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larisa [96]
3 years ago
6

The reactants of photosynthesis are

Chemistry
1 answer:
Levart [38]3 years ago
7 0
Carbón dioxide and water
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Four students all do the same experiment for the science fair. They test reaction times for pushing a button when a specific col
dsp73

The order of the students from the most reliable to the least reliable is C. Student 4, Student 1, Student 2, Student 3.

<h3>what student has the most reliable data?</h3><h3 />

the student with the most reliable data is the one that has the least variation in their data in the various trials.

this student is therefore student 4.

the next student would be student 1 and student 2 would be the third most reliable.

student 3 has large variations in their trials which makes their data the least reliable.

find out more on reliable data at brainly.com/question/8391667.

#SPJ1

7 0
2 years ago
Determine the percent water in MgSO4*7H20?
Semmy [17]

Answer:

\% H_2O=51.2\%

Explanation:

Hello!

In this case, since the percent water is computed by dividing the amount of water by the total mass of the hydrate; we infer we first need the molar mass of water and that of the hydrate as shown below:

MM_{MgSO_4* 7H_2O}=120.36 g/mol+7*18.02g/mol\\\\MM_{MgSO_4* 7H_2O}=246.5g/mol

Thus, the percent water is:

\% H_2O=\frac{7*MM_{H_2O}}{MM_{MgSO_4* 7H_2O}} *100\%\\\\

So we plug in to obtain:

\% H_2O=\frac{7*18.02}{246.5} *100\%\\\\\% H_2O=51.2\%

Best regards!

5 0
3 years ago
the valence electrons of an atom of which element would feel a smaller effective nuclear charge than the valence electrons of a
Dvinal [7]
D. Strontium is the right answer
5 0
3 years ago
A. CH,0, molar mass is 90 g/mol
Luba_88 [7]

what is that i cant see anything?

7 0
3 years ago
A 100.0 mL solution containing 0.864 g of maleic acid (MW=116.072 g/mol) is titrated with 0.276 M KOH. Calculate the pH of the s
Lilit [14]

Answer:

pH = 1.32

Explanation:

                 H₂M + KOH ------------------------ HM⁻ + H₂O + K⁺

This problem involves a weak diprotic acid which we can solve by realizing they amount  to buffer solutions.  In the first  deprotonation if all the acid is not consumed we will have an equilibrium of a wak acid and its weak conjugate base. Lets see:

So first calculate the moles reacted and produced:

n H₂M = 0.864 g/mol x 1 mol/ 116.072 g  =  0.074 mol H₂M

54 mL x  1L / 1000 mL x 0. 0.276 moles/L = 0.015 mol KOH

it is clear that the maleic acid will not be completely consumed, hence treat it as an equilibrium problem of a buffer solution.

moles H₂M left = 0.074 - 0.015 = 0.059

moles HM⁻ produced = 0.015

Using the Henderson - Hasselbach equation to solve for pH:

ph = pKₐ + log ( HM⁻/ HA) = 1.92 + log ( 0.015 / 0.059) = 1.325

Notes: In the HH equation we used the moles of the species since the volume is the same and they will cancel out in the quotient.

For polyprotic acids the second or third deprotonation contribution to the pH when there is still unreacted acid ( Maleic in this case) unreacted.

           

3 0
3 years ago
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