Which structure represents a ribosome?<br> Choose 1 answer:

Write balanced chemical equations for the following reactions.

VLD [36.1K]

❃ The following points should be kept in mind to write and balance a chemical equation :

Step 1 : Write the molecular formula of all the reactants and products correctly.

Step 2 : Separate reactants and products by a sign of arrow. If reactants or products are more than one, connect them by a sign of a plus.

Step 3 : Balance the atoms of O and H at last [ The atoms used at many places in an equation should be balanced at last ]. For balancing , the number should be added as coefficient i.e in the front of the molecules.

[ Remember those substance that take part in a chemical reaction are called reactants. Likewise , those substances which are formed after a chemical reaction are called products ]

$\large{ \tt{❁ \: LET'S \: GET \: STARTED}} :$

1. Carbon disulfide + Oxygen gas gives carbon dioxide + Sulfur dioxide.

Step 1 : The molecular formula of carbon disulfide is CS₂ , molecular formula of Oxygen gas is 0₂ [ Since oxygen is a diatomic element ] molecular formula of carbon dioxide is CO₂ and molecular formula of sulfur dioxide is SO₂.

Step 2 : CS₂ + O₂ ⟶ CO₂ + SO₂

Step 3 : In the reactant side , there is two ' S ' but on the other side , there is one ' S '. So , add 2 as a coefficient before S on the product side. Now , There are two ' O ' in the reactant side but six ' O ' in the product side. So , add 3 as a coefficient before O on the reactant side. Now , there are equal atom of C , S and O on both sides

i.e CS₂ + 3O₂ ⟶ CO₂ + 2SO₂

Answer : $\boxed{ \tt{CS₂ + 3O₂ ⟶ CO₂ + 2SO₂}}$

-----------------------------------------

2. Silver + nitric acid gives silver nitrate + nitrogen dioxide + water

Step 1 : The molecular formula of Silver is Ag, molecular formula of nitric acid is HNO₃ , molecular formula of Silver nitrate is Ag ( No₃ ) , molecular formula of nitrogen dioxide is NO₂ and molecular formula of water is H₂O.

Step 2 : Ag + HNO₃ ⟶ Ag ( NO₃ ) + NO₂ + H₂O

Step 3 : In the reactant side , There is one ' H ' but on the other side , there are two ' H '. Now add 2 before H on the reactant side. There are equal atom of ' Ag ' , ' H ' , ' N ' , and ' O '.

i.e Ag + 2HNO₃ ⟶ Ag ( NO₃ ) + NO₂ + H₂O

Answer : $\boxed{ \tt{Ag + 2HNO₃ ⟶ Ag ( NO₃ ) + NO₂ + H₂O }}$

Yay! We're done ! :)

- The last step is a bit more confusing I guess. So , which balancing , count the atoms in following ways :

The number written at the right lower corner of an atom is counted for that atom only. For example : In MgSO₄ , there are one ' Mg ' , one ' S ' and four ' O '

The number written at the right lower corner of a bracket is for all the atoms enclosed in the bracket. For example : In Al₂ ( SiO₃ ) has two Al , three ' S ' and nine ' O '.

The coefficient number is for all the atoms of the molecule. For example , in 2 Al ₂( SiO₃ )₃ , there are four ' Al ' , six ' Al ' and eighteen ' O '.

- Hope this helps! :)

4 0

3 years ago

Read 2 more answers

A tank of water was contaminated with a colored dye (D). To determine the concentration of D, an analyst took 5.0-mL solution fr

alekssr [168]

Answer:

0.005 M

Explanation:

Given data:

volume of sample solution ( volume of D ) = 5.0 mL

volume of added stock solution ( V1 ) = 5.0 mL

concentration of added stock solution ( N1 ) = 0.02 M

Total volume of concentration ( V2 )= 10 mL = ( 5.0 mL + 5.0mL)

concentration of Total volume of sample ( C2 ) = 0.01

N2 = ( N1V1 ) / V2

= ( 0.02 * 5 ) / 10 = 0.01 m

absorbance of sample solution ( A1 ) = 0.10

absorbance of additional sample solution ( A2 ) = 0.20

attached below is the remaining part of the detailed solution

3 0

3 years ago

How many grams of carbon monoxide are needed to react with an excess of iron (III) oxide to produce 198.5 grams of iron? Fe2O3(s

erastova [34]

Answer : The grams of carbon monoxide needed are 148.89 g

Solution : Given,

Mass of iron, Fe = 198.5 g

Molar mass of iron, Fe = 56 g/mole

Molar mass of carbon monoxide, CO = 28 g/mole

First we have to calculate the moles of iron, Fe.

$\text{ Moles of Fe}=\frac{\text{ Mass of Fe}}{\text{ Molar mass of Fe}}=\frac{198.5g}{56g/mole}=3.545moles$

The balanced chemical reaction is,

$Fe_2O_3(s)+3CO(g)\rightarrow 3CO_2(g)+2Fe(s)$

From the balanced reaction, we conclude that

2 moles of iron produces from the 3 moles of carbon monoxide

3.545 moles of iron produces from the $\frac{3}{2}\times 3.545=5.3175$ moles of carbon monoxide

Now we have to calculate the mass of carbon monoxide, CO.

$\text{ Mass of CO}=\text{ Moles of CO}\times \text{ Molar mass of CO}$

$\text{ Mass of CO}=(5.3175moles)\times (28g/mole)=148.89g$

Therefore, the grams of carbon monoxide needed are 148.89 g

7 0

3 years ago

What is a heterogenous mixture?

Nezavi [6.7K]

Answer: a heterogenous mixture is simply any mixture that is not uniform in composition- its non-uniform mixture of smaller constituent parts

Explanation:

8 0

3 years ago

Write the molecular formula for a compound with the possible elements C, H, N and O that exhibits a molecular ion at M

liberstina [14]

Answer:

$= \mathbf{C_3H_6O}$

Explanation:

From the given information, since the molecular mass of the ion M+ is not given;

Let's assume M+ = 58.0423

So, by applying the 13th rule;

we will need to divide the mass by 13, after dividing it;

The quotient n = no. of carbon; &

The addition of the quotient (n) with the remainder r = no. of hydrogen.

So;

$\dfrac{58}{13}= 4 \ remainder \ 6$

So;

$C_nH_{n+r} = C_4H_{4+6}$

$= C_4H_{10}$

From the given information; we have oxygen present, so since the mass of oxygen = 16, we put oxygen in the molecular formula by removing $CH_4$ . Also, since the mass is an even number then Nitrogen is 0.

So, we have:

$= \mathbf{C_3H_6O}$

6 0

3 years ago

Which structure represents a ribosome? Choose 1 answer: