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3 years ago

In order to make a hot pack, do you want to use a chemical that absorbs energy or

Chemistry

1 answer:

ollegr [7]3 years ago

6 0

Answer:

releases energy

Explanation:

In order to make a hot pack, <u>a chemical that releases heat</u> must be used.

<em>A hot pack is typically a pack that is used to applied heat to injured parts of the body during physical activities to relieve pain and reduce swelling. </em>

Hence, in order to make a chemical-based hot pack, a chemical that releases heat when in solution should be used. In order words, a chemical that elicits an exothermic reaction in solution must be used.

This is as opposed to cold packs in which a chemical that absorbs heat has to be used to generate the required coldness to treat injuries.

You might be interested in

Electrons will occupy a p-orbital if the s-orbital is?

DedPeter [7]

Answer:l ectrons will occupy a p orbital only after the s orbital is full

Explanation: Electrons can begin to occupy energy levels with the next highest integer designation only after all of the orbitals on the energy level below it are occupied.

please mark brainliest thank you :)

6 0

3 years ago

The sulfur content of an ore is determined gravimetrically by reacting the ore with concentrated nitric acid and potassium chlor

katen-ka-za [31]

Answer:

13.92 %

Explanation:

Mass of $BaSO_4$ = 12.5221 g

Molar mass of $BaSO_4$ = 233.43 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{12.5221\ g}{233.43\ g/mol}$

Moles of $BaSO_4$ = 0.0536 moles

According to the given reaction,

$Ba^{2+}_{(aq)}+SO_4^{2-}_{(aq)}\rightarrow BaSO_4_{(s)}$

1 mole of $BaSO_4$ is formed from 1 mole of $SO_4^{2-}$

Thus,

0.0536 moles of $BaSO_4$ is formed from 0.0536 moles of $SO_4^{2-}$

Moles of $SO_4^{2-}$ = 0.0536 moles

Moles of sulfur in 1 mole $SO_4^{2-}$ = 1 mole

Moles of sulfur in 0.0536 mole $SO_4^{2-}$ = 0.0536 mole

Molar mass of sulfur = 32.065 g/mol

Mass = Moles * Molar mass = 0.0536 * 32.065 g = 1.7187 g

Mass of ore = 12.3430 g

Mass % = $\frac{Mass\ of\ Sulfur}{Mass_{ore}}\times 100$ = $\frac{1.7187}{12.3430}\times 100$ = 13.92 %

3 0

4 years ago

Question 4 (4 points)

Fiesta28 [93]

I don’t know what is your problem

7 0

3 years ago

What mass of silver oxide, ag2o, is required to produce 25.0 g of silver sulfadiazine, agc10h9n4so2, from the reaction of silver

LenaWriter [7]

Step one write the chemical equation for reaction
= Ag2O + 2(C10H10N4SO2)---> 2 ( AgC10H9N4SO2)

The reacting ratio of Ag2O to AgC10H9N4SO2 is 1:2 from the reaction above

step 2; find the number of moles of AgC10H9N4SO2
that is mass/molar mass
The molar mass of AgC10H9N4SO2 = 107.86 +(12 x10) + (1 x 9) + (4 x 14) +32 +(16 x2) =356.86g/mol
moles is therefore= 25g/356.86g/mol= 0.07moles

by use of mole ratio the moles of Ag2O= 0.0702=0.035moles
mass = moles x molar mass
the molar mass of Ag2O=231.72 g/mol
mass is therefore= 231.72g/mol x 0.035moles= 8.11grams

5 0

3 years ago

If a weaker solution of sodium bicarbonate was used in beaker B, would that solution require more or less acetic acid to neutral

Anarel [89]

Answer is: less acetic acid to neutralize it.

Balanced chemical reaction of sodium bicarbonate solution and acetic acid: NaHCO₃(aq) + CH₃COOH(aq) → CH₃COONa(aq) + H₂O(l) + CO₂(g).

According to chemical reaction: n(NaHCO₃) : n(CH₃COOH) = 1 : 1.

Stronger solution of sodium bicarbonate (NaHCO₃), more acetic acid (CH₃COOH) is neeed for neutralization.

7 0

4 years ago