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gizmo_the_mogwai [7]

2 years ago

11

True or false Compounds link up to make elements

1 answer:

RSB [31]2 years ago

6 0

This is false because a compound can have only one element.

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What is the thermal energy needed to completely melt 9.60 mol of ice at 0.0 C

inysia [295]

The thermal energy needed to completely melt 9.60 mole of ice at 0.0 C is 57.8 Kj

Explanation
ice melt to form water

The molar heat of fusion for water is 6.02 Kj/mol
Thermal energy = moles x molar heat of fussion for water

=9.6 mol x6.02 kj/mol =57.8 Kj

4 0

3 years ago

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Write the balanced equation for the reaction of aqueous sodium carbonate and aqueous calcium chloride dihydrate to form solid ca

faltersainse [42]

<span>Na2CO3 (aq) + CaCl2H4O2 (aq) = CaCO3 (s) + 2 NaCl (aq) + 2 H2O (l)</span>

5 0

3 years ago

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Which one is it ????

lianna [129]

Cells can generate from non living matter is the answer

3 0

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

Express the following quantity in scientific notation. The answer needs to have the correct number of significant figures. 21,30

melisa1 [442]

2.13 x 10 E 7 i believe this is correct

4 0

3 years ago

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