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3 years ago

Just vibin yall how about you

Chemistry

2 answers:

Misha Larkins [42]3 years ago

8 0

Answer:

<h2>hyy mate imm need friend I didn't have any friend can you my friend^_^</h2>

Explanation:

Inspired by the McCarthy hearings of the 1950s, Arthur Miller's play, The Crucible, focuses on the inconsistencies of the Salem witch trials and the extreme behavior that can result from dark desires and hidden agendas.

and women

Vlada [557]3 years ago

4 0

Answer:

Not much just operating brainly and waiting for my friends :)

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How many joules of energy are required to melt 423g of water at 0°C?

Mkey [24]

The amount of heat needed to melt 423 g of water at 0°C is 141282 J

The heat required to melt water can be obtained by using the following formula:

Q is the heat required.

L is the latent heat of fusion (334 J/g)

m is the mass.

With the above formula, we can obtain the heat required to melt the water as illustrated below:

Mass of water (m) = 423 g

Latent heat of fusion (L) = 334 J/g

<h3>Heat (Q) required =? </h3>

Q = mL

Q = 423 × 334

Therefore, the amount of heat needed to melt 423 g of water at 0°C is 141282 J

Learn more: brainly.com/question/17084080

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3 years ago

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The process which plants use to make food is called:

riadik2000 [5.3K]

The answer is Photosynthesis!

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4 years ago

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Consider the diphenyl boron group as a substituent on abenzene

sergij07 [2.7K]

Answer:

Please see attachment

Explanation:

Please see attachment

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3 years ago

The balanced combustion reaction for C 6 H 6 C6H6 is 2 C 6 H 6 ( l ) + 15 O 2 ( g ) ⟶ 12 CO 2 ( g ) + 6 H 2 O ( l ) + 6542 kJ 2C

Lana71 [14]

Explanation:

First, we will calculate the molar mass of $C_{6}H_{6}$ as follows.

Molar mass of $C_{6}H_{6}$ = $6 \times 12 + 6 \times 1$

= 78 g/mol

So, when 2 mol of $C_{2}H{6}$ burns, then heat produced = 6542 KJ

Hence, this means that 2 molecules of $C_{6}H{6}$ are equal to $78 \times 2 = 156 g$ of $C_{6}H_{6}$ burns, heat produced = 6542 KJ

Therefore, heat produced by burning 5.5 g of $C_{6}H{6}$ =

$6542 kJ \times \frac{5.5 g}{156 g}$

= 228.97 kJ

= 228970 J (as 1 kJ = 1000 J)

It if given that for water, m = 5691 g

And, we know that specific heat capacity of water is 4.186 $J/g^{o}C$ .

As, Q = $m \times C \times (T_{f} - T_{i})$

228970 J = $5691 g \times 4.184 J/g^{o}C \times (T_{f} - 21)
^{o}C$

$T_{f} - 21^{o}C = 9.616^{o}C$

$T_{f} = 30.6^{o}C$

Thus, we can conclude that the final temperature of the water is $30.6^{o}C$ .

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3 years ago

2. What is the process of diverting un-<br>wanted electric charge directly into<br>the earth?

AnnyKZ [126]

Answer: grounding

Explanation:

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4 years ago