All categories

3 years ago

Mixing salt with water is an example of a _________change. * physical change chemical change

Chemistry

1 answer:

SIZIF [17.4K]3 years ago

6 0

Answer:

physical

Explanation:

no chemical reaction is happening

You might be interested in

Plant cell synthesize energy rich organic molecules and later energy is released through the processes of

zmey [24]

Pretty sure its photosynthesis ?

7 0

2 years ago

A substance made of metal atoms only?

SVEN [57.7K]

It has to be a metal, it can't be anything else.

5 0

2 years ago

HELP!!!!! NO SPAM!!!!!!!!!!!!!!!!!

Lisa [10]

Answer:

Explanation: S + 6 HNO3 --> H2SO4 + 6 NO2 + 2 H2O In the above equation how many moles of water can be made when 115.3 grams of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Element Molar Mass Hydrogen 1 Nitrogen 14 Sulfur 32 Oxygen 16...

Hope it helps..!!

4 0

2 years ago

Read 2 more answers

2AlBr3 + ___ -> 6KBr + Al2(SO4)3

Masja [62]

Answer:

Explanation:

6 0

2 years ago

Read 2 more answers

Most fertilizers consist of nitrogen-containing compounds such as NH3,CO(NH2)2,NH4NO3, and (NH4)2SO4. Plants use the nitrogen co

Y_Kistochka [10]

Answer: 1. $NH_3=82.4\%$

2. $CO(NH_2)_2=46.7\%$

3. . $NH_4NO_3=35\%$

4. $(NH_4)_2SO_4=21.2\%$

$NH_3$ has highest nitrogen content.

Explanation:

To calculate the mass percent of element in a given compound, we use the formula:

$\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Molar mass of nitrogen compound}}\times 100$

1. $NH_3$

$\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of} NH_3}=\frac{14}{17}\times 100=82.4\%$

2. $CO(NH_2)_2$

$\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of} CO(NH_2)_2}=\frac{14\times 2}{12\times 1+16\times 1+2\times 14+4\times 1}\times 100=\frac{28}{60}\times 100=46.7\%$

3. $NH_4NO_3$

$\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of} NH_4NO_3}=\frac{14\times 2}{14\times 2+16\times 3+4\times 1}\times 100=\frac{28}{80}\times 100=35\%$

4. $(NH_4)_2SO_4$

$\text{Mass percent of nitrogen}=\frac{\text{Mass of nitrogen}}{\text{Mass of}(NH_4)_2SO_4}=\frac{14\times 2}{14\times 2+16\times 4+32\times 1+8\times 1}\times 100=\frac{28}{132}\times 100=21.2\%$

Thus $NH_3$ has highest nitrogen content of 82.4%.

8 0

3 years ago