Ask question

Ask question

All categories

oksano4ka [1.4K]

3 years ago

7

Identify the reagents represented by the letters in the above reaction scheme. (enter your answer as a string of letters without

punctuation,
e.g. abcd.)

1 answer:

MAXImum [283]3 years ago

7 0

Please show the whole question including the diagram so that you can receive help with the question.

You might be interested in

An element X exists in three forms A, B and C in the ratio 1:2:3. If C has 10 protonsand the number of neutrons in A, B and C ar

Strike441 [17]

x21 +ANSWER

(i) Ne-22

(ii)1s2s22p6

(iii)21.3

An element X exists in three forms A, B and C in the ratio 1:2:3. If C has 10 protons and the number of neutrons in A, B and C are 10, 11 and 12 respectively,Give the following:(i) Representation of form C of the element X(ii) Electronic configuration of form B of the element(iii) Calculate the average atomic mass.

(i)C has 10 protons and 12 neutrons so a mass of 10 +12 =22

element 10 is Neon (Ne) so this isotope is Ne-22

(ii) they all have the sane atomic number so the same number of electrons

with an electronic structure of 1s2s22p6

(iii) A weighs 20, B weighs 21, C weighs 22

the ratio is 1:2:3

weighted average weight is therefor

(1X20 +2X21 +3X22)/6 =21.3

4 0

3 years ago

A 5.50 gram sample of C2H6 gas has a volume of 2.50 L. If the sample is at 41.20C, what will it’s pressure be?

vovangra [49]

Multiple them divided by 2.50

8 0

3 years ago

What is the temperature when ice Melt

kenny6666 [7]

The temperature when ice melts is 32 degrees Fahrenheit.

6 0

4 years ago

In an experiment designed to determine the concentration of Cu 2 ions in an unknown solution, you need to prepare 100 mL of 0.10

Alexxandr [17]

Answer:

1.6 grams

Explanation:

We need to prepare 100 mL (0.100 L) of a 0.10 M CuSO₄ solution. The required moles of CuSO₄ are:

0.100 L × 0.10 mol/L = 0.010 mol

The molar mass of CuSO₄ is 159.61 g/mol. The mass corresponding to 0.010 moles is:

0.010 mol × (159.61 g/mol) = 1.6 g

We should use 1.6 grams of CuSO₄.

8 0

3 years ago

A chemist titrates 150.0 mL of a 0.2653 M carbonic acid (H2CO3) solution with 0.2196 M NaOH solution at 25 °C. Calculate the pH

xxTIMURxx [149]

Answer:

9.3

Explanation:

This is long and complicated so get ready

We are going to use the conjugate base of carbonic acid with water to make carbonic acid and OH- (Na is simply a spectator ion and is irrelavent here)

Let the conjugate base be A- and Carbonic acid be HA

A- + H20 ⇄ HA + OH-

To find the concentration of A- we must find the concentration of the reactants given. We know this will be equal because it is a strong base and all of it disassociates.

to get moles of acid we take the concentration and multiply by liters to cancel

.2653 x .150 = .039795 mol HA

Because it is at equivalence point we know the moles will be equal. We are given the concentration so we only have to solve for liters

We plug it into the equation and found: .181 L

Now use moles and combined volums to fins concentrarion which is .120 M

Now plug that use the Ka converted to Kb to find the cincentrations of HA and OH-

Ka is (10^-3.60) = 2.4E-4

Kb x Ka is 10^-14

Kb = 3.98E-11

Now we know Kb = [HA] [OH] / [A-]

Solve for this through algebra by using x for the values you dont know

youll find x^2 = 3.3E-10

X = 1.8 E -5

this is the OH- concentration

-log [oh] = pOH

pOH = 4.73

We know 14-pOH = ph so pH= 9.3

6 0

3 years ago