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3 years ago

8 mm = Cm What’s the answer to that???

Chemistry

1 answer:

Vika [28.1K]3 years ago

4 0

Answer:

0.8 cm

Explanation:

If 1mm is 0.1 cm, then

8mm is 0.8 cm since 8 * 0.1 is 0.8

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Heating of glass until it melts what change is it

Natasha2012 [34]

Answer:

physcial change

Explanation:

As it has visible changes on shape and size

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2 years ago

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CaCO3 + 2HCl --> CaCl2 + CO2 + H2O In the reaction above, what mass of carbon dioxide is produced when 10 moles of HCl reacts

puteri [66]

According to the stoichiometry the CO2 formed is 1/2 the moles of H2O. So take the moles of CO2 as 5moles.

n=m/M

Where :

n = mole

m = mass

M = molar mass

Molar mass of CO2 = 44gmol^-1

Therefore mass = 5mol× 44gmol^-1= 220g

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4 years ago

Using the HH eq. calculate the amounts (masses) of sodium phosphate monobasic monohydrate (NaH2PO4 H2O) and sodium phosphate dib

pishuonlain [190]

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3 years ago

Identify which one is the reducing agent in this reaction

Romashka-Z-Leto [24]

Answer:

Na.

Explanation:

The oxidation-reduction reaction contains a reductant and an oxidant (oxidizing agent).

An oxidizing agent, or oxidant, gains electrons and is reduced in a chemical reaction. Also known as the electron acceptor, the oxidizing agent is normally in one of its higher possible oxidation states because it will gain electrons and be reduced.

A reducing agent (also called a reductant or reducer) is an element (such as calcium) or compound that loses (or "donates") an electron to another chemical species in a redox chemical reaction.

For the reaction:

Na is oxidized to Na⁺ in (Na₂S) (loses 1 electron). "reducing agent".

S is reduced to S²⁻ in (Na₂S) (gains 2 electrons). "oxidizing agent".

6 0

3 years ago

When the following oxidation-reduction occurs, what is the balanced reduction half-reaction after the electrons in both half rea

Lostsunrise [7]

Answer : The balanced reduction half-reaction is:

$3Cu^{2+}+6e^-\rightarrow 3Cu$

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

The given balanced redox reaction is :

$Al(s)+Cu^{2+}(aq)\rightarrow Al^{3+}(aq)+Cu(s)$

The half oxidation-reduction reactions are:

Oxidation reaction : $Al\rightarrow Al^{3+}+3e^-$

Reduction reaction : $Cu^{2+}+2e^-\rightarrow Cu$

In order to balance the electrons, we multiply the oxidation reaction by 2 and reduction reaction by 3 and then added both equation, we get the balanced redox reaction.

Oxidation reaction : $2Al\rightarrow 2Al^{3+}+6e^-$

Reduction reaction : $3Cu^{2+}+6e^-\rightarrow 3Cu$

The balanced redox reaction will be:

$2Al(s)+3Cu^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Cu(s)$

Thus, the balanced reduction half-reaction is:

$3Cu^{2+}+6e^-\rightarrow 3Cu$

6 0

3 years ago