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mojhsa [17]
3 years ago
12

Bromine has two isotopes, Br79 and Br81. The isotopes occur in a 50:50 (1:1) ratio. Given that the mass spectrum of bromine cont

ains peaks for both bromine atoms and diatomic bromine molecules, predict the number of peaks in the spectrum. What would be the relative height of the atomic peaks
Chemistry
1 answer:
AlekseyPX3 years ago
7 0

Answer:

There will be 3 peaks.

Relative height of the atomic peaks would be; 158, 160 and 162

Explanation:

We are told that Bromine has two isotopes namely 79Br and 81Br in a 1 : 1 ratio (50 : 50).

This means that a compound which contains 1 bromine atom will have two peaks in the molecular ion region but it depends on which bromine isotope is contained in the molecular ion.

Thus;

Relative height of atomic peaks is given by;

m/z = 79Br¯ 79Br+ = 158

79Br¯ 81Br+ = 160

81Br¯ 81Br+ = 162

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Which of the following is the best example of a scientific law?
il63 [147K]

Answer:

The correct answer is :'The gravitational force between two objects is related mathematically to their mass and the distance between them'.

Explanation:

A scientific law is a statement which explains physical phenomena and has been tested multiple times through the correct scientific methods and experimentation. It will give same results and observations after each conduct.

A scientific law comes into picture after the acceptance of a theory which explains or exposes the reason behind any physical phenomena occurrence.

So the best example of scientific law:

The gravitational force between two objects is related mathematically to their mass and the distance between them.

5 0
3 years ago
Read 2 more answers
A weather balloon is filled with helium that occupies a volume of 5.00 × 10^4 L at 0.995 atm and 32.0°C. After it is released, i
DaniilM [7]

Answer:

The new volume is 5.913*10^4 L

Explanation:

Step 1: Write out the formula to be used:

Using general gas equation;

P1V1 / T1 =P2V2 /T2

V2 = P1V1T2 / P2T1

Step 2: write out the values given and convert to standard unit's where necessary

P1 = 0.995atm

P2 0.720atm

V1 = 5*10^4 L

T1 = 32°C = 32+ 273 = 305K

T2 = -12°C = -12 + 273 = 261K

Step 3: Equate your values and do the calculation:

V2 = 0.995 * 5*10^4 * 261 / 0.720 * 305

V2 = 1298.475 * 10^4 / 219.6

V2 = 5.913 * 10^4 L

So the new volume of the balloon is 5.913*10^4 L

3 0
3 years ago
How many moles of a gas would occupy 22.4 Liters at 273 K and 1 atm?
Molodets [167]

Answer:

1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm

Explanation:

An ideal gas is a set of atoms or molecules that move freely without interactions. The pressure exerted by the gas is due to the collisions of the molecules with the walls of the container. The ideal gas behavior is at low pressures, that is, at the limit of zero density. At high pressures the molecules interact and intermolecular forces cause the gas to deviate from ideality.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

  • P= 1 atm
  • V= 22.4 L
  • n= ?
  • R= 0.082 \frac{atm*L}{mol*K}
  • T=273 K

Reemplacing:

1 atm* 22.4 L= n* 0.082 \frac{atm*L}{mol*K} *273 K

Solving:

n=\frac{1 atm* 22.4 L}{0.082 \frac{atm*L}{mol*K} *273 K}

n= 1 mol

Another way to get the same result is by taking the STP conditions into account.

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C (or 273 K) are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.

<u><em>1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm</em></u>

4 0
2 years ago
Besides plants, do other organism get their energy directly from the Sun?<br> yes or no
Contact [7]

yes they doExplanation:

3 0
3 years ago
Read 2 more answers
What pressure in atmospheres(atm) is equal to 45.6 kPa?
postnew [5]
1 kpa = 0.0098692327 atm so just multiply that by 45.6
4 0
3 years ago
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