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MrMuchimi
3 years ago
15

All camels are basically similar in structure. They have developed adaptations for

Chemistry
1 answer:
Feliz [49]3 years ago
5 0

Answer:

B. Camels’ ears are lined with fur to keep out sand and other blowing matter.

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In this case you have unlimited iron, but only 6.40 moles of oxygen (O2). How much Fe2O3 can you produce?
vlada-n [284]

Answer:

wattter

Explanation: H20 jk lma++ooo

7 0
3 years ago
Hydrogen peroxide slowly decomposes in light:
IgorLugansk [536]

Answer:

Explanation: the answer is A

3 0
3 years ago
Why do you think it would be important for scientists to test local water?
il63 [147K]

Answer:

To see if the water is safe to drink.

Explanation:

It is important for local water to be tested to see how the water quality is and to check if there are any pollutants (such as fertilizers or oil). Most of the world's water is not safe to consume, it would be useful to know what your local water is like.

4 0
3 years ago
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HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)
RSB [31]

Answer:

0.036 g

Explanation:

<em>0.036 g of water should be produced.</em>

From the equation of reaction, 1 mole of HCl requires 1 mole of NaOH in order to produce 1 mole of H2O.

20 mL of 0.10 M HCl contains 20/1000 x 0.10 = 0.002 moles of HCl

46 grams of NaOH contains 46/40 = 1.15 moles of NaOH

<em>It thus means that the HCl is a limiting reagent in the reaction.</em>

From the equation:

1 mole  HCl will produce 1 mole of H2O.

0.002 HCl with therefore produce 0.002 x 1/1 = 0.002 mole of H2O

<em>Mass of water produced = mole x molar mass</em>

    0.002 x 18 = 0.036 g.

Hence, 0.036 g of water would be produced.

8 0
3 years ago
If 500.0 ml of 0.10 m ca2+ is mixed with 500.0 ml of 0.10 m so42−, what mass of calcium sulfate will precipitate? ksp for caso4
attashe74 [19]

Answer : The mass of calcium sulfate precipitate will be, 6.12 grams

Solution :

First we have to calculate the moles of Ca^{2+} and SO_4^{2-}.

\text{Moles of }Ca^{2+}=\text{Molarity of }Ca^{2+}\times \text{Volume of }Ca^{2+}=0.10mole/L\times 0.5L=0.05\text{ moles}

\text{Moles of }SO_4^{2-}=\text{Molarity of }SO_4^{2-}\times \text{Volume of }SO_4^{2-}=0.10mole/L\times 0.5L=0.05\text{ moles}

As, 0.05 moles of Ca^{2+} is mixed with 0.05 moles of  SO_4^{2-}, it gives 0.05 moles of calcium sulfate.

Now we have to calculate the solubility of calcium sulfate.

The balanced equilibrium reaction will be,

CaSO_4\rightleftharpoons Ca^{2+}+SO_4^{2-}

The expression for solubility constant for this reaction will be,

K_{sp}=(s)\times (s)

K_{sp}=(s)^2

Now put the value of K_{sp} in this expression, we get the solubility of calcium sulfate.

2.40\times 10^{-5}=(s)^2

s=4.89\times 10^{-3}M

Now we have to calculate the moles of dissolved calcium sulfate in one liter solution.

\text{Moles of }CaSO_4=\text{Molarity of }CaSO_4\times \text{Volume of }CaSO_4=4.89\times 10^{-3}mole/L\times 1L=4.89\times 10^{-3}\text{ moles}

Now we have to calculate the moles of calcium sulfate that precipitated.

\text{Moles of }CaSO_4\text{ precipitated}=\text{Moles of }CaSO_4\text{ present}-\text{Moles of }CaSO_4\text{ dissolved}

\text{Moles of }CaSO_4\text{ precipitated}=0.05-4.89\times 10^{-3}=0.045\text{ moles}

Now we have to calculate the mass of calcium sulfate that precipitated.

\text{Mass of }CaSO_4\text{ precipitated}=\text{Moles of }CaSO_4\text{ precipitated}\times \text{Molar mass of }CaSO_4

\text{Mass of }CaSO_4\text{ precipitated}=0.045moles\times 136g/mole=6.12g

Therefore, the mass of calcium sulfate precipitate will be, 6.12 grams

5 0
3 years ago
Read 2 more answers
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