><em>from </em><em>plastic</em></h2><h3 /><h3 /><h3>#CARRYONLEARNING</h3>

BY : <em>EDLYN MORENO</em>

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Balance the equation<br> N2O5 + H2 -> NH3 + H2O

Lubov Fominskaja [6]

Answer:

I hope this is it. I'm not really sure.

4 0

3 years ago

Why is a typical car battery in a car is filled with a solution of sulferic acid

Lesechka [4]

Answer:

Sulfuric acid has a higher density than water, which causes the acid formed at the plates during charging to flow downward and collect at the bottom of the battery.

8 0

3 years ago

A chef fills a 100 ml container with 76.5 g of cooking oil. What is the density of the oil? \

Feliz [49]

Formula for density is mass / volume.

100 ml is volume. 76.5g of cooking oil is
the mass.

Therefore

76.5/100 = .765g/ml

7 0

3 years ago

In the chemical reaction, how many grams of nitrogen are needed to completely react with 24.3 grams of hydrogen

vlabodo [156]

Answer:

112.540 gram of N2

Explanation:

From the balanced chemical equation

N2+3H2----->2NH3

It means that 1 mole of Nitrogen needs 3 moles of hydrogen

In term of mass,we can say that

6.048 gram of H2 needs 28.01 gram of N2

or, 1 gram of H2 needs (28.01/6.048) gram of N2

and 24.3gram of H2 needs (24.3*28.01/6.048) gram of N2

=112.540 gram of N2

5 0

3 years ago

If 4.00 moles of gasoline are burned according to the chemical

denis23 [38]

Answer: The volume of oxygen at STP is needed for complete given combustion is 1121.28 L.

Explanation:

The given reaction equation is as follows.

$2C_{2}H_{18}(l) + 25O_{2}(g) \rightarrow 16CO_{2}(g) + 18H_{2}O(g)$

This shows that 2 moles of gasoline requires 25 moles of . Hence, moles of oxygen required to react with 4 moles of gasoline are calculated as follows.

$\frac{25 mol O_{2}}{2 mol C_{2}H_{18}} \times 4 mol C_{2}H_{18}\\= 50 mol O_{2}$

At STP, the pressure is 1 atm and temperature is 273.15 K. Therefore, using ideal gas equation the volume of oxygen is calculated.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$PV = nRT\\1 atm \times V = 50 mol \times 0.0821 L atm/mol K \times 273.15 K\\V = 1121.28 L$

Thus, we can conclude that volume of oxygen at STP is needed for complete given combustion is 1121.28 L.

6 0

2 years ago