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Alex787 [66]
2 years ago
7

The temperature on a distant, undiscovered planet is expressed in degrees B. For example, water boils at 180 ∘ B and freezes at

50 ∘ B . If it is 31 ∘ C on Earth, what would that temperature be in terms of degrees B?
Chemistry
1 answer:
marin [14]2 years ago
5 0

Answer:

40.3∘C

Explanation:

At planet B;

Water boils = 180∘C

Water freezes = 50∘C

In this planet the temperature difference = 180 - 50 = 130 compared to earth where the temperature difference is; 100 - 0 = 100

This means;

130 ∘C = 100 ∘C

x ∘C = 31 ∘C

x = 31 * 130 / 100

x = 40.3∘C

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Unit Conversion Help Thank you
AlekseyPX

Answer : 1721.72 g/qt are in 18.2 g/cL

Explanation :

As we are given: 18.2 g/cL

Now we have to convert 18.2 g/cL to g/qt.

Conversions used are:

(1) 1 L = 100 cL

(2) 1 L = 1000 mL

(3) 1 qt = 946 qt

The conversion expression will be:

\frac{18.2g}{1cL}\times \frac{100cL}{1L}\times \frac{1L}{1000mL}\times \frac{946mL}{1qt}

=1721.72\text{ g/qt}

Therefore, 1721.72 g/qt are in 18.2 g/cL

5 0
2 years ago
Anna lives in a city that experiences high precipitation, with an average annual rainfall of 524 millimeters. It is warm all yea
gavmur [86]

Anna lives in a city that is part of the tropical climate types. It has a constantly warm weather, and thus higher humidity, and according to the annual rainfall, it is most probably a rainfall that appears seasonally, not throughout the whole year.

Tim, on the other hand, lives in a city that is part of the dry climate types. It is most probably a place that is deep into the mainland, like the cold deserts of Central Asia, where the temperatures in the summer are high, and in winter are very low. Because of the distance from the sea, the rainfall doesn't reach this places, so they are very dry, and only have symbolic amount of annual rainfall.

6 0
2 years ago
At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20∘C to 25∘C
Tatiana [17]

Answer: 0.0007 moles of CO_2 is released when temperature is raised.

Explanation:

To calculate the number of moles, we use the ideal gas equation, which is:

PV=nRT

where,

P = pressure of the gas = 1.01 bar

V = Volume of the gas = 1L

R = Gas constant = 0.08314\text{ L bar }mol^{-1}K^{-1}

  • Number of moles when T = 20° C

Temperature of the gas = 20° C = (273 + 20)K = 293K

Putting values in above equation, we get:

1.01bar\times 1L=n_1\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 293K\\n_1=0.04146moles

  • Number of moles when T = 25° C

Temperature of the gas = 25° C = (273 + 25)K = 298K

Putting values in above equation, we get:

1.01bar\times 1L=n_2\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 298K\\n_2=0.04076moles

  • Number of moles released = n_1-n_2=0.04146-0.04076=0.0007moles

Hence,  0.0007 moles of CO_2 is released when temperature is raised from 20° C to 25° C

5 0
2 years ago
For each case below, identify the most likely value for x: a. BHx b. CHx c. NHx d. CH2Clx
Snezhnost [94]

Answer:

BHx, x=3

CHx, x=4

NHx, x=3

CH2Clx, x=2

Explanation:

We have to know that the value of x must depend on the valency of the central atom. If we look at each of the species;

Boron has a common valency of 3

Carbon has a common valency of 4

Nitrogen has a common valency of 3

The valency of each elements will determine the most likely value of x as outlined in the answer above.

8 0
2 years ago
An unknown compound with a molar mass of 155.06 g/mol consists of 46.47% c, 7.80% h, and 45.72% cl. find the molecular formula f
Contact [7]

Answer:- Molecular formula of the compound is C_6H_1_2Cl_2 .

Solution:- From given information:

C = 46.47%

H = 7.80%

Cl = 45.72%

First of all we find out the empirical formula from given percentages. We divide the given percentages by their respective atomic masses to calculate the moles:

C=\frac{46.47}{12.01}  = 3.87

H=\frac{7.80}{1.01}  = 7.72

Cl=\frac{45.72}{35.45}  = 1.29

Now, we divide the moles of each by the least one of them. Least one is Cl as it's moles are least as compared to the moles of C and H. So, let's divide the moles of each by 1.29.

C=\frac{3.87}{1.29} = 3

H=\frac{7.72}{1.29} = 6

Cl=\frac{1.29}{1.29} = 1

So, the empirical formula of the compound is C_3H_6Cl .

Empirical formula mass = 3(12.01) + 6(1.01) + 1(35.45)

= 36.03 + 6.06 + 35.45

= 77.54

To calculate the number of formula units we divide molar mass by empirical formula mass.

number of empirical formula units = \frac{155.06}{77.54}

= 2

So, the molecular formula would be two times of empirical formula that is, C_6H_1_2Cl_2 .

4 0
2 years ago
Read 2 more answers
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