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Maurinko [17]
2 years ago
7

A food worker had safely cooled a large pot of soup to 70 F (21 C) with two hours. What temperature must the soup Reach in the f

our hours to be cooled properly
Chemistry
1 answer:
padilas [110]2 years ago
4 0

The temperature reached after four hours of cooling is 140 F (or) 42 C.

Explanation:

A food worker cooled a cup of soup for two hours,

step 1: The temperature reached in <u>two hours</u>= 70 F (or) 21 C

step 2: Then for <u>four hours</u>, <u>it is twice the value</u>

∴ The temperature reached in four hours= 2(70)= 140 F (or) 2(21)= 42 C

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anzhelika [568]
The final temperature of the copper is 59.0. The specific heat capacity of copper is 0.38 j/g -k
3 0
2 years ago
A column is filled with four different liquids of different densities. A red liquid, a blue liquid, a green liquid, and a purple
Svet_ta [14]

<em>Answer:</em>

The order of liquid from top to bottom is as follow

  •        Purple, green, red, blue

<em>Explanation:</em>

Chart of densities:

  •   Red = 1.2 g/cm∧3
  •   Blue = 1.6 g/cm∧3
  •   green = 0.8 g/cm∧3
  •   Purple = 0.1 g/cm∧3

<em>Density:   </em>

Density is the ratio of mass and volume as follow

                             d = m/v

<em>Summary:</em>

  • Greater the density, it will be at bottom and vice versa.
  • Blue liquid has greater density so it will be at bottom
  • Purple liquid has low density, so it will be at top.
5 0
2 years ago
Read 2 more answers
Type the correct answer in the box. Express your answer to three significant figures.
satela [25.4K]

Answer:

The partial pressure of argon in the jar is 0.944 kilopascal.

Explanation:

Step 1: Data given

Volume of the jar of air = 25.0 L

Number of moles argon = 0.0104 moles

Temperature = 273 K

Step 2: Calculate the pressure of argon with the ideal gas law

p*V = nRT

p = (nRT)/V

⇒ with n = the number of moles of argon = 0.0104 moles

⇒ with R = the gas constant = 0.0821 L*atm/mol*K

⇒ with T = the temperature = 273 K

⇒ with V = the volume of the jar = 25.0 L

p = (0.0104 * 0.0821 * 273)/25.0

p = 0.00932 atm

1 atm =101.3 kPa

0.00932 atm = 101.3 * 0.00932 = 0.944 kPa

The partial pressure of argon in the jar is 0.944 kilopascal.

5 0
2 years ago
A bar of gold is 5.0mm thick, 10.0cm long and 2.0cm wide. It has a mass of exactly 193.0g. What is the desity of gold?
Tanzania [10]
<h3>Answer:</h3>

19.3 g/cm³

<h3>Explanation:</h3>

Density of a substance refers to the mass of the substance per unit volume.

Therefore, Density = Mass ÷ Volume

In this case, we are given;

Mass of the gold bar = 193.0 g

Dimensions of the Gold bar = 5.00 mm by 10.0 cm by 2.0 cm

We are required to get the density of the gold bar

Step 1: Volume of the gold bar

Volume is given by, Length × width × height

Volume =  0.50 cm × 10.0 cm × 2.0 cm

             = 10 cm³

Step 2: Density of the gold bar

Density = Mass ÷ volume

Density of the gold bar = 193.0 g ÷ 10 cm³

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Thus, the density of the gold bar is 19.3 g/cm³

3 0
2 years ago
How many lead (Pb) atoms will be generated when 5.38 moles of ammonia react according to the following equation: 3PbO+2NH3→3Pb+N
jasenka [17]

Answer:

4.86×10^23 molecule of Pb

Explanation:

Based on that equation, for every 2 moles of ammonia, you get 3 moles of lead.

So:

2 mol NH3/ 3 mol Pb

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(5.38 NH3)(3 Pb/ 2 NH3) = (5.38)(3/2) mol Pb = 8.07 mol Pb

Then, we just need to use Avagadro's number to get the number of molecules.

(8.07)(6.02×10^23) = 4.86×10^23 molecule of Pb

4 0
2 years ago
Read 2 more answers
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