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3 years ago

If solid iron is dropped in liquid iron, it will most likely?

Chemistry

2 answers:

vodka [1.7K]3 years ago

6 0

Answer:sink

Explanation:

S_A_V [24]3 years ago

4 0

it will sink

Explanation:

the solid iron will sink because it is dense than the liquid iron I will sink and it will melt

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Which type of energy refers to the sum of potential and kinetic energies in the particles of a substance?

MrRa [10]

Explanation:

the sum of PE and KE is mechanical energy this means energy during motion and position I think the answer is motion and stored or it may be internal

3 0

3 years ago

Read 2 more answers

What is the enthalpy change when 49.4 ml of 0.430 m sulfuric acid reacts with 23.3 ml of 0.309 m potassium hydroxide?

Leni [432]

Potassium hydroxide commonly known as caustic potash is an inorganic compound with a chemical formula KOH which is a strong base that is marketed in several forms.

H2SO4(aq) + 2KOH(aq) ---> K2SO4(aq) + 2H2O(l) H°= –111.6 kJ/mol

The answer in this question is -0.402 kJ

7 0

4 years ago

From the enthalpies of reaction H2(g)+F2(g)→2HF(g)ΔH=−537kJ C(s)+2F2(g)→CF4(g)ΔH=−680kJ 2C(s)+2H2(g)→C2H4(g)ΔH=+52.3kJ calculate

DIA [1.3K]

Answer:

$\Delta H$ for the given reaction is -2486.3 kJ

Explanation:

The given equation can be written as a combination of the following equation:

$2H_{2}(g)+2F_{2}(g)\rightarrow 4HF(g)$ ; $\Delta H_{1}= (2\times -537kJ)=-1074 kJ$

$2C(s)+4F_{2}(g)\rightarrow 2CF_{4}(g)$ ; $\Delta H_{2}=(2\times -680kJ)=-1360kJ$

$C_{2}H_{4}(g)\rightarrow 2C(s)+2H_{2}(g)$ ; $\Delta H_{3}=-52.3kJ$

-----------------------------------------------------------------------------------

$C_{2}H_{4}(g)+6F_{2}(g)\rightarrow 2CF_{4}(g)+4HF(g)$

$\Delta H=\Delta H_{1}+\Delta H_{2}+\Delta H_{3}=(-1074-1360-52.3)kJ=-2486.3kJ$

6 0

4 years ago

If 11.7 g of aluminum reacts with 37.2 g of copper (II) sulfate according to the following reaction, how many grams of aluminum

zhannawk [14.2K]

Answer:

There is 26.59 grams of aluminium sulfate produced

Explanation:

Step 1: Data given

Mass of aluminium = 11.7 grams

Mass of copper (II) sulfate = 37.2 grams

Molar mass of Aluminium = 26.98 g/mol

Molar mass of CuSO4 = 159.61 g/mol

Molar mass of Al2(SO4)3 = 342.15 g/mol

Step 2: The balanced equation

2Al + 3CuSO4 → Al2(SO4)3 + 3Cu

Step 3: Calculate moles of Aluminium

Moles Al = mass Al / molar mass Al

Moles Al = 11.7 grams / 26.98 g/mol

Moles Al = 0.434 mol

Step 4: Calculate moles of CuSO4

Moles CuSO4 = 37.2 grams / 159.61 g/mol

Moles CuSO4 = 0.233 moles

Step 5: Calculate limiting reactant

For 2 moles of Al we need 3 moles of CuSO4

CuSO4 is the limiting reactant. It will be completely consumed (0.233 moles).

Al is in excess. There will be consumed 0.233 *(2/3) = 0.1553 moles

There will remain 0.434 - 0.1553 = 0.2787 moles

Step 6: Calculate moles of Al2(SO4)3

For 2 moles of Al we need 3 moles of CuSO4, to produce 1 mole of Al2(SO4)3 and 3 moles of Cu

For 0.233 moles CuSO4 we produce 0.233/3 = 0.0777 moles of Al2(SO4)3

Step 7: Calculate mass of Al2(SO4)3

Mass of Al2(SO4)3 = moles Al2(SO4)3 * molar mass Al2(SO4)3

Mass of Al2(SO4)3 = 0.0777 moles * 342.15g/mol

Mass of Al2(SO4)3 = 26.59 grams

There is 26.59 grams of aluminium sulfate produced

4 0

3 years ago

Why are redox reactions often written as net ionic equations?

Scorpion4ik [409]

Answer:

A. To focus on only those ions that form the precipitate

Explanation:

Net ionic equations cancel out the ions that appear on both sides of the reaction because they essentially don't participate in the reaction. This is very useful when dealing with redox reactions because are complicated enough without spectator ions being in the way, so they help focus on those ions that actually form the precipitate.

Key Terms

Spectator Ions: an ion that does not take part in the chemical reaction.
Net ionic equations: a equation where ions that appear on both sides are canceled out.
Redox reaction: an oxidation-reduction reaction.

3 0

3 years ago