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Slav-nsk [51]
3 years ago
6

Day/Night and Seasons (8.7A)

Chemistry
1 answer:
Natasha_Volkova [10]3 years ago
5 0
The length of the seasons would increase
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56. The electron configuration for phosphorous is [Ar]3s23p4.<br> a. TRUE<br> b. FALSE
melomori [17]

Answer:

False

Explanation:

7 0
2 years ago
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Our wine is consisted of 12% v/v alcohol. How much a man of alcohol are consistent in 4 L of Wine
Zina [86]

Answer:

0.48

Explanation:

all you need is to decide 12% with 100% then you multiply it by 4L.

4 0
3 years ago
How many grams of carbon dioxide are produced when 16 g of methane and 48 g of oxygen gas combust
larisa [96]
I believe the correct answer is 11 g
6 0
2 years ago
what is the percent yield of titanium (II) oxide if 20.0 grams of titanium (II) sulfide is reacted with water? The actual yield
earnstyle [38]

Answer : The percent yield of titanium (II) oxide is, 142.5 % and the impurities could have caused the percent yield to be so high.

Explanation : Given,

Mass of titanium(II) sulfide = 20.0 g

Molar mass of titanium(II) sulfide = 79.9 g/mole

Molar mass of titanium(II) oxide = 63.9 g/mole

First we have to calculate the moles of titanium(II) sulfide.

\text{ Moles of titanium(II) sulfide}=\frac{\text{ Mass of titanium(II) sulfide}}{\text{ Molar mass of titanium(II) sulfide}}=\frac{20.0g}{79.9g/mole}=0.2503moles

Now we have to calculate the moles of titanium(II) oxide.

The balanced chemical reaction is,

TiS+H_2O\rightarrow TiO+H_2S

From the reaction, we conclude that

As, 1 mole of titanium(II) sulfide react to give 1 mole of titanium(II) oxide

So, 0.2503 mole of titanium(II) sulfide react to give 0.2503 mole of titanium(II) oxide

Now we have to calculate the mass of titanium(II) oxide.

\text{ Mass of titanium(II) oxide}=\text{ Moles of titanium(II) oxide}\times \text{ Molar mass of titanium(II) oxide}

\text{ Mass of titanium(II) oxide}=(0.2503moles)\times (63.9g/mole)=15.99g

To calculate the percentage yield of titanium (II) oxide, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of titanium (II) oxide = 22.8 g

Theoretical yield of titanium (II) oxide = 15.99 g

Putting values in above equation, we get:

\%\text{ yield of titanium (II) oxide}=\frac{22.8g}{15.99g}\times 100\\\\\% \text{yield of titanium (II) oxide}=142.5\%

Hence, the percent yield of titanium (II) oxide is, 142.5 %

If the percent yields is greater than 100% that means the product of the reaction contains impurities which cause its mass to be greater than it actually.

5 0
3 years ago
A 60.0 kg object is moving east at 8.00 m/s, and then slows down to 4.00 m/s. How much work was done?
Colt1911 [192]

Answer:

A

-1440J

Explanation:

Hello,

This question requires us to calculate the work done on a object to move it from point A to point B

Data

Mass = 60kg

Initial velocity (V1) = 8.0m/s

Final velocity (V2) = 4.0m/s

Workdone on an object is equal to force applied on the object to move it through a particular distance.

Work done = force × distance

Force (F) = mass × acceleration

Distance = s

F = Ma

Work done = M× a × s

But a = velocity (v) / time (t)

Work done = mvs / t

But velocity = distance/ time

Work done = mv × v/

Work done = mv²

Work done = ½mv²

Workdone = ½M(V2² - V1²)

Workdone = ½ × 60 (4² - 8²)

Work done = 30 × (16 - 64)

Workdone = 30 × (-48)

Work done = -1440J

Work done = -1.44kJ

The workdone on the object is equal to -1.44kJ

5 0
3 years ago
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