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3 years ago

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What does it mean if a substance is insoluble? A. It does not dissolve. B. It dissolves in another substance. C. It makes new mo

lecules. D. It creates a new compound.

1 answer:

hodyreva [135]3 years ago

8 0

Answer:

A because insoluble man's it cannot be dissolved

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A person slips over banana pills. Give reason

zhenek [66]

Answer:

We slip when we step on a banana peel because the inner side of banana peel being smooth and slippery reduces the friction between the sole of our shoe and the surface of road.

8 0

3 years ago

Which equation represents the reaction of a weak acid with water?

shusha [124]

Acid is anything which will give H+ to other species.

Have a look at the equations given.

In A) HCl changes to Cl- by giving its H+ to H2O. So HCl is an acid.

In B) HCO3- changes to H2CO3^2- by accepting H+. It did Not give its H+ rather it takes from other species. So it is not an acid at all.

In C) H2O is just breaking to H+ and OH-. It is not giving H+ to other species. So it is also not an acid in this reaction.

In D) HCOOH is giving its H+ to H2O. So it is also an acid.

So out of all reactions with water. The only two species are acting as acid with water namely HCl and HCOOH.

Out of these two HCl is very strong acid but HCOOH is a weak acid.

So the answer is D

6 0

3 years ago

Read 2 more answers

From the balanced reaction below, when you have 3.33 moles of (NH4)2Cr2O7, how many grams of N2 will be produced

natima [27]

Answer:

$m_{N_2}=93.3gN_2$

Explanation:

Hello there!

In this case, for this stoichiometry-based problem, it is firstly necessary to realize that the decomposition of ammonium dichromate is given by:

$(NH_4)_2Cr_2O_7(s)\rightarrow N_2(g)+4H_2O(l)+Cr_2O_3(s)$

Thus, since the mole ratio between ammonium dichromate and the gaseous nitrogen (molar mass = 28.02 g/mol) is 1:1, we can compute the produced mass of the latter via stoichiometry as shown below:

$m_{N_2}=3.33mol(NH_4)_2Cr_2O_7*\frac{1molN_2}{1mol(NH_4)_2Cr_2O_7}*\frac{28.01gN_2}{1molN_2}\\\\ m_{N_2}=93.3gN_2$

Best regards!

3 0

3 years ago

Need help with this question

Veseljchak [2.6K]

Answer: last one

Explanation:

5 0

3 years ago

The following reaction has Kp = 109 at 25°C. 2 NO(g) + Br2(g) equilibrium reaction arrow 2 NOBr(g) If the equilibrium partial pr

kati45 [8]

<u>Answer:</u> The equilibrium partial pressure of NO is 0.0034 atm

<u>Explanation:</u>

For the given chemical equation:

$NO(g)+Br_2(g)\rightleftharpoons 2NOBr(g)$

The expression of $K_p$ for above equation follows:

$K_p=\frac{(p_{NOBr})^2}{p_{NO}\times p_{Br_2}}$

We are given:

Equilibrium partial pressure of $Br_2$ = 0.0159 atm

Equilibrium partial pressure of NOBr = 0.0768 atm

$K_p=109$

Putting values in above equation, we get:

$109=\frac{(0.0768)^2}{p_{NO}\times 0.0159}\\\\p_{NO}=0.0034atm$

Hence, the equilibrium partial pressure of NO is 0.0034 atm

3 0

3 years ago