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3 years ago

Is cornstarch able to disintegrate in fire or an open flame?

Chemistry

2 answers:

Darya [45]3 years ago

7 0

Answer:

Yes

Explanation:

I just quickly looked it up. Cornstarch is extremely flammable.

JulsSmile [24]3 years ago

4 0

Corn starch, like wood, consists of a carbohydrate complex, which is why it burns – but it will only ignite when it is dispersed in air. While it's packed in the container or in a pile on the counter it will not burst into flames due to insufficient oxygen.

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Sodium sulfate dissolves as follows: Na2SO4(s) → 2Na+(aq) + SO42- (aq). How many moles of Na2SO4 are required to make 1.0 L of s

maxonik [38]

Answer: The number of moles of $Na_2SO_4$ is 0.05 moles.

Explanation:

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

We are given:

Molarity of solution = 0.10 mol/L

Volume of solution = 1 L

Putting values in above equation, we get:

$0.10mol/L=\frac{\text{Moles of sodium}}{1.0L}\\\\\text{Moles of sodium}=0.10mol$

The chemical reaction for the ionization of sodium sulfate follows the equation:

$Na_2SO_4(s)\rightarrow 2Na^+(aq.)+SO_4^{2-}(aq.)$

By Stoichiometry of the reaction:

2 moles of sodium ions are produced by 1 mole of sodium sulfate

So, 0.10 moles of sodium ions will be produced by = $\frac{1}{2}\times 0.1=0.05moles$ of sodium sulfate.

Hence, the number of moles of $Na_2SO_4$ is 0.05 moles.

8 0

3 years ago

Using the appropriate ksp value from appendix d in the textbook, calculate the ph of a saturated solution of ca(oh)2 .

Alex777 [14]

The ph of a saturated solution of Ca(OH)2 is 12.35

CALCULATION:
For the reaction
Ca(OH)2 → Ca2+ + 2OH-
we will use the Ksp expression to solve for the concentration [OH-] and then use the acid base concepts to get the pH:
Ksp = [Ca2+][OH-]^2

The listed Ksp value is 5.5 x 10^-6. Substituting this to the Ksp expression, we have
Ksp = 5.5 x 10^-6 = (s) (2s)^2 = 4s^3
s3 = 5.5x10^-6 / 4

Taking the cube root, we now have
s = cube root of (5.5x10^-6 / 4)s
= 0.01112

We know that the value of [OH-] is actually equal to 2s:
[OH-] = 2s = 2 * 0.01112 = 0.02224 M

We can now calculate for pOH:
pOH = - log [OH-]
= -log(0.02224)
= 1.65

Therefore, the pH is
pH = 14 - pOH
= 14 - 1.65
= 12.35

4 0

4 years ago

Question 15 of 20 Which model could represent a neutral atom of nitrogen?

Evgesh-ka [11]

The picture is black

4 0

3 years ago

In the reaction between Lithium Sulfate and an excess of Lead (II) Nitrate, how many molecules of Lithium Nitrate can be expecte

siniylev [52]

Answer:

$1.46x10^{23}molecules \ LiNO_3$

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

$Li_2SO_4 + Pb(NO_3)_2 \rightarrow PbSO_4+2LiNO_3$

Thus, since lead (II) nitrate is in excess, we can directly compute the moles of lithium nitrate by applying the 1:2 molar ratio between them in the chemical reaction as well as the molar mass of Lithium Sulfate that is 110 g/mol for the stoichiometric shown below factor:

$n_{LiNO_3}=13.3gLi_2SO_4*\frac{1molLi_2SO_4}{110gLi_2SO_4} *\frac{2molLiNO_3}{1molLi_2SO_4} =0.242molLiNO_3$