What kind of intermolecular force is between hydrogen sulfide and hydrogen iodide?

How could you test to see if an enzyme was completely saturated during an experiment?

rodikova [14]

To test this, you'd need to see if a reaction is still taking place, If the enzyme is completely depleted, then the reaction could no longer occur.

6 0

3 years ago

In the Mond process for the purification of nickel, carbon monoxide is reacted with heated nickel to produce Ni(CO)4, which is a

igor_vitrenko [27]

<u>Answer:</u> The equilibrium constant for this reaction is $1.068\times 10^{6}$

<u>Explanation:</u>

The equation used to calculate standard Gibbs free change is of a reaction is:

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

For the given chemical reaction:

$Ni(s)+4CO(g)\rightleftharpoons Ni(CO)_4(g)$

The equation for the standard Gibbs free change of the above reaction is:

$\Delta G^o_{rxn}=[(1\times \Delta G^o_{(Ni(CO)_4(g))})]-[(1\times \Delta G^o_{(Ni(s))})+(4\times \Delta G^o_{(CO(g))})]$

We are given:

$\Delta G^o_{(Ni(CO)_4(g))}=-587.4kJ/mol\\\Delta G^o_{(Ni(s))}=0kJ/mol\\\Delta G^o_{(CO(g))}=-137.3kJ/mol$

Putting values in above equation, we get:

$\Delta G^o_{rxn}=[(1\times (-587.4))]-[(1\times (0))+(4\times (-137.3))]\\\\\Delta G^o_{rxn}=-38.2kJ/mol$

To calculate the equilibrium constant (at 58°C) for given value of Gibbs free energy, we use the relation:

$\Delta G^o=-RT\ln K_{eq}$

where,

$\Delta G^o$ = Standard Gibbs free energy = -38.2 kJ/mol = -38200 J/mol (Conversion factor: 1 kJ = 1000 J )

R = Gas constant = 8.314 J/K mol

T = temperature = $58^oC=[273+58]K=331K$

$K_{eq}$ = equilibrium constant at 58°C = ?

Putting values in above equation, we get:

$-38200J/mol=-(8.314J/Kmol)\times 331K\times \ln K_{eq}\\\\K_{eq}=e^{13.881}=1.068\times 10^{6}$

Hence, the equilibrium constant for this reaction is $1.068\times 10^{6}$

4 0

3 years ago

Briefly explain why an unbalanced chemical equation cannot fully describe a reaction?

zubka84 [21]

From the conservation of mass, matter is not created nor destroyed. So ponder it this way, for example I put one piece of toast in a toaster, but when it is done I had two pieces, that makes no sense right? Same thing with a chemical reaction but in molecular terms, all things must stay constant. If you put a convinced amount you have to get that quantity back, not less or not more in broad terms.

5 0

3 years ago

Alkaline earth metals are very reactive because of how many valence electrons ?

Alborosie

Their is 2 valence electrons

8 0

3 years ago

if you are using 657.0 grams of oxygen gas to react with calcium how many gram of calcium oxide will u product

DochEvi [55]

Answer:

The amount in grams of CaO that will be produced is 2,302.67824 grams

Explanation:

The reaction between calcium and oxygen to produce calcium oxide (quicklime) can be presented as follows;

2Ca (s) + O₂ (g) → 2CaO (s)

From the above chemical equation, we have;

2 moles of calcium, Ca, react with 1 mole of oxygen gas, O₂, to produce 2 moles of CaO

With the assumption that there is an excess amount of Ca, we have;

The molar mass of O₂ = 32 g/mol

The number of moles, 'n', of O₂ in 657.0 grams of oxygen is therefore;

The number of moles of a substance = Mass of substance/(Molar mass of substance)

∴ n = 657.0 g/(32 g/mol) = 20.53125 moles

The number of moles of O₂ in the 657.0 grams of oxygen present in the reaction, n = 20.53125 moles

1 mole of O₂ produces 2 moles of CaO, therefore, 20.53125 moles of oxygen will produce 2 × 20.53125 or 41.0625 moles of CaO

The molar mass of CaO = 56.0774 g/mol

Therefore, the mass of 41.0625 moles of CaO is given as follows;

Mass of substance = (The number of moles of a substance) × (Molar mass of substance)

The mass of CaO produced = 41.0625 moles × 56.0774 g/mol = 2,302.67824 g.

3 0

3 years ago