All categories

4 years ago

How is stoichiometry used to calculate the amount of products

1 answer:

7 0

Stoichiometry measures the quantitative relationships, and is used to determine the amounts of products and reactants that are produced or needed in a given reaction

You might be interested in

Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.57×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.46×10−19, what is the equilib

Dvinal [7]

Answer: The value of $K_c$ for the final reaction is $7.16\times 10^{25}$

Explanation:

The given chemical equations follows:

Equation 1: $H_2S(aq.)\rightleftharpoons HS^-(aq.)+H^(aq.);K_1$

Equation 2: $HS^-(aq.)\rightleftharpoons S^{2-}(aq.)+H^(aq.);K_2$

The net equation follows:

$S^{2-}(aq.)+2H^+(aq.)\rightleftharpoons H_2S(aq.);K_c$

As, the net reaction is the result of the addition of reverse of first equation and the reverse of second equation. So, the equilibrium constant for the net reaction will be the multiplication of inverse of first equilibrium constant and the inverse of second equilibrium constant.

The value of equilibrium constant for net reaction is:

$K_c=\frac{1}{K_1}\times \frac{1}{K_2}$

We are given:

$K_1=9.57\times 10^{-8}$

$K_2=1.46\times 10^{-19}$

Putting values in above equation, we get:

$K_c=\frac{1}{(9.57\times 10^{-8})}\times \frac{1}{(1.46\times 10^{-19})}=7.16\times 10^{25}$

Hence, the value of $K_c$ for the final reaction is $7.16\times 10^{25}$

5 0

3 years ago

Balance the following equation H2S+SO2➡️S+H2O

grin007 [14]

2H2S+2SO2 》》 4S+2H2O hope that'll help u

8 0

4 years ago

The density of silver is 10.5 g/cm3. what would be the mass (in grams) of a piece of silver that occupies a volume of 23.6 cm3?

Keith_Richards [23]

Hey there : !

density = 10.5 g/cm³

volume = 23.6 cm³

therefore:

D = m / V

10.5 = m / 23.6

m = 10.5 * 23.6

m = 247.8 g

hope this helps!

6 0

3 years ago

Read 2 more answers

BRAINLIESTTT ASAP!! PLEASE HELP ME :)

AlladinOne [14]

Answer : False, there will be two lithium and one oxygen atoms in a unit molecular structure of lithium oxide.

Explanation:

Electronic configuration of lithium is :

$Li=1s^2s^1$

In order to attain stable electronic configuration it will loose an electron and form positively charge cation.

$Li^+=1s^22s^0$

The electronic configuration of oxygen is:

$O=1s^22s^22p^4$

Oxygen being second most electronegative atom requires two electrons to attain noble gas configuration stability and form negatively charge ion with 2- charge.:

$O^{2-}=1s^22s^22p^6$

When two atom of lithium and oxygen comes together , one electron from each lithium atom get transferred to an oxygen atom which results in formation of lithium oxide.

$2Li^++O^{2-}\rightarrow Li_2O$

4 0

3 years ago

Read 2 more answers

What mass percent solution will result from dissolving 0.126 moles of AgNO3 in 475 g. of water

Kruka [31]

Answer:

The answer to your question is: 4.5 %

Explanation:

0.126 moles of AgNO3

mass percent = ?

mass of water = 475 g

Formula

weight percent = weight of solute / weight of solution x 100

Weight of solute

MW AgNO3 = 108 + 14 + (16 x 3)

= 108 + 14 + 48

= 170 g

170 g of AgNO3 ------------------- 1 mol

x --------------------- 0.126 moles

x = (0.126 x 170) / 1 = 21.42 g of AgNO3

Weight percent = 21.42/475 x 100

= 4.5 %

7 0

3 years ago