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Vadim26 [7]
3 years ago
11

Which of the following is an example of a chemical change

Chemistry
1 answer:
luda_lava [24]3 years ago
6 0

Answer:

D. all of these are chemical changes

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A photon has an energy of 2.93 × 10 to the power of -25 J. What is its frequency? What type of electromagnetic radiation is this
Svet_ta [14]
You need to know the energy frequency relationship for photons, which is thanks to Max Planck:

Photon Energy = Planck constant x Frequency

Rarranged:
Photon Energy / Planck Constant = Frequency

Planck Constant = 6.63x10^-34

2.93x10^-25 / 6.63x10^-34 = Frequency

6 0
3 years ago
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g aqueous barium hydroxide (ba(oh)2) and nitric acid (hno3) participate in a complete neutralization reaction. in the molecular
Whitepunk [10]

Answer:

Where the products are H2O and Ba(NO3)2

Explanation:

A base, as, barium hydroxide (Ba(OH)2) reacts with an acid (HNO3), producing water (H2O), and the related salt (Ba(NO3)2) in a reaction called <em>neutralization reaction.</em>

The balanced reaction is:

Ba(OH)2 + 2 HNO3 → 2 H2O + Ba(NO3)2

<em>Where the products are H2O and Ba(NO3)2</em>

4 0
3 years ago
A certain gas is present in a 13.0 L cylinder at 1.0 atm pressure. If the pressure is increased to 2.0 atm , the volume of the g
Scorpion4ik [409]
<h3>Answer:</h3>

The gas obeys the Boyle's law

<h3>Explanation:</h3>
  • According to Boyle's law, the volume of a fixed mass of a gas and the pressure are inversely proportional at constant absolute temperature.
  • That is; P\alpha\frac{1}{V}
  • Therefore, k=PV, where k is a constant
  • At varying volume and pressures while keeping absolute temperature constant; k = P1V1 =P2V2

In this case, we are given;

Initial Volume of 13.0 L at initial pressure of 1.0 atm

New volume of 6.5 L at new pressure of 2.0 atm

But, K = PV

Therefore,

k1 = P1V1

   = 1.0 atm × 13.0 L

  = 13 atm.L

k2 = P2V2

    = 2.0 atm × 6.5 L

    = 13 atm.L

Thus, k1=k2

Thus, the gas obeys the Boyle's law

8 0
3 years ago
What is true for two pieces of iron at the same temperature?
Ber [7]
<span>D. The average kinetic energy of their particles is the same.</span>
5 0
3 years ago
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A sample of argon gas occupies 105 mL at 0.871 atm. If
qwelly [4]

Answer:

1. final pressure = 0.259atm

2. 196.84mmHg

Explanation:

Using Boyle's law of equation

P1V1 = P2V2

Where;

P1 = initial pressure (atm)

P2 = final pressure (atm)

V1 = initial volume (mL)

V2 = final volume (mL)

According to the information given in this question:

V1 = 105mL

V2 = 352mL

P1 = 0.871atm

P2 = ?

Using P1V1 = P2V2

P2 = P1V1/V2

P2 = 0.871 × 105/352

P2 = 91.455/352

P2 = 0.2598

P2 = 0.259atm

To convert 0.259atm of the gas into mmHg, we multiply the value in atm by 760.

Hence, 0.259 × 760

= 196.84mmHg

6 0
3 years ago
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