What is a number at the bottom right of an element in a chemical equation called?

Chemistry

2 answers:

Ann [662]3 years ago

7 0

Answer:

There’s a particular way of writing what’s in a molecule called a chemical formula. The chemical formulae for all the elements that form each molecule and uses a small number to the bottom right of an element’s symbol to stand for the number of atoms of that element. For example, the chemical formula for water is H 2 O.

Explanation:

laila [671]3 years ago

4 0

Answer:an element in a chemical equation is called a subscript.

Explanation:

it represents the the number of atoms of that element present in the compound. hope this helps have a great day yall

You might be interested in

H3PO4 +CaCOH)2=Ca3(PO4)2+H20<br> The equation balance

AnnyKZ [126]

Answer:

2H3PO4 +3Ca(OH) 2 = Ca3 (PO4) 2 +6H20

7 0

3 years ago

An empty steel container is filled with 2.0 atm of H₂ and 1.0 atm of F₂. The system is allowed to reach equilibrium according to

Darina [25.2K]

H₂ (g) + F₂ (g) ⇌ 2 HF (g)

5 0

3 years ago

What is the balanced equation for the reaction of aqueous cesium sulfate and aqueous barium perchlorate?

Aleksandr-060686 [28]

Answer:

The balanced chemical reaction is given as:

$Cs_2SO_4(aq)+Ba(ClO_4)_2(aq)\rightarrow BaSO_4(s)+2CsClO_4(aq)$

Explanation:

When aqueous cesium sulfate and aqueous barium perchlorate are mixed together it gives white precipitate barium sulfate and aqueous solution od cesium perchlorate.

The balanced chemical reaction is given as:

$Cs_2SO_4(aq)+Ba(ClO_4)_2(aq)\rightarrow BaSO_4(s)+2CsClO_4(aq)$

According to reaction, 1 mole of cesium sulfate reacts with 1 mole of barium perchlorate to give 1 mole of a white precipitate of barium sulfate and 2 moles of cesium perchlorate.

3 0

3 years ago

How many grams of lead(II) sulfate (303 g/mol) are needed to react with sodium chromate (162 g/mol) in order to produce 0.162 kg

Afina-wow [57]

Answer : The mass of $PbSO_4$ needed are, 1.515 grams.

Explanation :

First we have to calculate the mole of $PbCrO_4$ .

$\text{Moles of }PbCrO_4=\frac{\text{Mass of }PbCrO_4}{\text{Molar mass of }PbCrO_4}=\frac{0.162g}{323g/mole}=0.005mole$

Now we have to calculate the moles of $PbSO_4$ .

The balanced chemical reaction will be,

$PbSO_4+Na_2CrO_4\rightarrow PbCrO_4+Na_2SO_4[tex]From the balanced chemical reaction, we conclude thatAs, 1 mole of [tex]PbCrO_4$ produced from 1 mole of $PbSO_4$