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pickupchik [31]
3 years ago
12

Generally, systems move spontaneously in the direction of increasing entropy. TRUE FALSE

Chemistry
1 answer:
allochka39001 [22]3 years ago
5 0

Answer:

true

Explanation:

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A man threw a Frisbee which weighs 3 kg with a velocity of 5 m/s. What is the KE in the system? *
arsen [322]
The answer would be 8 just took the test
4 0
3 years ago
Which of the following is not a step in balancing redox reactions in acidic solution, using the half-reaction method?
schepotkina [342]
B <span>Divide the chemical equation into two half-reaction equations, identifying which half-reaction is oxidation and which is reduction 
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7 0
3 years ago
Read 2 more answers
Silver nitrate reacts with aluminum chloride to form the insoluble compound, silver chloride. The reaction proceeds according to
viva [34]

The theoretical yield of silver chloride, AgCl is 5.2109 g

The balanced equation for the reaction is given below:

<h3>3AgNO₃(aq) + AICI₃(aq) —> Al(NO₃)₃ (aq) + 3AgCl (s) </h3>

Next, we shall determine the mass of aluminum chloride, AICI₃ that reacted and the mass of silver chloride, AgCl produced from the balanced equation. This is illustrated below:

Molar mass of AICI₃ = 133.34 g/mol

Mass of AICI₃ from the balanced equation = 1 × 133.34 = 133.34 g

Molar mass of AgCl = 143.32 g/mol

Mass of AgCl from the balanced equation = 3 × 143.32 = <em>429.96 g</em>

<h3>SUMMARY</h3>

From the balanced equation above,

133.34 g of AICI₃ reacted to produce 429.96 g of AgCl.

Finally, we shall determine the theoretical yield of AgCl by the reaction of 1.616 g of AICI₃ as follow:

From the balanced equation above,

133.34 g of AICI₃ reacted to produce 429.96 g of AgCl.

Therefore,

1.616 g of AICI₃ will react to produce = \frac{1.616 * 429.96}{133.34} = 5.2109 g of AgCl.

Thus, the theoretical yield of silver chloride, AgCl is 5.2109 g

Learn more: brainly.com/question/24653699

3 0
3 years ago
Calculate the number of kilojoules of energy required to convert 50.0 grams of solid DMSO initially at a temperature of 19.0°C t
GuDViN [60]

Answer:

20.79 kilojoules

Explanation:

Using Q = m×c×∆T

Where;

Q = Quantity of heat (J)

c = specific heat capacity of solid DMSO (1.80 J/g°C)

m = mass of DMSO

∆T = change in temperature

According to the provided information, m= 50g, initial temperature = 19.0°C, final temperature= 250.0°C

Q = m×c×∆T

Q = 50 × 1.80 × (250°C - 19°C)

Q = 90 × 231

Q = 20790 Joules

To convert Joules to kilojoules, we divide by 1000 i.e.

20790/1000

= 20.79 kilojoules

Hence, 20.79 kilojoules of energy is required to convert 50.0 grams of solid DMSO to gas.

4 0
3 years ago
What is the main reason that Absolute Zero has not been achieved under laboratory conditions?
Alexeev081 [22]

Answer:

The reason is because Charle's Law which states that volume is directly proportional to temperature. So, for the temperature to be absolute zero, there would need to be no volume. It's Impossible.

Explanation:

3 0
3 years ago
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