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nordsb [41]
3 years ago
6

Answer ian rlly kno ...........

Chemistry
2 answers:
stich3 [128]3 years ago
6 0
The slope would be -1/2
0-2
2+2 (cause one was negative add instead of subtract)
You would get -2/4 simply that to
-1/2
VMariaS [17]3 years ago
5 0
A ..............................
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Koi Hain Jo bat kr le mujh se :/​
Studentka2010 [4]

Mai hu

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7 0
3 years ago
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How much heat is absorbed when a 298.3 g piece of brass goes from 30.0 to 150
igor_vitrenko [27]

Answer:

Q = 1360.248 j

Explanation:

Given data:

Mass of brass = 298.3 g

Initial temperature = 30.0°C

Final temperature = 150°C

Specific heat capacity of brass = 0.038 J/g.°C

Heat absorbed = ?

SOLUTION:

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = 150°C - 30.0°C  

ΔT = 120°C

Q = 298.3 g × 0.038 J/g.°C × 120°C

Q = 1360.248 j

3 0
3 years ago
Calculate the mole mass of following compound<br> FeSO4
Arada [10]

Explanation:

the molar mass of the compound is 1502g/mol

3 0
3 years ago
A balloon filled with helium occupies 20.0 l at 1.50 atm and 25.0◦c. How many moles of helium will there be in the balloon at st
satela [25.4K]

Answer:

  • There will be 1.23 moles of helium in the balloon at STP

Explanation:

1) <u>Initial conditions of the helium gas</u>:

  • V = 20.0 liter
  • p = 1.50 atm
  • T = 25.0 °C = 25.0 + 273.15 K = 298.15 K

2) <u>Ideal gas equation</u>:

  • pV = n RT
  • p, V, and T are given above
  • R is the Universal constant = 0.0821 atm-liter / ( K - mol)
  • n is the unknown number of moles

3) <u>Solve for n</u>:

  • n = pV / (RT) =
  • n = 1.50 atm × 20.0 liter / (0.0821 atm-liter /k -mol ×298.15K)
  • n = 1.23 mol

4) <u>At STP:</u>

  • STP stands for standard pressure and temperature.
  • The amount (number of moles) of the gas will not change because the change of pressure and temperature, so the number of moles reamain the same: 1.23 mol.
8 0
3 years ago
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Natasha_Volkova [10]

to be honestl id ldm

4 0
3 years ago
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