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3 years ago

Why does carbon, C, have a larger atomic mass than boron, B, even though the

2 answers:

8 0

Carbon is chemical element denoted by the symbol C, have a larger atomic mass than boron, B, even though the each have six neutrons is due to the difference in the amount of protons.

Explanation:

Atomic mass is defined as the total mass of protons, electrons and neutrons, where due to less weightage electrons are neglected in calculation. Boron has 5 number of protons where carbon has 6 number of protons. As carbon has one more proton than boron, its value of atomic mass varies with boron.

scZoUnD [109]3 years ago

3 0

Answer:

Because carbon has one more proton than boron. Carbon has six and Boron has five.

Explanation:

Because it has more subatomic particles. It has one more proton, one more neutron (usually), and one more electron than boron.

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CO2(g)+CCl4(g)⇌2COCl2(g) Calculate ΔG for this reaction at 25 ∘C under these conditions: PCO2PCCl4PCOCl2===0.140 atm0.185 atm0.7

padilas [110]

Answer: The $\Delta G$ for the reaction is 54.425 kJ/mol

Explanation:

For the given balanced chemical equation:

$CO_2(g)+CCl_4(g)\rightleftharpoons 2COCl_2(g)$

We are given:

$\Delta G^o_f_{CO_2}=-394.4kJ/mol\\\Delta G^o_f_{CCl_4}=-62.3kJ/mol\\\Delta G^o_f_{COCl_2}=-204.9kJ/mol$

To calculate $\Delta G^o_{rxn}$ for the reaction, we use the equation:

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

For the given equation:

$\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(COCl_2)})]-[(1\times \Delta G^o_f_{(CO_2)})+(1\times \Delta G^o_f_{(CCl_4)})]$

Putting values in above equation, we get:

$\Delta G^o_{rxn}=[(2\times (-204.9))-((1\times (-394.4))+(1\times (-62.3)))]\\\Delta G^o_{rxn}=46.9kJ=46900J$

Conversion factor used = 1 kJ = 1000 J

The expression of $K_p$ for the given reaction:

$K_p=\frac{(p_{COCl_2})^2}{p_{CO_2}\times p_{CCl_4}}$

We are given:

$p_{COCl_2}=0.735atm\\p_{CO_2}=0.140atm\\p_{CCl_4}=0.185atm$

Putting values in above equation, we get:

$K_p=\frac{(0.735)^2}{0.410\times 0.185}\\\\K_p=20.85$

To calculate the gibbs free energy of the reaction, we use the equation:

$\Delta G=\Delta G^o+RT\ln K_p$

where,

$\Delta G$ = Gibbs' free energy of the reaction = ?

$\Delta G^o$ = Standard gibbs' free energy change of the reaction = 46900 J

R = Gas constant = $8.314J/K mol$

T = Temperature = $25^oC=[25+273]K=298K$

$K_p$ = equilibrium constant in terms of partial pressure = 20.85

Putting values in above equation, we get:

$\Delta G=46900J+(8.314J/K.mol\times 298K\times \ln(20.85))\\\\\Delta G=54425.26J/mol=54.425kJ/mol$

Hence, the $\Delta G$ for the reaction is 54.425 kJ/mol

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3 years ago

Robidium and cesium have similar chemical properties because in the ground it states the atoms of both elements each have

anzhelika [568]

It would be one electron in the outermost shell. Hope this helps!

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3 years ago

What is true about all real machines?

AfilCa [17]

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2 years ago

How is a pure substance different from a mixture?

Sauron [17]

The answer is A.
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3 years ago

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Which orbital notation represents a noble gas in the ground state

MA_775_DIABLO [31]

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