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german
4 years ago
5

Give reason

Chemistry
1 answer:
Bess [88]4 years ago
7 0

Answer:

Explanation:

The solid copper reacts with the silver nitrate solution (in water) to produce solid silver and copper nitrate. This is called a redox reaction. The copper gives up 2 electrons (oxidized) and transfers them to 2 silver ions to produce solid silver (reduction).

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Initially 10.0 mL of water was placed in a graduate cylinder and then a solid metal was immersed in the water in the graduated c
Ahat [919]

Answer: 1682 kg/m^3

Explanation:

the formula for density is mass/volume

to get the volume of the metal = Final Volume - Initial Volume

= 15.5 - 10.0 = 5.5mL

density of the metal = 9.25g/5.5mL = 1.682g/mL

to convert from g/mL to kg/m^3, multiply by 1000

density of metal = 1682 kg/m^3

7 0
3 years ago
The closeness of a measurement to its true value is a measure of its _____.
svlad2 [7]
The closeness of a measurement to its true value is a measure of its accuracy. This term is the degree of which a certain measurement conforms to the correct value or the standard value. It is not the same with the term precision. Precision, on the other hand, is a measure used to characterize the closeness of the data measured.
7 0
3 years ago
Read 2 more answers
When the valve between the two containers is opened and the gases allowed to mix, how does the volume occupied by the n2 gas cha
schepotkina [342]
Missing question: 
Nitrogen: <span>2.0 L; </span>1.0 atm; 25°<span>C.
Oxygen: 3</span>.0 L; 2.0 atm; 25°C.
<span>When the valve between the two containers is opened, nitrogen gas moves from one container to another container and gases are mixed together, total volume of nitrogen is than:
V(nitrogen) = 2,0 L + 3,0 L = 5,0 L.</span>
4 0
3 years ago
Read 2 more answers
Nitrogen gas reacts with hydrogen gas to produce ammonia. How many liters of hydrogen gas at 95kPa and 15∘C are required to prod
viktelen [127]

Answer:

222.30 L

Explanation:

We'll begin by calculating the number of mole in 100 g of ammonia (NH₃). This can be obtained as follow:

Mass of NH₃ = 100 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3

= 17 g/mol

Mole of NH₃ =?

Mole = mass /molar mass

Mole of NH₃ = 100 / 17

Mole of NH₃ = 5.88 moles

Next, we shall determine the number of mole of Hydrogen needed to produce 5.88 moles of NH₃. This can be obtained as follow:

N₂ + 3H₂ —> 2NH₃

From the balanced equation above,

3 moles of H₂ reacted to produce 2 moles NH₃.

Therefore, Xmol of H₂ is required to p 5.88 moles of NH₃ i.e

Xmol of H₂ = (3 × 5.88)/2

Xmol of H₂ = 8.82 moles

Finally, we shall determine the volume (in litre) of Hydrogen needed to produce 100 g (i.e 5.88 moles) of NH₃. This can be obtained as follow:

Pressure (P) = 95 KPa

Temperature (T) = 15 °C = 15 + 273 = 288 K

Number of mole of H₂ (n) = 8.82 moles

Gas constant (R) = 8.314 KPa.L/Kmol

Volume (V) =?

PV = nRT

95 × V = 8.82 × 8.314 × 288

95 × V = 21118.89024

Divide both side by 95

V = 21118.89024 / 95

V = 222.30 L

Thus the volume of Hydrogen needed for the reaction is 222.30 L

8 0
3 years ago
126785033% Divided by 348675948849 = <br> what does it equal
meriva

Answer:

0.00000363618

could be wrong.

double check me someone or just trust me

(don't blame me if you get it wrong)

5 0
3 years ago
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