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3 years ago

If nickel is added to copper sulfate solution, the nickel will replace the copper. write the balanced equation

Chemistry

2 answers:

svp [43]3 years ago

8 0

Ni(s) + CuSO₄(aq) → Cu(s) + NiSO₄(aq)

Ni + Cu²⁺ + SO₄²⁻ → Cu + Ni²⁺ + SO₄²⁻

Ni + Cu²⁺ → Cu + Ni²⁺

Andrew [12]3 years ago

8 0

Answer:-

Ni + CuSO4 --> NiSO4 + Cu

Explanation:-

The symbol for Nickel is Ni.

The Symbol for copper is Cu.

Copper Sulphate has the formula CuSO4.

If Nickel replaces copper from copper sulphate then nickel sulphate is formed.

Nickel sulphate has the formula NiSO4.

So the equation becomes

Ni + CuSO4 --> NiSO4 + Cu

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Nitrogen in plants and soil is changed into nitrogen compounds by _____.

grandymaker [24]

Answer:

Explanation:

because It's the process by which atmospheric nitrogen is converted either by a natural or an industrial means to form of nitrogen such as ammonia.

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3 years ago

Which of the following elements has the largest atomic radius?

kirza4 [7]

Answer:Noble gases:

are highly reactive.

react only with other gases.

do not appear in the periodic table.

are not very reactive with other elements.

Explanation:Noble gases:

are highly reactive.

react only with other gases.

do not appear in the periodic table.

are not very reactive with other elements.

4 0

2 years ago

If the volame ofa gas coetainer at 32°C changes froem 1.55 L to 753 ml, what will the final temperature be? Assume the pressure

motikmotik

Answer : The final temperature of gas will be, 149 K

Explanation :

Charles' Law : It is defined as the volume of gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

$V\propto T$

or,

$\frac{V_1}{V_2}=\frac{T_1}{T_2}$

where,

$V_1$ = initial volume of gas = 1.55 L

$V_2$ = final volume of gas = 753 ml = 0.753 L

$T_1$ = initial temperature of gas = $32^oC=273+32=305K$

$T_2$ = final temperature of gas = ?

Now put all the given values in the above formula, we get the final temperature of the gas.

$\frac{1.55L}{0.753L}=\frac{305K}{T_2}$

$T_2=149K$

Therefore, the final temperature of gas will be, 149 K

7 0

4 years ago

What is the difference between mineral and non-mineral nutrients? provide an example of each.

Alex

The difference between mineral and non-mineral nutrients is that one has minerals and the other doesn’t. For example, an apple and a table. An apple has nutrients, but a table doesn’t lol

3 0

2 years ago

When 2.935 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 9.920 grams of CO2 and 2.031 grams of H

aleksley [76]

Answer: The empirical and molecular formula for the given organic compound are $CH$ and $C_2H_2$ respectively.

Explanation:

The empirical formula is the chemical formula of the simplest ratio of the number of atoms of each element present in a compound.

The chemical equation for the combustion of hydrocarbon having carbon and hydrogen follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of $CO_2$ = 9.920 g

Mass of $H_2O$ = 2.031 g

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 9.920 g of carbon dioxide, $=\frac{12}{44}\times 9.920g=2.705g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 2.031 g of water, $=\frac{2}{18}\times 2.031g=0.226g$ of hydrogen will be contained.

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Molar mass of C = 12 g/mol

Molar mass of H = 1 g/mol

Putting values in equation 1, we get:

$\text{Moles of C}=\frac{2.705g}{12g/mol}=0.225 mol$

$\text{Moles of H}=\frac{0.226g}{1g/mol}=0.226 mol$

Step 2: Calculating the mole ratio of the given elements.

Calculating the mole fraction of each element by dividing the calculated moles by the least calculated number of moles that is 0.225 moles

$\text{Mole fraction of C}=\frac{0.224}{0.225}=1$

$\text{Mole fraction of H}=\frac{0.226}{0.225}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H = 1 : 1

The empirical formula of the compound becomes $K_1Mn_1O_4=KMnO_4$

To calculate the molecular formula, the number of atoms of the empirical formula is multiplied by a factor known as valency that is represented by the symbol, 'n'.

$n =\frac{\text{Molecular mass}}{\text{Empirical mass}}$ .....(2)

We are given:

Mass of molecular formula = 26.04 g/mol

Mass of empirical formula = 13 g/mol

Putting values in equation 3, we get:

$n=\frac{26.04g/mol}{13g/mol}=2$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{1\times 2}H_{1\times 2}=C_2H_2$

Hence, the empirical and molecular formula for the given organic compound are $CH$ and $C_2H_2$ respectively.

7 0

3 years ago