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igomit [66]
3 years ago
9

How many grams of aluminum can react with 336g oxygen? 4Al + 3O2 --> 2Al2O3

Chemistry
1 answer:
baherus [9]3 years ago
5 0

Answer: 714 g Al2O3

Explanation: Solution attached

First convert mass of O2 to moles

Do the mole ratio between O2 and Al2O3 from the balanced equation.

Convert moles of Al2O3 to mass using its molar mass.

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Complete this sentence. If mass remains the same while the volume of a substance ________, the density of the substance will____
Andre45 [30]
<span> If mass remains the same while the volume of a substance increases, the density of the substance will decrease. The increase in the volume is called expansion, while the decrease in the volume is called contraction.
</span><span>The density measures how much matter (mass) there is in a given amount of space (volume).  So, if the mass stays the same and the volume increases then there is the same amount of mass ad before but in bigger volume so the density is decreased. </span>
4 0
3 years ago
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For a second order reaction, the half-life is equal to:_____.
gtnhenbr [62]

Answer:

Half life = 1 / k[Ao]

Explanation:

From:

1/ [A] = kt + 1/ [Ao]

Isolating t on its own, we have:

kt = 1 / [A] - 1 / [Ao]

t = 1 / [Ao] / k

Re-arranging we have:

t = 1 / k [Ao]

The t represents the t=half life of the second order reaction and the formula can be re-written as:

t1/2 = 1 / k [Ao]

This is so because second order reaction decreases at a much faster rate than zero and first order reactions and there slopes decreases to zero at a much faster rate.

4 0
3 years ago
There are a equal number of protons and electeons in natural atoms True or false​
Rudiy27

Answer:

false

Explanation:

There are a equal number of protons and electrons in neutral atoms.

5 0
3 years ago
Consider the reaction between hydrazine and hydrogen to produce ammonia, N2H4(g)+H2(g)→2NH3(g). Use enthalpies of formation and
kupik [55]

Answer:

The enthalpy of the nitrogen-nitrogen bond in N2H4 is 162.6 kJ

Explanation:

For the reaction: N2H4(g)+H2(g)→2NH3(g), the enthalpy change of reaction is

ΔH rxn = 2 ΔHºf NH3 - ΔHºf N2H4

but we also know that the ΔH rxn is calculated by accounting   the sum of number of bonds formed and bonds broken as follows:

ΔH rxn = 6H (N-H) + 4 (N-H) + 2H (H-H)  

where H is the bond enthalpy .When bonds are broken H is positive, and negative when formed,  in the product there are 6 N-H bonds , and in the reactants 4 N-H and 1 H-H bonds).

Consulting an appropiate reference handbook or table the following values are used:

ΔHºf (NH3) = -46 kJ/mol

ΔHºf (N2H4) = 95.94 kJ/mol

(The enthalpy of fomation of hydrogen in its standard state is zero)

H (N-H) = 391 kJ

H (H-H) = 432 kJ

H (N-N) = ?

So plugging our values:

ΔH rxn =  2mol ( -46.0 kJ/mol) - 1mol(95.4 kJ/mol) = -187.40 kJ

-187.40 kJ = 6(-391 kJ) + 4 (391 kJ) + 432 +  H(N-N)

-187.40 kJ = -350 kJ + H(N-N)

H(N-N) = 162.6 kJ

7 0
3 years ago
If the actual yield of the reaction was 75% instead of 100%, how many molecules of no would be present after the reaction was ov
artcher [175]
To be able to answer this equations, we must set given information. Suppose the reaction to yield NO is:

N₂ + O₂ → 2 NO

Next, suppose you have 1 g of each of the reactants. Determine first which is the limiting reactant.

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Number of molecules = 0.07154 mol NO(6.022×10²³ molecules/mol)
<em>Number of molecules = 4.3×10²² molecules NO present</em>
8 0
3 years ago
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