All categories

2 years ago

In a chemical reaction, which of the following is true of the products?

Chemistry

2 answers:

zalisa [80]2 years ago

4 0

Your answer would be c I’m pretty sure

a_sh-v [17]2 years ago

4 0

Answer: i think its c

Explanation:

You might be interested in

What does electronegativity measure

Rainbow [258]

Electronegativity is a measure of an atom's ability to attract shared electrons to itself. On the periodic table, electronegativity generally increases as you move from left to right across a period and decreases as you move down a group.

3 0

2 years ago

At a certain temperature this reaction follows second-order kinetics with a rate constant of 14.1·M−1s−1 : →2SO3g+2SO2gO2g Suppo

RoseWind [281]

Answer:

$[SO_3]=0.25M$

Explanation:

Hello there!

In this case, since the integrated rate law for a second-order reaction is:

$[SO_3]=\frac{[SO_3]_0}{1+kt[SO_3]_0}$

Thus, we plug in the initial concentration, rate constant and elapsed time to obtain:

$[SO_3]=\frac{1.44M}{1+14.1M^{-1}s^{-1}*0.240s*1.44M}\\\\$

$[SO_3]=0.25M$

Best regards!

4 0

2 years ago

What are the 3 most important ecosystem services of a coral reef

kkurt [141]

2 Corsls provide treatments

3 0

2 years ago

Read 2 more answers

Working with one sample at a time, add water to the glass one tablespoon at a time. Water should soak the sample from the bottom

Vedmedyk [2.9K]

Answer:

This is confusing

but if you still need help, you can search it online

Explanation:

7 0

2 years ago

Read 2 more answers

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid. HCl(aq), as described by

melisa1 [442]

Answer:

0.88 g

Explanation:

Using ideal gas equation to calculate the moles of chlorine gas produced as:-

$PV=nRT$

where,

P = pressure of the gas = 805 Torr

V = Volume of the gas = 235 mL = 0.235 L

T = Temperature of the gas = $25^oC=[25+273]K=298K$

R = Gas constant = $62.3637\text{torr}mol^{-1}K^{-1}$

n = number of moles of chlorine gas = ?

Putting values in above equation, we get:

$805torr\times 0.235L=n\times 62.3637\text{ torrHg }mol^{-1}K^{-1}\times 298K\\\\n=\frac{805\times 0.235}{62.3637\times 298}=0.01017\ mol$

According to the reaction:-

$MnO_2+4HCl\rightarrow MnCl_2+2H_2O+Cl_2$

1 mole of chlorine gas is produced when 1 mole of manganese dioxide undergoes reaction.

So,

0.01017 mole of chlorine gas is produced when 0.01017 mole of manganese dioxide undergoes reaction.

Moles of $MnO_2$ = 0.01017 moles

Molar mass of $MnO_2$ = 86.93685 g/mol

So,

$Mass=Moles\times Molar\ mass$

Applying values, we get that:-

$Mass=0.01017moles \times 86.93685\ g/mol=0.88\ g$

<u>0.88 g of $MnO_2(s)$ should be added to excess HCl (aq) to obtain 235 mL of $Cl_2(g)$ at 25 degrees C and 805 Torr.</u>

6 0

2 years ago