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Sphinxa [80]
3 years ago
15

The particles that make up matter do not change during a ?

Chemistry
2 answers:
Bogdan [553]3 years ago
8 0
Matter can only me transformed, but not created or destroyed.
S_A_V [24]3 years ago
6 0
Matter can't be destroyed nor created but only transferred.
You might be interested in
How much heat, in calories, is needed to raise the temperature of 125.0 g of Lead (c lead = 0.130 J/g°C) from 17.5°C to 41.1°C?
pav-90 [236]
95.6 cal
are needed.
Explanation:
Use the following equation:
q
=
m
c
Δ
T
,
where:
q
is heat energy,
m
is mass,
c
is specific heat capacity, and
Δ
T
is the change in temperature.
Δ
T
=
T
final
−
T
initial
Known
m
=
125 g
c
Pb
=
0.130
J
g
⋅
∘
C
T
initial
=
17.5
∘
C
T
final
=
42.1
∘
C
Δ
T
=
42.1
∘
C
−
17.5
∘
C
=
24.6
∘
C
Unknown
q
Solution
Plug the known values into the equation and solve.
q
=
(
125
g
)
×
(
0.130
J
g
⋅
∘
C
)
×
(
24.6
∘
C
)
=
400. J

(rounded to three significant figures)
Convert Joules to calories
1 J
=
0.2389 cal
to four significant figures.
400
.
J
×
0.2389
cal
1
J
=
95.6 cal

(rounded to three significant figures)
95.6 cal
are needed.
8 0
3 years ago
Where are the least reactive elements on the periodic table?
FinnZ [79.3K]
Helium is the least reactive because it has the least protons
8 0
2 years ago
This from ionic compounds escape room​
stira [4]

Answer:

Fe2O3 - S

PbO2 - D

PbO - I

Fe2O - U

Fe(OH)3 - H

FeO2 - T

FeO - R

Pb2O - G

Pb(OH)2 - O

FeOH - N

Pb(OH)3 - A

Explanation:

In writing the formula of ionic compounds we consider the valency or oxidation state of each ion.

For instance, given the compound iron II oxide. The oxidation states of both iron and oxygen are +2 and -2 respectively. Ignoring the charges, this cancels out and we have FeO as the correct formula of the compound.

For Iron III oxide, the oxidation states of iron and oxygen are +3 and -2 respectively, the both atoms exchange charges. If we ignore the signs and write the exchanged numbers as subscripts we obtain the formula Fe2O3.

4 0
2 years ago
Smoke is a homo or hetero
vlabodo [156]

Answer:

it is heterogeneous

Explanation:

3 0
3 years ago
How many grams of N2 can be produced when 6.50 g of O2<br> reacts?
Olenka [21]

Answer:

3.79 g of N2.

Explanation:

We'll begin by writing the balanced equation for the reaction.

This is given below:

4NH3 + 3O2 → 2N2 + 6H2O

Next, we shall determine the mass of O2 that reacted and the mass of N2 produced from the balanced equation.

This is illustrated below:

Molar mass of O2 = 16x2 = 32 g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96 g

Molar mass of N2 = 2x14 = 28 g/mol

Mass of N2 from the balanced equation = 2 x 28 = 56 g

Summary:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Finally, we shall determine the mass of N2 produced by reacting 6.50 g of O2.

This can be obtained as follow:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Therefore, 6.50 g of O2 will react to produce = (6.50 x 56)/96 = 3.79 g of N2.

Therefore, 3.79 g of N2 were obtained from the reaction..

4 0
2 years ago
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