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3 years ago

What happens in the artificial transmutation of an element? Include an example.

1 answer:

6 0

What happens in the artificial transmutation is that the nucleous is bombarded with high energy particles which we can describe as kinetic energy and the idea for them is to induce what we call transmutation. Also what happens is that the high energy particles are accelerated. One of the examples is when nitrogen is transformed into hydrogen by combining its nucleous with an alpha particle

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1. Except for special cases such as peroxides, oxygen has an oxidation number of _______ in compounds. A. +2 B. –1 C. +1 D. –2

egoroff_w [7]

Answer:

The Typical Oxidation number of Oxygen is –2.

And as the question said... its Oxidation changes to –1 when it is in Peroxides and –½ when its in SuperOxides.

Correct Answer : Option D.

7 0

2 years ago

Convert each of the measurements given to the new unit stated using the factor label method (dimensional analysis). Show all wor

jeka94

26 cm -0.26 m

4 hr - 240 min

3.25 km -3250 m

5 ft -60 inches

8 0

2 years ago

how many moles of sodium hydroxide would have to be added to 250 ml of a 0.403 m acetic acid solution, in order to prepare a buf

jonny [76]

The volume of the buffer solution having a ph value is calculated by henderson's hasselbalch equation.

Buffer solution is water based solution which consists of a mixture containing a weak acid and a conjugate base of the weak acid. or a weak base and conjugate acid of a weak base.it is a mixture of weak acid and a base. The pH of the buffer solution is determined by the expression of the henderson hasselbalch equation.

pH=pKa + log [salt]/[acid]

Where, pKa =dissociation constant , A- = concentration of the conjugate base, [HA]= concentration of the acid. Here, a buffer solution contains 0.403m acetic acid and 250 ml is added in order to prepare a buffer with a ph of 4.750. Putting all the values in the henderson hasselbalch equation we find the pH of the buffer solution.

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6 0

9 months ago

A sample of thionylchloride, SOCl2, contains 0.206 mol of the compound. What is the mass of the sample, in grams?

Ilia_Sergeevich [38]

Explanation:

Moles=mass/molar mass

moles × molar mass = mass

0.206 x 119= mass

Mass= 24. 51grams

3 0

2 years ago

Read 2 more answers

How many moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.0 degrees Cel

o-na [289]

1.137448506 mol moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.0 degrees Celsius.

<h3>What is an ideal gas equation?</h3>

The ideal gas equation, pV = nRT, is an equation used to calculate either the pressure, volume, temperature or number of moles of a gas. The terms are: p = pressure, in pascals (Pa). V = volume, in $m^3$ .

We apply the formula of the ideal gases, we clear n (number of moles); we use the ideal gas constant R = 0.082 l atm / K mol:

PV= nRT

Given data:

P=100.0 kPa =0.986923 atm

T=100 degree celcius= 100 + 273 =373 K

V=35.5 L

Substituting the values in the equation.

n= $\frac{\;0,98 \;atm \;X \;35,5 \;L }{\;0,082\;atm / \;K mol \;X \;373 K}$

n= 1.137448506 mol

Hence, 1.137448506 mol moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.0 degrees Celsius.

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7 0

1 year ago