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crimeas [40]
3 years ago
14

What type of reaction is represented by the following example? 2CO2 (g) + 4H2O (l) + 1452 kJ 2CH3OH (l) (g) + 3O2 (g) exothermic

endothermic
Chemistry
2 answers:
Elodia [21]3 years ago
8 0

endothermic  

I hope this helped :)

CaHeK987 [17]3 years ago
7 0

Answer : The given reaction is an example of endothermic reaction.

Explanation :

Endothermic reaction : It is a type of chemical reaction in which the energy is absorbed by the surroundings. In this reaction, the energy of reactants are less than the energy of products.  In this reaction, the energy is given to the system.

Exothermic reaction : It is a type of chemical reaction in which the energy is released into the surroundings. In this reaction, the energy of reactants are more than the energy of products. In this reaction, the energy is released from the system.

The given balanced chemical reaction is,

2CO_2(g)+4H_2O(l)+1452KJ\rightarrow 2CH_3OH(l)+3O_2(g)

In this reaction, the 1452 KJ energy is given to the system. So, the given reaction is an example of endothermic reaction.

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A pure copper penny contains approximately 2.9×1022 copper atoms. Use the following definitions to determine how many ______ of
hammer [34]

Complete question is;

A pure copper penny contains approximately 2.9 × 10^(22) copper atoms.

1 doz = 12

1 gross = 144

1 ream = 500

1 mol = 6.022 × 10^(23)

Use these definitions to determine the following:

A) How many dozens of copper atoms are in a penny.

B) How many gross of copper atoms are in a penny

C) How many reams of copper atoms are in a penny.

D) how many moles of copper atoms are in a penny?

All answers can be rounded to two significant figures

Answer:

A) 2.4 × 10^(21) dozens

B) 2.01 × 10^(20) gross

C) 5.8 × 10^(19) reams

D) 0.048 mol

Explanation:

A) A dozen contains 12.

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/12 dozens = 2.42 × 10^(21).

In 2 significant figures, we have;

2.4 × 10^(21) dozens

B) 1 gross = 144

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/144 gross ≈ 2.01 × 10^(20) gross

C) 1 ream = 500

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/500 reams = 5.8 × 10^(19) reams

D) 1 mol = 6.022 × 10^(23)

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/(6.022 × 10^(23)) = 0.048 mol

6 0
3 years ago
How many g of silver chloride will be produced by reacting 10g of silver nitrate with sodium chloride?
I am Lyosha [343]

Answer:

16.8 g of AgCl are produced

Explanation:

The reactants are: NaCl and AgNO₃

The products are:  AgCl, NaNO₃

Balanced equation:  NaCl(aq) +  AgNO₃(aq)  → NaNO₃(aq) + AgCl(s) ↓

We convert the mass of AgNO₃ to moles → 10 g / 85g/mol = 0.117 moles

Ratio is 1:1, therefore 0.117 moles of nitrate will produce 0.117 moles of AgCl.

According to stoichiormetry.

We convert the moles to mass → 0.117 mol . 143.3g /1mol = 16.8 g

7 0
3 years ago
Read 2 more answers
What is the mass of a 1.00 l sample of a liquid that has a density of 0.967 g/ml ? express your answer using three significant f
BARSIC [14]

Mass = 1000 mL x 0.967 g/1 mL = 967 g

5 0
3 years ago
5. How do scientists analyze the TRAPPIST system? Write two key ideas. Work with a partner.
pentagon [3]

Answer:

They start with the planet furthest from us then go down the line of how many miles from us it is. Mars and Venus are the closests to us.

Explanation:

Its showing miles away it is and how fast it rotates and scientists study and analyze that.

5 0
3 years ago
You are given 25.00 mL of an acetic acid solution of unknown concentration. You find it requires 35.75 mL of a 0.1950 M NaOH sol
oee [108]

Answer:

0.2788 M

1.674 %(m/V)

Explanation:

Step 1: Write the balanced equation

NaOH + CH₃COOH → CH₃COONa + H₂O

Step 2: Calculate the reacting moles of NaOH

0.03575 L \times \frac{0.1950mol}{L} = 6.971 \times 10^{-3} mol

Step 3: Calculate the reacting moles of CH₃COOH

The molar ratio of NaOH to CH₃COOH is 1:1.

6.971 \times 10^{-3} molNaOH \times \frac{1molCH_3COOH}{1molNaOH} = 6.971 \times 10^{-3} molCH_3COOH

Step 4: Calculate the molarity of the acetic acid solution

M = \frac{6.971 \times 10^{-3} mol}{0.02500L} =0.2788 M

Step 5: Calculate the mass of acetic acid

The molar mass of acetic acid is 60.05 g/mol.

6.971 \times 10^{-3} mol \times \frac{60.05g}{mol} =0.4186 g

Step 6: Calculate the percentage of acetic acid in the solution

\frac{0.4186g}{25.00mL}  \times 100\% = 1.674 \%(m/V)

6 0
3 years ago
Read 2 more answers
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