The strongest intermolecular forces are in ion-ion bonds which happen when a metal bonds to another metal. 2. The next strongest forces are ion-dipole bonds which happen when metals bond to nonmetals. 3.

4 0

2 years ago

In the Reaction CuCl2 + 2 NaNO3 —> Cu(NO3)2 + 2 Naci

Lunna [17]

Explanation:

The molar mass of the compounds are incorrect

5 0

2 years ago

Positive feedback is when the change caused by the stimulus is A )decreased B) changes constantly C) nonexistent D) Increased HE

polet [3.4K]

Answer:

c) nonexistent

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6 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]

Answer: The mass of decane produced is $1.743\times 10^2g$

Explanation:

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