All categories

2 years ago

Write the formula of each compound, and determine its molecular (formula) mass:

1 answer:

4 0

the molecular mass of the magnesium nitrite trihydrate will be 170.3 g/mol and the formula for the magnesium nitrite trihydrate will be $Mg(NO_{2})_{2} 3H_{2} O$ .

A molecule's molecular formula reveals which atoms and the number of each kind are included within it. No subscript will be used if there is just one atom of a certain kind. A subscript is added to the symbol for an atom if it contains two or more atoms of a certain type of atom.

Calculation of the molecular mass as:

Molar mass of Magnesium(Mg) = 24.3 g/mol

Molar mass of nitrogen(N) = 14 g/mol

Molar mass of hydrogen(H) = 1 g/mol

Molar mass of oxygen (O)= 16 g/mol

So, the molecular mass of the magnesium nitrite trihydrate will be (24.3×1) + (14×2) + (16×7) + (1×6)= 170.3 g/mol

Therefore, the molecular mass of the magnesium nitrite trihydrate will be 170.3 g/mol.

To know more about formula

brainly.com/question/20748250

#SPJ4

You might be interested in

how many moles of carbon dioxide (CO2) are produced when reacting 6.00 moles of butane (C4H10) in excess oxygen (O2)?

sergeinik [125]

Balance the equation first:

1C4H10 + 13O2 ----> 8CO2 + 10H2O

As we know oxygen is in excess, butane is the limiting reactant.
the ratio between butane and CO2 is 1-8
Therfore
1:8
6:x
x=48
48 moles of CO2 will be produced

8 0

4 years ago

Read 2 more answers

For the following reaction, 28.6 grams of zinc oxide are allowed to react with 9.54 grams of water . zinc oxide(s) water(l) zinc

maw [93]

Answer:

34.9 g of Zn(OH)₂ is the maximum mass that can be formed

Explanation:

Let's state the reaction:

ZnO(s) + H₂O(l) → Zn(OH)₂ (aq)

First of all, we need to determine the moles of each reactant and state the limiting:

28.6 g . 1mol /81.38 g = 0.351 moles of ZnO

9.54 g . 1mol /18 g = 0.53 moles of water

As ratio is 1:1, for 0.53 moles of water, we need 0.53 moles of ZnO, but we only have 0.351, so the limiting reactant is the ZnO.

Ratio with the product is also 1:1. From 0.351 moles of oxide we can produce 0.351 moles of hydroxide. Let's calculate the mass:

0.351 mol . 99.4 g /1mol = 34.9 g

3 0

3 years ago

Write the formula for the compound formed between potassium and sulfur. ks ks2 k2s k2so3 k3s2

Mars2501 [29]

The answer should be K2S

6 0

3 years ago

A chemical company makes pure silver by reacting silver nitrate with Zinc. the company needs to make 800 grams of pure silver fo

kirill115 [55]

Answer:

Yes. Since they have more than the required reactants.

Explanation:

Zinc reduces silver nitrate to silver metal according to the following equation.

2AgNO₃ + Zn → 2Ag + Zn(NO₃)₂

From the equation 2 moles of AgNO₃ produce 2 moles of silver.

If we consider the zinc to be used number of moles=mass/RAM

RAM of zinc =65.38

No. of moles=500/65.38

=7.6476moles

To produce 800 grams of silver they require:

800/107.868 moles=7.4165 moles of silver nitrate since the ratio of silver nitrate to silver produced is 1:1

The number of moles of silver nitrate available=1500/169.872

=8.83 moles.

As the amount of reactants available is more than the required the company will make it in producing the 800 grams of silver required.

3 0

3 years ago

hydrogen and oxygen gas combine to form water. if 1.00g of hydrogen and 1.00g of oxygen are reacted, what is the theoretical yie

AlekseyPX

The equation for the reaction of hydrogen and oxygen is:

$2H_2 + O_2 \rightarrow 2H_2O$

$M_r(H_2) = 2\\\\\therefore n(H_2) = \frac{1}{2}= 0.5mol = n(H_2O)\\\\m(H_2O) = 0.5 \times M(H_2O) = 0.5 \times 18 = 9g$

Thus, the theoretical yield of water is 9 grams.

6 0

3 years ago