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1 year ago

Aqueous Copper (II) nitrate reacts with aqueous potassium iodide to form Copper (II) iodide solid and potassium nitrate

Chemistry

1 answer:

nikitadnepr [17]1 year ago

7 0

Answer:

Cu(NO₃)₂ (aq) + 2 KI (aq) ---> CuI₂ (s) + 2 KNO₃

Explanation:

When writing the reaction with the symbols, you need to take into account the charges of the ions. If he charges on the ions do not balance out in a molecule, they need to be made up for in the form of subscripts. For example, copper (+2) and iodine (-1) have charges which do not balance. Thus, to make the molecule neutral, you need to have two iodine atoms (CuI₂).

The unbalanced equation:

Cu(NO₃)₂ (aq) + KI (aq) ---> CuI₂ (s) + KNO₃

Reactants: 1 copper, 2 nitrate, 1 potassium, 1 iodine

Products: 1 copper, 1 nitrate, 1 potassium, 2 iodine

The balanced equation:

1 Cu(NO₃)₂ (aq) + 2 KI (aq) ---> 1 CuI₂ (s) + 2 KNO₃

Reactants: 1 copper, 2 nitrate, 2 potassium, 2 iodine

Products: 1 copper, 2 nitrate, 2 potassium, 2 iodine

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Calculate the mass of water produced when 7.26 g of butane reacts with excess oxygen

MaRussiya [10]

Answer:

11.3 g.

Explanation:

Hello there!

In this case, since the combustion of butane is:

$C_4H_{10}+\frac{13}{2} O_2\rightarrow 4CO_2+5H_2O$

Thus, since there is a 1:5 mole ratio between butane and water, we obtain the following mass of water:

$m_{H_2O}=7.26gC_4H_{10}*\frac{1molC_4H_{10}}{58.14gC_4H_{10}}*\frac{5molH_2O}{1molC_4H_{10}} *\frac{18.02gH_2O}{1molH_2O}$

Therefore, the resulting mass of water is:

$m_{H_2O}=11.3gH_2O$

Best regards!

4 0

3 years ago

A 1.68 g sample of water is injected into a closed evacuated 5.3 liter flask at 65°C. What percent (by mass) of the water will b

Angelina_Jolie [31]

Answer:

50.4 % of the water will be vapor

Explanation:

Step 1: Data given

Mass of water = 1.68 grams

volume of the flask = 5.3 L

Temperature = 65°C

Vapor pressure of water at 65°C = 187.5 mmHg = 0.2467 atm

Step 2: Calculate moles of H2O

p*V=n*R*T

⇒ p = the pressure of water = 0.2467 atm

⇒ V = the volume of the flask = 5.3 L

⇒ n = moles of water

⇒ R = gas constant = 0.08206 L*atm/ K*mol

⇒ T = the temperature = 65°C = 338 Kelvin

n = (p*V)/(R*T)

n = (0.2467 * 5.3) /(0.08206* 338)

n = 0.047 moles

Step 3: Calculate mass of water

Mass of water = moles of water * molar mass of water

Mass of water = 0.047 moles *18.02 g/mol

Mass of water = 0.84694 grams

Step 4: Calculate the percent of water vaporized

% = (0.84694 grams/1.68 grams) *100%

% = 50.4%

50.4 % of the water will be vapor

5 0

3 years ago

How many moles of NO gas are formed from 2.25 moles of nitrogen?

VikaD [51]

Hey there!

A mole is measured in atoms, molecules, particles. It's kind of a loose sort of measurement, just unit of the substance.

Since there is a ratio of 1 to 1 nitrogen to oxygen, there will be the same amount of molecules as atoms of nitrogen.

2.25 moles of NO gas are formed from 2.25 moles of nitrogen.

Hope this helps!

7 0

3 years ago

Pls help!! Which statement best describes the type of radioactive decay shown in the model?

agasfer [191]

Answer:

C. The model shows beta decay, whichis not tyoe of nuclear fission

5 0

3 years ago

Select all the correct answers.

stich3 [128]

Answer : The products of the acid-base reaction between $HClO_3$ and LiOH are, $LiClO_3$ and $H_2O$

Explanation :

Neutralization reaction : It is a type of chemical reaction in which an acid react with a base to give salt and water as a product that means it reacts to give a neutral solution. It is also known as acid-base reaction.

The acid-base reaction will be:

$HClO_3+LiOH\rightarrow LiClO_3+H_2O$

Therefore, the products of the acid-base reaction between $HClO_3$ and LiOH are, $LiClO_3$ and $H_2O$

6 0

3 years ago

Read 2 more answers