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zhuklara [117]
3 years ago
15

What is the oxidation number for each atom in NH4CI?

Chemistry
1 answer:
Alika [10]3 years ago
5 0
<span>N = +3, H = +1 ,Cl = -1
</span><span>

</span>
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What is c4???????<br><br> will give brainliest if right
Lena [83]

C-4 or Composition C-4 is a common variety of the plastic explosive family known as Composition C, which uses RDX as its explosive agent. C-4 is composed of explosives, plastic binder, plasticizer to make it malleable, and usually a marker or odorizing taggant chemical.

Or

The explosive material in C-4 is cyclotrimethylene-trinitramine (C3H6N6O6), commonly called RDX (which stands for "royal demolition explosive" or "research development explosive").

5 0
3 years ago
1. A gas has a pressure of 799.0 mm Hg at 50.0 degrees C. What is the temperature at standard Pressure?
larisa [96]

Answer:

A = 674.33mmHg

B = 0.385atm

Explanation:

Both question A and B requires the application of pressure law which states that the pressure of a fixed mass of gas is directly proportional to its temperature provided that volume is kept constant.

Mathematically,

P = kT, k = P / T

P1 / T1 = P2 / T2 = P3 / T3 =.......= Pn/Tn

A)

Data:

P1 = 799mmHg

T1 = 50°C = (50 + 273.15) = 323.15K

P2 = ?

T2 = 273.15K

P1 / T1 = P2 / T2

Solve for P2

P2 = (P1 × T2) / T1

P2 = (799 × 273.15) / 323.15

P2 = 674.37mmHg

The final pressure is 674.37mmHg

B)

P1 = 0.470atm

T1 = 60°C = (60 + 273.15)K = 333.15K

P2 = ?

T2 = 273.15K

P1 / T1 = P2 / T2

Solve for P2,

P2 = (P1 × T2) / T1

P2 = (0.470 × 273.15) / 333.15

P2 = 0.385atm

The final pressure is 0.385atm

7 0
2 years ago
Read 2 more answers
(b) If 45.0% of the ethanol that did not produce the ether reacts by the side reaction, what mass (g) of ethylene is produced?
Finger [1]

Ethylene is a hydrocarbon which has the formula C ₂H ₄ or H₂C=CH₂. It is a colourless flammable gas with a faint "sweet and musky" odour when pure. It is the simplest alkene.

Ethylene is widely used in the chemical industry, and its worldwide production exceeds that of any other organic compound.

<h3>What is ethylene used for?</h3>

Medical: Ethylene is used as an anaesthetic. Metal Fabrication: Ethylene is used as oxy-fuel gas in metal cutting, welding and high velocity thermal spraying. Refining: Ethylene is used as refrigerant, especially in LNG liquefaction plants. Rubber & Plastics: Ethylene is used in the extraction of rubber.

<h3>Is ethylene harmful to humans?</h3>

* Ethylene gas can affect you when breathed in. * Skin contact with liquid Ethylene can cause frostbite. * Exposure to Ethylene can cause headache, dizziness, fatigue, lightheadedness, confusion and unconsciousness. * Ethylene is a HIGHLY FLAMMABLE and REACTIVE chemical and a DANGEROUS FIRE and EXPLOSION HAZARD.

Learn more about ethylene here:

<h3>brainly.com/question/27566273</h3><h3 /><h3>#SPJ4</h3>
3 0
1 year ago
Can yall assist me with this lab? It is really screwing me up... No spam!! the only part that I need is the last page. I will ma
Vesna [10]

Answer:

What is the real meaning of this questions

5 0
2 years ago
Name:_____________________________________________________ Date:___________ Period:_________ 3/23 - 3/27 Assignment 1: Gas Law P
crimeas [40]

Answer:

The answers are;

1. 8.2 liters

2. 1214.84 ml

3. 318.027 K

4. 4.00 l.

Explanation:

1. Boyle's law states that the volume of  given mass of gas is inversely proportional to its pressure at constant temperature

that is

P₁·V₁ = P₂·V₂

Where:

P₁ = Initial pressure = 40.0 mm Hg

V₁ = Initial volume = 12.3 liters

P₂ = Final pressure = 60.0 mm Hg

V₂ = Final volume = Required

From P₁·V₁ = P₂·V₂, V₂ is given by

V_2=\frac{P_1\cdot V_1}{P_2} = \frac{40.0 mm Hg\cdot 12.3 l}{60.0 mm Hg} =  8.2 l

The volume reduces to V₂ = 8.2 liters

2. Here Charles law states that

\frac{T_1}{V_1} =\frac{T_2}{V_2}

T₁ = Initial temperature = 27.0 °C = 300.15 K

V₁ = Initial volume = 900.0 mL

T₂ = Final temperature = 132.0 °C = 405.15 K

V₂ = Final volume = Required

Therefore  V_2 =\frac{T_2\cdot V_1}{T_1} = \frac{405.15 K\times 900.0 mL}{300.15 K} = 1214.84 ml

V₂ = 1214.84 ml

3.  Gay-Lussac's Law states that

\frac{T_1}{P_1} =\frac{T_2}{P_2}

Where:

P₁ = Initial pressure = 15.0 atmospheres

T₁ = Initial temperature = 25.0 °C = 298.15 K

P₂ = Final pressure = 16.0 atmospheres

T₂ = Final temperature = Required

∴ T_2 = \frac{T_1\times P_2}{P_1}

=  \frac{298.15 K\times 16.0atm}{15.0atm} = 318.027 K

T₂ = 318.027 K

4. Avogadro's law states that,

Equal volume of all gases at the same temperature and pressure contain equal number of molecules.

Therefore if 5.00 moles of gas occupies 2.00 l volume, then

1 moles will occupy 2.00/5 l volume and

10 moles will occupy 2.00/5 × 10 or 4.00 l volume.

6 0
3 years ago
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