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2 years ago

10

Balance and classify the following equations as synthesis, decomposition, single replacement, double replacement, or combustion:

a. C4H10 + 02 -> CO2 + H20 Reaction Type: b. ___ HNO3 + Mg(OH)2 -> Mg(NO3)2 + H20 Reaction Tyne.

1 answer:

vodomira [7]2 years ago

8 0

See which one is the bigger equitation to classify the smallest in order

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An ionic compound is composed of elements X and Y. X forms

mote1985 [20]

Answer: X2Y3

Explanation: I had the same question ;) (and got it right)

7 0

2 years ago

For the reaction: 2 A (g) + B (s)= 2 C(s) + D (g)

jolli1 [7]

Answer:

The value of the equilibrium constant = 5.213

Explanation:

Here $K_p$ (equilibrium constant) is referred to as the partial pressure of product divided by the partial pressure of reactant with each pressure term raised to power that is equal to its stoichiometric coefficient in balanced equation .

As such only gas appear in $K_p$ expression as solids takes a value of 1;

SO ; in the given equation from the question:

2 A (g) + B (s) ----> 2 C(s) + D (g)

$K_p = \dfrac{[D]}{[A]^2}$

$K_p = \dfrac{2.71}{0.721^2}$

$K_p = 5.213$

The value of the equilibrium constant = 5.213

8 0

2 years ago

Question 18 (Essay Worth 8 points)

DENIUS [597]

Yes, the law of conservation of mass holds.

Explanation:

In every chemical reaction, mass is always conserved. This implies that in chemical reaction, the process proceeds maintaining the same set of atom in the same proportion without new ones forming.

From the description given, decomposition of the Silver carbonate will produce a silver residue with the given mass.
The other mass that seems lost can be examined to be given off as carbon dioxide gas which is the other product of the reaction and oxygen.
Therefore, since the products are silver, carbon dioxide and oxygen, the remaining mass is that of the carbon dioxide and oxygen. It is not lost.

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4 0

2 years ago

Use the balanced equation from number four above to determine the limiting reactant if we had a mixture of 5.0 moles of Fe and 4

Tom [10]

Answer:

2Fe + 3O₂ → 2Fe₂O₃

Limiting reactant: O₂

2Fe + O₂ → 2FeO

Limiting reactant: Fe

Explanation:

2Fe + 3O₂ → 2Fe₂O₃

2Fe + O₂ → 2FeO

These are the possible reactions:

In first case, 2 moles of Fe need 3 mol of oyxgen to react

If I have 5 moles of Fe, I will need (5 .3)/2 = 7.5 moles of O₂

Then, the oxygen is my limiting ( I only have 4 moles)

3 moles of O₂ need 2 moles of Fe

If I have 4 moles of O₂, I will need (4 .2)/3 = 2.66 moles (I have 5)

Fe, is the reactant in excess.

For second case, 2 moles of Fe need 1 mol of O₂, to react.

If I have 5 moles of Fe, I will need ( 5 .1) / 2 =2.5 moles of O₂

I have 4 moles of oxygen, so now it is my excess.

1 mol of O₂ need 2 moles of Fe, to react

If I have 4 moles of O₂, I will need the double of amount, 8 moles of Fe.

I have 5 moles, then the Fe is my limtiing reactant.

8 0

2 years ago

Identify the functional groups attached to the benzene ring as either, being electron withdrawing, electron donating, or neither

Dominik [7]

-OH is elctron donating -C=-N is electron withdrawing -O-CO-CH3 is electron withdrawing -N(CH3)2 is electron donating -C(CH3)3 is electron donating -CO-O-CH3 is electron withdrawing -CH(CH3)2 is electron donating -NO2 is electrong withdrawing -CH2

8 0

3 years ago