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3 years ago

A typical carbon atom has six protons, six neutrons, and six electrons. Which of these has the least amount of mass?

Chemistry

2 answers:

ella [17]3 years ago

8 0

Answer:

Explanation:

vova2212 [387]3 years ago

8 0

Answer:

six electrons

Explanation:

Electrons have almost virtually no mass and much less than a proton and neutron.

(a neutron and electron have about 1 amu while electrons have 0.000548 amu)

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If you burn 52.0 g of hydrogen and produce 465 g of water, how much oxygen reacted?

Nadusha1986 [10]

Well, since matter doesn't simply poof into existence and water is H2O, 465g of water is a combination of 52.0g of H and 413g O

7 0

4 years ago

Pentaborane-9, B5H9, is a colorless, highly reactive liquid that will burst into flame when exposed to oxygen. The reaction is 2

mina [271]

<u>Answer:</u> The amount of energy released per gram of $B_5H_9$ is -71.92 kJ

<u>Explanation:</u>

For the given chemical reaction:

$2B_5H_9(l)+12O_2(g)\rightarrow 5B_2O_3(s)+9H_2O(l)$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f_{(product)}]-\sum [n\times \Delta H^o_f_{(reactant)}]$

The equation for the enthalpy change of the above reaction is:

$\Delta H^o_{rxn}=[(5\times \Delta H^o_f_{(B_2O_3(s))})+(9\times \Delta H^o_f_{(H_2O(l))})]-[(2\times \Delta H^o_f_{(B_5H_9(l))})+(12\times \Delta H^o_f_{(O_2(g))})]$

Taking the standard enthalpy of formation:

$\Delta H^o_f_{(B_2O_3(s))}=-1271.94kJ/mol\\\Delta H^o_f_{(H_2O(l))}=-285.83kJ/mol\\\Delta H^o_f_{(B_5H_9(l))}=73.2kJ/mol\\\Delta H^o_f_{(O_2(g))}=0kJ/mol$

Putting values in above equation, we get:

$\Delta H^o_{rxn}=[(5\times (1271.94))+(9\times (-285.83))]-[(2\times (73.2))+(12\times (0))]\\\\\Delta H^o_{rxn}=-9078.57kJ$

We know that:

Molar mass of pentaborane -9 = 63.12 g/mol

By Stoichiometry of the reaction:

If 2 moles of $B_5H_9$ produces -9078.57 kJ of energy.

Or,

If $(2\times 63.12)g$ of $B_5H_9$ produces -9078.57 kJ of energy

Then, 1 gram of $B_5H_9$ will produce = $\frac{-9078.57kJ}{(2\times 63.12)}\times 1g=-71.92kJ$ of energy.

Hence, the amount of energy released per gram of $B_5H_9$ is -71.92 kJ

8 0

3 years ago

Energy Sources (6 points) A. Sort the types of energy into the "renewable" and "nonrenewable" columns. (1 point)

denpristay [2]

Explanation:

(A) Renewable resources are defined as the resources that can be used again and again.

For example, wind, hydroelectric energy, geothermal etc.

On the other hand, resources which cannot be used again and again and which cannot be replaced by natural means are known as non-renewable resources.

For example, coal, petroleum etc are all non-renewable resources.

Therefore, given options are distinguished as follows.

Renewable energy : Wind, Hydroelectric, Geothermal, Biomass, and Solar.

Non-renewable energy : Coal, Petroleum, Natural gas.

(B) Fuels which decompose for a long period of time and which arise from old life forms are known as fossil fuels.

When fossil fuels burn in the presence of air that is, combustion of fossil fuels give carbon dioxide and water.

7 0

4 years ago

The boiling point of an aqueous 1.83 m (nh4)2so4 (molar mass = 132.15 g/mol) solution is 102.5°c. determine the value of the van

Goshia [24]

We need to know the value of van't hoff factor.

The van't hoff factor is: 2.66 or 2.7 (approximately)

(NH₄)₂SO₄ is an ionic compound, so it dissociates in solution and produces 3 ionic species. Therefore van't hoff factor is more than one.

From the equation: Δ $T_{b}$ =i $K_{b}$ .m, where Δ $T_{b}$ = elevation of boiling point=102.5 - 100=2.5°C.

m=molality of solute=1.83 m (Given)

$K_{b}$ = Ebullioscopic constant or Boiling point elevation constant= 0.512°C/m (Given)

i= Van't Hoff factor

So, 2.5= i X 0.512 X 1.83

i= $\frac{2.5}{0.512 X 1.83}$

i=2.66= 2.7 (approx.)

6 0

3 years ago

Noz at

Ne4ueva [31]

Answer:

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4 0

3 years ago