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3 years ago

What is happening to the temperature/pressure during the Deposition Change of State?

1 answer:

jeka943 years ago

4 0

A material will change from one state or phase to another at specific combinations of temperature and surrounding pressure. Typically, the pressure is atmospheric pressure, so temperature is the determining factor to the change in state in those cases.

Names such as boiling and freezing are given to the various changes in states of matter. The temperature of a material will increase until it reaches the point where the change takes place. It will stay at that temperature until that change is completed.

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How many grams of sulfur in 4.20 x 1021 atoms of sulfur?

Stolb23 [73]

Answer:

look it up

Explanation:

6 0

2 years ago

What volume of o2 is needed to react fully with 720. Ml of nh3

Galina-37 [17]

Ammonia undergoes combustion with oxygen to produce nitric oxide and water. The volume of the oxygen required to react with 720 ml of ammonia is 900 ml.

<h3>What is volume?</h3>

Volume is the area occupied by the substance and is the ratio of the mass to the density.

At STP, 1 mole of gas occupies 22.4 L of volume

Given,

Volume of ammonia reacted = 0.720 L

The combustion reaction is shown as,

$\rm 4NH_{3} + 5O_{2} \rightarrow 4NO +6H_{2}O$

From the stoichiometry of the reaction, it can be said that,

$(4 \times 22.4)$ L of ammonia reacts with $(5 \times 22.4)$ L of oxygen gas.

So, 0.720 L of ammonia will react with:

$\dfrac{ (5 \times 22.4)}{(4 \times 22.4)} \times 0.720 = 0.9 \;\rm L$

Therefore, the volume of oxygen required is 900 mL.

Learn more about volume here:

brainly.com/question/14090111

#SPJ4

6 0

2 years ago

Sewage is a liquid waste which causes<br> _________ and ________ pollution.

nadezda [96]

Answer:

Lake and River pollution?

Explanation:

5 0

2 years ago

Read 2 more answers

Burning 12.00 g of an oxoacid produces 17.95 g of carbon dioxide and 4.87 g of water. Consider that 0.25

Veseljchak [2.6K]

Answer: The molecular formula will be $C_6H_6O_6$

Explanation:

Mass of $CO_2$ = 17.95 g

Mass of $H_2O$ = 4.87 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 17.95 g of carbon dioxide, = $\frac{12}{44}\times 17.95=4.89g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 4.87 g of water, = $\frac{2}{18}\times 4.87=0.541g$ of hydrogen will be contained.

Mass of oxygen in the compound = (12.00) - (4.89+0.541) = 6.57 g

Mass of C = 4.89 g

Mass of H = 0.541 g

Mass of O = 6.57 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{4.89g}{12g/mole}=0.407moles$

Moles of H= $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.541g}{1g/mole}=0.541moles$

Moles of O= $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{6.57g}{16g/mole}=0.410moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{0.407}{0.407}=1$

For H = $\frac{0.541}{0.407}=1$

For O = $\frac{0.410}{0.407}=1$

The ratio of C : H : O = 1: 1 : 1

Hence the empirical formula is $CHO$ .

Hence the empirical formula is $CHO$

The empirical weight of $CHO$ = 1(12)+1(1)+1(16)= 29 g.

If 0.25 moles has mass of 44.0 g

Thus 1 mole has mass of = $\frac{44.0}{0.25}\times 1=176g$

Thus molecular mass is 176 g

Now we have to calculate the molecular formula.

$n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{176g}{29g}=6$

The molecular formula will be= $6\times CHO=C_6H_6O_6$

5 0

3 years ago

Which of the following statements about subatomic particles best characterizes protons?

REY [17]

Lets get this straight:-

Protons → Positive charge, found in nucleus, heavy

Now, the only one we see that seems to be correct is A) positive charge, heavy, found in the nucleus of an atom

3 0

3 years ago