The OAC simulation showed that warm air over a cold current:

What is the mass of 2.1 moles of the hydrate Nickel (II) carbonate pentahydrate (NiCO3 x 5H2O)?

kifflom [539]

The mass of 2.1 moles of the hydrate Nickel (II) carbonate pentahydrate NiCO3 x 5H2O 773.5 grams.

<h3>What are moles?</h3>

Mole is the smallest particle of atom which is equal to the Avogadro's number which is 2.303 × 10²³moles of an atom and can be calculated by,

number of moles = mass of mole / molar mass of the mole.

mass = 2.1 moles

molar mass of NiCO3 x 5H2O = 368.38

Substituting the value in the formula,

2.1 mole = mass of mole / 368.38

mass of mole = 773.59 grams.

Therefore, mass of 2.1 moles of the hydrate Nickel (II) carbonate pentahydrate NiCO3 x 5H2O 773.5 grams.

Learn more about moles, here:

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4 0

2 years ago

2) write down two examples of mixtures and state their use in daily life.

prisoha [69]

Answer:

first example is. Air it is mixture of many 

gases 

it's us it keeps us alive and many more uses

second example is water is also a mixture 

made up of carbon and hydrogen 

and its uses is to fulfill our needs 

hope it helps

7 0

3 years ago

Balanced Chemical Equation: 2H2(g)+O2(g)——> 2H2O(g)

Tcecarenko [31]

You must use 134 g O₂ to produce 118 g H₂O.

$\%\text{ yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100 \%$

$\text{Theoretical yield} = \text{Actual yield}\times \frac{100\%}{\%\text{ yield}} = \text{118 g }\times \frac{100 \%}{78.2 \%} = \text{150.9 g}$

M_r: 32.00 18.02

2H₂ + O₂ ⟶ 2H₂O

Moles of H₂O = 150.9 g H₂O × (1 mol H₂O/18.02 g H₂O) = 8.374 mol H₂O

Moles of O₂ = 8.374 mol H₂O × (1 mol O₂/2 mol H₂O) = 4.187 mol O₂

Mass of O₂ = 4.1877 mol O₂ × (32.00 g O₂/1 mol O₂) = 134 g O₂

6 0

3 years ago

Pyrotechnician is a fancy name given to people who make or use

andrey2020 [161]

Answer:

fire

Explanation:

8 0

4 years ago

A chemist dissolves 248mg of pure hydrochloric acid in enough water to make up 140mL of solution.Calculate the pH of the solutio

evablogger [386]

Answer : The pH of the solution is, 1.31

Explanation : Given,

Mass of $HCl$ = 248 mg = 0.248 g (1 mg = 0.001 g)

Volume of solution = 140 mL

Molar mass of $HCl$ = 36.5 g/mole

First we have to calculate the concentration of hydrochloric acid.

Molarity : It is defined as the number of moles of solute present in one liter of volume of solution.

Formula used :

$\text{Molarity}=\frac{\text{Mass of }HCl\times 1000}{\text{Molar mass of }HCl\times \text{Volume of solution (in mL)}}$

Now put all the given values in this formula, we get:

$\text{Molarity}=\frac{0.248g\times 1000}{36.5g/mole\times 140mL}=0.0485mole/L=0.0485M$

The concentration of HCl is, 0.0485 M

As we know that, HCl dissociates to give hydrogen ion and chloride ion.

The dissociation reaction is:

$HCl\rightarrow H^++Cl^-$

Concentration of HCl = Concentration of H⁺ = Concentration of Cl⁻ = 0.0485 M

Now we have to calculate the pH of the solution.

pH : It is defined as the negative logarithm of hydrogen ion concentration.

Mathematically,

$pH=-\log [H^+]$

$pH=-\log (0.0485)$

$pH=1.31$

Therefore, the pH of the solution is, 1.31

6 0

3 years ago