The isotope of an atom containing 31 protons and 39 neutrons suddenly has two neutrons added to it. What isotope is create?

In an experiment, Ann mixes concentrated sulfuric acid with water in a reaction test tube. The walls of the test tube turn hot.W

vladimir2022 [97]

B) Exothermic
The reaction released heat energy to its surrounding, thus, it was exothermic.
"exo" is to expel or put outside
"thermic" means heat

8 0

2 years ago

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Aluminum has a density of 2.70g/cm what is the volume occupied by a block of aluminum which weights 4.32kg

romanna [79]

Answer:

Explanation:

0.000625 cm3

0.625 cm3

1.60 cm3

4 0

2 years ago

A sample of a compound containing only carbon and hydrogen atoms is completely combusted, producing

shusha [124]

It’s the last one C2H

5 0

2 years ago

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Please someone help me to solve this problem

Zinaida [17]

Answer:

(a) The final pressure of the sample becomes one-fourth of the original pressure.

(b) The pressure of the sample remains unchanged.

(c) The final pressure of the sample becomes four times of the original pressure.

Explanation:

(a)

$P_{2}=\frac{P_{1}V_{1}T_{2}}{T_{1}V_{2}}$

The volume of sample doubled and kelvin temperature halved.

$V_{2}=2V_{1}$

$T_{2}=\frac{1}{2}T_{1}$

$P_{2}=\frac{P_{1}\times V_{1}\times \frac{1}{2}T_{1}}{T_{1}\times2V_{1}}=\frac{P_{1}}{4}$

Therefore, the final pressure of the sample becomes one-fourth of the original pressure.

(b)

Volume and temperature of sample doubled.

$V_{2}=2V_{1}$

$T_{2}=2T_{1}$

$P_{2}=\frac{P_{1}\times V_{1}\times 2T_{1}}{T_{1}\times2V_{1}}={P_{1}}$

Therefore, the pressure of the sample unchanged.

(c)

Volume of sample halved and temperature double.

$V_{2}=\frac{1}{2}V_{1}$

$T_{2}=2T_{1}$

$P_{2}=\frac{P_{1}\times V_{1}\times 2T_{1}}{T_{1}\times \frac{1}{2}V_{1}}={4P_{1}}$

Therefore, the pressure of the sample becomes four times of the original pressure.

6 0

2 years ago

What is the empirical formula of ascorbic acid (Vitamin C). If Carbon is 40.91%, Hydrogen is 4.5% and Oxygen is 54.50%. Show you

kkurt [141]

Answer:

In 100 g of ascorbic acid, we will have 40.92 g C, 4.58 g H, and 54.50 g O. The whole-number ratio gives us the subscripts for the empirical formula. Thus, the empirical formula is C3H4O3.

Explanation:

When given % composition, and asked for the empirical formula, it is easiest to just assume 100 g of material. Thus,

Mass C = 40.92 g. Moles C = 40.92 g x 1 mole/12 g = 3.41 moles C

Mass H = 4.58 g. Moles H = 4.58 g x 1 mole/1.0 g = 4.58 moles H

Mass O = 54.50 g. Moles O = 54.50 g x 1 mole/16 g = 3.41 moles O

Next, we want to get the moles into whole numbers, so we begin by dividing all by the smallest, i.e. divide all by 3.41.

Moles C = 3.41/3.41 = 1

Moles H = 4.58/3.41 = 1.34

Moles O = 3.41/3.41 = 1

Now, in order to get 1.34 to be a whole number we multiply it (and all others) by 3

Moles C = 1x3 = 3

Moles H = 1.34x3 = 4

Moles O = 1x3 = 3

Empirical Formula = C3H4O3

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Miss Hawaii

8 0

2 years ago