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Delicious77 [7]
3 years ago
11

What is the product of the unbalanced combustion reaction below?

Chemistry
1 answer:
bezimeni [28]3 years ago
7 0

Answer:

C

Explanation:

because it is complete combustion so it will produced CO2 +H2O :)

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Which describes the state at which products form at the same rate as reactants?
swat32

Chemical equilibrium<span> is the state in which both reactants and products are present in concentrations which have no further tendency to change with time.
</span><span>Or, we can say that in chemical equilibrium the  ratio between the concentration of the reactants and the products is constant.</span><span>
Chemical equilibrium is a result state when </span><span>the forward reaction proceeds at the same rate as the reverse reaction.
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8 0
2 years ago
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LAB: predicting products
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Answer:

1) synthesis MgI2

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2 years ago
What’s that’s balanced out
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3 years ago
Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. Termed hydrogenation, t
Vitek1552 [10]

<u>Answer:</u> The mass of decane produced is 1.743\times 10^2g

<u>Explanation:</u>

To calculate the number of moles, we use the equation:  

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}       ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

\text{Moles of }H_2=\frac{2.45g}{2g/mol}=1.225mol

The chemical equation for the hydrogenation of decene follows:

C_{10}H_{20}(l)+H_2(g)\rightarrow C_{10}H_{22}(s)

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = \frac{1}{1}\times 1.225=1.225mol of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\\\\\text{Mass of carbon dioxide}=(1.225mol\times 142.30g/mol)=174.3g=1.743\times 10^2g

Hence, the mass of decane produced is 1.743\times 10^2g

5 0
3 years ago
The SI base unit for mass is the gram. TRUE FALSE ​
Anni [7]
The answer is true the si base unit for mass is the gram
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