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3 years ago

Explain the differences between an ionic crystal like "NaCl" (Sodium Chloride) and a metal like Fe (Iron).

Chemistry

1 answer:

lesantik [10]3 years ago

7 0

Answer:

salt is weaker and has looser atomic bonds and iron has stronger and tighter ionic bonds

Explanation:

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notsponge [240]

Answer:

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2 years ago

1. A 99.8 mL sample of a solution that is 12.0% KI by mass (d: 1.093 g/mL) is added to 96.7 mL of another solution that is 14.0%

bagirrra123 [75]

Answer:

$m_{PbI_2}=18.2gKI$

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

$2KI+Pb(NO_3)_2\rightarrow 2KNO_3+PbI_2$

Thus, we proceed to compute the reacting moles of Pb(NO3)2 and KI, by using the given concentrations and densities and molar masses which are 331.2 g/mol and 166 g/mol respectively:

$n_{Pb(NO_3)_2}=96.7mL*\frac{1.134g}{mL}*\frac{0.14gPb(NO_3)_2}{1g}*\frac{1molPb(NO_3)_2}{331.2gPb(NO_3)_2} =0.0464molPb(NO_3)_2\\\\n_{KI}=99.8mL*\frac{1.093g}{mL}*\frac{0.12gKI}{1g}*\frac{1molKI}{166gKI} =0.0789molKI$

Next, the 0.0464 moles of Pb(NO3)2 will consume the following moles of KI (consider their 1:2 molar ratio):

$n_{KI}^{consumed\ by\ Pb(NO_3)_2}=0.0464molPb(NO_3)_2*\frac{2molKI}{1molPb(NO_3)_2} =0.0928molKI$

Hence, as only 0.0789 moles of KI are available, KI is the limiting reactant, therefore the formed grams of PbI2, considering its molar mass of 461.01 g/mol and 2:1 molar ratio, are:

$m_{PbI_2}=0.0789molKI*\frac{1molPbI_2}{2molKI} *\frac{461.01gPbI_2}{1molPbI_2} \\\\m_{PbI_2}=18.2gKI$

Best regards.

3 0

4 years ago

How many moles are in 25 grams of dihydrogen monoxide

timurjin [86]

If you'd like the full working, here it is:

I calculated this by using the formula triangle.

Mass

Number Formula
Of moles Mass

To calculate the number if moles in a substance, you need to divide the Mass by the Formula mass. You get the formula mass by adding the atomic masses of the elements in the compound together. In this situation, H2O, it would be two hydrogen molecules plus one oxygen molecule which is 2 + 16. This is because the atomic mass of Hydrogen is 1 and the atomic mass of Oxygen is 16.

Now that we have the Formula mass we can go ahead and do the calculation since we already have the Mass. You do as follows:

Mass divided by Formula mass which is in this case - 25 divided by 18

By doing this calculation you will get the answer which is 1.38 moles which can be rounded to 1.4

Hope this helps :)

6 0

3 years ago

Read 2 more answers

P4O10 -> 4P+5O2 How many moles of phosphorus would be produced if 5.3 mol of P4O10 reacted?

viktelen [127]

Answer:

21.2 moles.

Explanation:

Hello!

In this case, for the given chemical reaction, we can see there is a 1:4 mole ratio between tetraphosphorous decaoxide and phosphorous; therefore, the following proportional factor provides the requested moles of phodphorous:

$n_P=5.3molP_4O_{10} *\frac{4molP}{1molP_4O_{10}} \\\\n_P=21.2molP$

Best regards!

5 0

3 years ago

HELP ASAP

Artemon [7]

10 minutes hope it helps

3 0

3 years ago