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dolphi86 [110]
3 years ago
12

Which type of reaction is Mg + S → MgS?

Chemistry
2 answers:
Anestetic [448]3 years ago
6 0

Answer: Synthesis reaction

Explanation:

Synthesis reaction as refers to as direct combination is a reaction in which two or more chemical species combine to form more complex product.

neonofarm [45]3 years ago
5 0

Answer:

the answer is the second option

Explanation:

hope this helps

You might be interested in
combustion analysis of a hydrocarbon produced 33.01g CO2 and 13.51g H2O. Calculate the empirical formula for the hydrocarbon
masya89 [10]

Answer:

\rm CH_2.

Explanation:

Carbon and hydrogen are the only two elements in a hydrocarbon. When a hydrocarbon combusts completely in excess oxygen, the products would be \rm CO_2 and \rm H_2O. The \rm C and \rm H would come from the hydrocarbon, while the \rm O atoms would come from oxygen.

Look up the relative atomic mass of these three elements on a modern periodic table:

  • \rm C: 12.011.
  • \rm H: 1.008.
  • \rm O: \rm 15.999.

Calculate the molar mass of \rm CO_2 and \rm H_2O:

M(\mathrm{CO_2}) = 12.011 + 2 \times 15.999 = 44.009\; \rm g \cdot mol^{-1}.

M(\mathrm{H_2O}) = 2 \times 1.008 + 15.999 = 18.015\; \rm g \cdot mol^{-1}

Calculate the number of moles of \rm CO_2 molecules in 33.01\; \rm g of \rm CO_2\!:

\displaystyle n(\mathrm{CO_2}) = \frac{m(\mathrm{CO_2})}{M(\mathrm{CO2})} = \frac{33.01\; \rm g}{44.009\; \rm g\cdot mol^{-1}} \approx 0.7501\; \rm mol.

Similarly, calculate the number of moles of \rm H_2O molecules in 13.51\; \rm g of \rm H_2O\!:

\displaystyle n(\mathrm{H_2O}) = \frac{m(\mathrm{H_2O})}{M(\mathrm{H_2O})} = \frac{13.51\; \rm g}{18.015\; \rm g\cdot mol^{-1}} \approx 0.7499\; \rm mol.

Note that there is one carbon atom in every \rm CO_2 molecule. Approximately0.7501\; \rm mol of \rm CO_2\! molecules would correspond to the same number of \rm C atoms. That is: n(\mathrm{C}) \approx 0.7501\; \rm mol.

On the other hand, there are two hydrogen atoms in every \rm H_2O molecule. approximately 0.7499\; \rm mol of \rm H_2O molecules would correspond to twice as many \rm H\! atoms. That is: n(\mathrm{H}) \approx 2 \times 0.7499 \; \rm mol\approx 1.500\; \rm mol.

The ratio between the two is: n(\mathrm{C}): n(\mathrm{H}) \approx 1:2.

The empirical formula of a compound gives the smallest whole-number ratio between the elements. For this hydrocarbon, the empirical formula would be \rm CH_2.

6 0
3 years ago
In molecular oxygen (O=O) which atom is partially positive?
saveliy_v [14]

the oxygen atom

Explanation:

Water is a molecular compound consisting of polar molecules that have a bent shape. The oxygen atom acquires a partial negative charge while the hydrogen atom acquires a partial positive charge.

4 0
3 years ago
Read 2 more answers
Suppose you put a whole antacid tablet in one glass of water and a crushed antacid tablet in another glass containing the same a
iogann1982 [59]
The crushed tablets would stop bubbling/fuzzing first because it has a smaller surface area which means that it would dissolve before the uncrushed tablets which has a larger surface area.
3 0
3 years ago
It takes 281.7 kJ of energy to remove 1 mole of electrons from the atoms on the surface of lithium metal. If lithium metal is ir
Alex17521 [72]

Answer:

The maximum kinetic energy of electron is = 2.93 × 10^{-19} Joule

Explanation:

We know that total energy

E = \frac{hc}{\lambda}  ------------ (1)

Here h = plank's constant = 6.62 × 10^{-34} J s

c = speed of light = 3 × 10^{8} \frac{m}{s}

\lambda = 261 nm = 261  × 10^{-9} m

Put all these values in equation (1) we get

E = 7.6   × 10^{-19} J

We know that

Total energy = Energy to remove an electron + K.E of electron

Energy to remove an electron = \frac{281.7 (1000)}{(6.023)10^{23} }

Energy to remove an electron = 4.67  × 10^{-19} J

K.E of electron = Total energy - Energy to remove an electron

K.E of electron = 7.6   × 10^{-19} -  4.67  × 10^{-19}

K.E of electron = 2.93 × 10^{-19} Joule

Therefore the maximum kinetic energy of electron is = 2.93 × 10^{-19} Joule

3 0
3 years ago
What is the enthalpy of combustion (per mole) of C4H10 (g)? 
Artemon [7]
The balanced chemical reaction for the complete combustion of C4H10 is shown below:

                    C4H10 + (3/2)O2 --> 4CO2 + 5H2O

The enthalpy of formation are listed below:
          C4H10: -2876.9 kJ/mol
              O2:   none (because it is pure substance)
             CO2: -393.5 kJ/mol
             H2O: -285.8 kJ/mol

The enthalpy of combustion is computed by subtracting the total enthalpy formation of the reactants from that of the products.

               ΔHc = (4)(-393.5 kJ/mol) + (5)(-285.8 kJ/mol) - (-2876.9 kJ/mol)
                       = -<em>126.1 kJ</em>

Thus, the enthalpy of combustion of the carbon is -126.1 kJ. 
5 0
3 years ago
Read 2 more answers
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