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OleMash [197]
3 years ago
10

What type of reaction is illustrated? C + 2F2 → CF4

Chemistry
2 answers:
ludmilkaskok [199]3 years ago
4 0

Answer:

Synthesis Reaction

Explanation:

An synthesis reaction is one in which two or more atoms/molecules react to create a different molecule. These reactions follow the general structure: A + B --> AB.

More specifically, this is an addition reaction. An addition reaction occurs when two or more atoms/molecules combine to create a larger molecule. In this case, carbon and fluorine react to form carbon tetrafluoride, a larger molecule consisting of all the reactants.

This is not a decomposition reaction because these reactions involve a molecule breaking down into atoms or simpler molecules. These reactions follow the general structure: AB --> A + B.

This is not a single-replacement reaction because these reactions involve atoms replacing atoms of a different element in a compound. These reactions follow the general structure: A + BX --> B + AX.

kifflom [539]3 years ago
3 0
I believe it is a redox reaction
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Which of the following describes a solution of 1 gram of salt dissolved in 500 mL of water?
Law Incorporation [45]

Answer:

B

Explanation

Salt water is a solution where the salt completely dissolves therefore is is homogeneous. Solvent is the liquid (water) that dissolves the solute (salt).

3 0
3 years ago
Read 2 more answers
Please someone help meeeeee!!!
Lorico [155]

Answer:

1 = Q =  7315 j

2 =Q =  -21937.5 j

Explanation:

Given data:

Mass of water = 50 g

Initial temperature = 20°C

Final temperature = 55°C

Energy required to change the temperature = ?

Solution:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Specific heat capacity of water is 4.18 j/g.°C.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = T2 - T1

ΔT = 55°C - 20°C

ΔT = 35°C

Q = 50 g× 4.18 j/g.°C×35°C

Q =  7315 j

Q 2:

Given data:

Mass of metal = 100 g

Initial temperature = 1000°C

Final temperature = 25°C

Energy released = ?

Specific heat capacity = 0.225 j/g.°C

Solution:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = T2 - T1

ΔT = 25°C - 1000°C

ΔT = -975°C

Now we will put the values in formula.

Q = 100 g × 0.225 j/g.°C × -975°C

Q =  -21937.5 j

Negative sign show that energy is released.

7 0
3 years ago
What mass of hydrochloric acid (in grams) can 2.7 g of sodium bicarbonate neutralize? (Hint: Begin by writing a balanced equatio
Julli [10]

Answer:

1.17 grams of HCl can neutralize 2.7 grams sodium bicarbonate

Explanation:

Step 1: Data given

Mass of sodium bicarbonate = 2.7 grams

Step 2: The balanced equation

HCl + NaHCO3 ⇔  NaCl + H2O + CO2

Step 3: Calculate moles NaHCO3

moles NaHCO3 =2.7 g / 84 g/mol= 0.032 moles

Step 4: Calculate moles HCl

For 1 mol NaHCO3 we need 1 mol HCl

For 0.032 moles NaHCO3 = 0.032 moles HCl

Step 5: Calculate mass HCl

Mass HCl = moles HCl * molar mass HCl

mass HCl = 0.032 * 36.46 g/mol= 1.17 grams

1.17 grams of HCl can neutralize 2.7 grams sodium bicarbonate

3 0
4 years ago
What is plasama?.......​
Andrej [43]

Explanation:

Plasma is the clear, straw-colored liquid portion of blood that remains after red blood cells, white blood cells, platelets and other cellular components are removed. It is the single largest component of human blood, comprising about 55 percent, and contains water, salts, enzymes, antibodies and other proteins.

5 0
3 years ago
Read 2 more answers
A chemical compound has a molecular weight of 89.05 g/mole. 1.400 grams of this compound underwent complete combustion under con
Nataly_w [17]

Answer:

\Delta _{comb}H=-2,265\frac{kJ}{mol}

Explanation:

Hello!

In this case, for such calorimetry problem, we can notice that the combustion of the compound releases the heat which causes the increase of the temperature by 11.95 °C, it means that we can write:

Q _{comb}=-C_{calorimeter}\Delta T_{calorimeter}

In such a way, we can compute the total released heat due to the combustion considering the calorimeter specific heat and the temperature raise:

Q _{comb}=-2980\frac{J}{\°C} *11.95\°C\\\\Q _{comb}=-35,611J

Next, we compute the molar heat of combustion of the compound by dividing by the moles, considering 1.400 g were combusted:

n=1.400g*\frac{1mol}{89.05g} =0.01572mol

Thus, we obtain:

\Delta _{comb}H=\frac{Q_{comb}}{n}=\frac{-35,611J}{0.01572mol}  \\\\\Delta _{comb}H=-2,265,331\frac{J}{mol}*\frac{1kJ}{1000J}  \\\\\Delta _{comb}H=-2,265\frac{kJ}{mol}

Best regards!

7 0
3 years ago
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