All categories

2 years ago

Which of the following compounds will produce H2O as one of the products when it decomposes?

Chemistry

2 answers:

aivan3 [116]2 years ago

8 0

B) Cu(OH) 2 Is the resulting answer when H20 is decomposed.

babunello [35]2 years ago

5 0

Cu(OH)2 will decompose to give water as one of the products

The decomposition reaction will be

Cu(OH)2(s) ----> CuO(s) + H2O(l)

Hence it is giving water as product

You might be interested in

How many grams of CrSO3 are in 2.4 moles of CrSO3

castortr0y [4]

Answer: 316.8 g CrSO3

Explanation: Solution:

2.4 moles CrSO3 x 132 g CrSO3 / 1 mole CrSO3 = 316.8 g CrSO4

The conversion factor is 1 mole of CrSO4 is equal to its molar mass which is 132 g CrSO3

4 0

3 years ago

Write a net ionic equation to show how codeine, c18h21o3n, behaves as a base in water.

Lera25 [3.4K]

Actually, the ionic equation for this is a reversible equation since codeine is a weak base. Any weak base or weak acids do not completely dissociate which makes them a reversible process. The ionic equation for this case is:

<span>C18H21O3N + H3O+ </span><=> C18H21O3NH+ + H2O

7 0

3 years ago

Rewrite 2000 to have 2 sig figs.

aliina [53]

20. Would be the right answer

4 0

3 years ago

Read 2 more answers

Which organic prefix is matched with the number of carbon atoms that it represents?

Mandarinka [93]

Answer:heat-,7

Explanation:According to table P, heat- is an organic prefix used to represent 7 carbon atoms

8 0

3 years ago

One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is Fe2O3 + 3CO → 2Fe + 3CO2 Su

Tpy6a [65]

Answer : The percent purity of $Fe_2O_3$ in the original sample is 87.94 %

Explanation :

The given balanced chemical reaction is:

$Fe_2O3+3CO\rightarrow 2Fe+3CO_2$

First we have to calculate the mass of Fe.

$\text{Moles of }Fe=\frac{\text{Mass of }Fe}{\text{Molar mass of }Fe}$

Molar mass of Fe = 55.8 g/mole

$\text{Moles of }Fe=\frac{1.79\times 10^3kg}{55.8g/mole}=\frac{1.79\times 10^3\times 1000g}{55.8g/mole}=3.15\times 10^4mole$

Now we have to calculate the moles of $Fe_2O_3$

From the balanced chemical reaction we conclude that,

As, 2 moles of Fe produced from 1 mole of $Fe_2O_3$

So, $3.15\times 10^4mole$ of Fe produced from $\frac{3.15\times 10^4}{2}=15750$ mole of $Fe_2O_3$

Now we have to calculate the mass of $Fe_2O_3$

$\text{ Mass of }Fe_2O_3=\text{ Moles of }Fe_2O_3\times \text{ Molar mass of }Fe_2O_3$

Molar mass of $Fe_2O_3$ = 159.69 g/mole

$\text{ Mass of }Fe_2O_3=(15750moles)\times (159.69g/mole)=2.515\times 10^6g=2.515\times 10^3kg$

Now we have to calculate the percent purity of $Fe_2O_3$ in the original sample.

Mass of original sample = $2.86\times 10^3kg$

$\text{Percent purity}=\frac{\text{Mass of }Fe_2O_3}{\text{Mass of sample}}\times 100$

$\text{Percent purity}=\frac{2.515\times 10^3kg}{2.86\times 10^3kg}\times 100=87.94\%$

Therefore, the percent purity of $Fe_2O_3$ in the original sample is 87.94 %

3 0

2 years ago