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Nata [24]
3 years ago
7

What is a chemical reaction?

Chemistry
2 answers:
Mila [183]3 years ago
8 0

Answer:

A chemical reaction is defined as per encyclopedia Britannia as a "a process in which one or more substances, are converted to one or more different substances, the products."

So A is correct, B is correct, C is correct.

So that means we choose D as they're all correct.

Mkey [24]3 years ago
5 0

Answer:

D.

Explanation:

this is because in a chemical reaction all 3 of those work.

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Each equation is incorrect. find the errors, then rewrite and balance each equation. cl2 + nai → nacl2 + i nh3 → n + h2 na + o2
VikaD [51]
1) Balanced chemical reaction: Cl₂ + 2NaI → 2NaCl + I₂.
Chlorine and iodine are diatomic molecules.
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3 years ago
How do scientists think that gravity affected the formation of our solar system?
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Maybe because gravity has control of each formation of the solarsydtem thats why its just a guess
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3 years ago
Naphthalene, C10H8, melts at 80.2°C. If the vapour pressure of the liquid is 1.3 kPa at 85.8°C and 5.3 kPa at 119.3°C, use th
sweet-ann [11.9K]

(a) One form of the Clausius-Clapeyron equation is

ln(P₂/P₁) = (ΔHv/R) * (1/T₁ - 1/T₂); where in this case:

  • P₁ = 1.3 kPa
  • P₂ = 5.3 kPa
  • T₁ = 85.8°C = 358.96 K
  • T₂ = 119.3°C = 392.46 K

Solving for ΔHv:

  • ΔHv = R * ln(P₂/P₁) / (1/T₁ - 1/T₂)
  • ΔHv = 8.31 J/molK * ln(5.3/1.3) / (1/358.96 - 1/392.46)
  • ΔHv = 49111.12 J/molK

(b) <em>Normal boiling point means</em> that P = 1 atm = 101.325 kPa. We use the same formula, using the same values for P₁ and T₁, and replacing P₂ with atmosferic pressure, <u>solving for T₂</u>:

  • ln(P₂/P₁) = (ΔHv/R) * (1/T₁ - 1/T₂)
  • 1/T₂ = 1/T₁ - [ ln(P₂/P₁) / (ΔHv/R) ]
  • 1/T₂ = 1/358.96 K - [ ln(101.325/1.3) / (49111.12/8.31) ]
  • 1/T₂ = 2.049 * 10⁻³ K⁻¹
  • T₂ = 488.1 K = 214.94 °C

(c)<em> The enthalpy of vaporization</em> was calculated in part (a), and it does not vary depending on temperature, meaning <u>that at the boiling point the enthalpy of vaporization ΔHv is still 49111.12 J/molK</u>.

3 0
3 years ago
The volume, in liters, occupied by 2.50 moles of N2 gas.<br><br><br> calculate at STP
kondaur [170]

Answer: The volume occupied by 2.50 moles of N_2 gas at STP is 56.0L

Explanation:

According to ideal gas equation:

PV=nRT

P = pressure of gas = 1 atm (at STP)

V = Volume of gas = ?

n = number of moles = 2.50

R = gas constant =0.0821Latm/Kmol

T =temperature =273K  (at STP)

V=\frac{nRT}{P}

V=\frac{2.50mol\times 0.0821Latm/K mol\times 273K}{1atm}=56.0L

Thus the volume occupied by 2.50 moles of N_2 gas at STP is 56.0L

6 0
3 years ago
In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white soli
Digiron [165]

Explanation:

When magnesium metal burns is heated i the air it forms magnesium oxide.The balanced chemical reaction is given as:

2Mg+O_2\rightarrow 2MgO

2 moles of magnesium metal when reacts with 1 moles of oxygen it gives 2 moles of magnesium oxide which is white in color.

Some times along with formation of magnesium oxide small amount of magnesium nitride also produced due to which magnesium oxide appears grey in color .The balanced chemical reaction is given as:

3Mg+N_2\rightarrow Mg_3N_2

3 moles of magnesium combines with 1 mol of nitrogen gas to to give 1 mol of magnesium nitride.

6 0
3 years ago
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