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alina1380 [7]
3 years ago
5

A calorimeter contains 124 g of water at 26.6°C. A block of metal with a mass of 26 g is heated to 95.8°C and then placed in the

water in the calorimeter. After sufficient time, the temperature of the water is measured and found to be 29.0°C. Calculate the heat capacity per gram of metal. Assume no heat is lost to the calorimeter or the surroundings.
Chemistry
1 answer:
Vinvika [58]3 years ago
8 0

Answer:

The heat capacity of the metal is 0.717 J/g°C

Explanation:

<u>Step 1: </u>Data given

Mass of water = 124.0 grams

Mass of metal = 26.0 grams

Temperature of water = 26.6 °C

Temperature of metal = 95.8 °C

Final temperature of the water = 29.0 °C

<u>Step 2</u>: Calculate heat capacity of metal

Qlost = -Q gained

Qmetal = -Qwater

Q = m*c*ΔT

⇒ with m = mass in grams

⇒ c= the heat capacity in J/g°C

⇒ ΔT = The change in temperature = T2 - T1 (in °C)

Qmetal = -Qwater

m(metal)*c(metal)*ΔT(metal) = -m(water)*c(water)*ΔT(water)

26 *c(metal) *(29-95.8) = -124 * 4.184 *(29-26.6)

-1736.8 * c(metal) = -1245.16

c(metal) = 0.717 J/g°C

The heat capacity of the metal is 0.717 J/g°C

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Which statement best describes the compressibility of a gas?
maria [59]

The answer to the question stated above is:
<span> Gas is easily compressible because the molecules of a gas are much further apart than those of a solid.</span>


characteristic properties of gases:

(1) they are easy to compress,

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7 0
3 years ago
The decomposition of HBr(g) into elemental species is found to have a rate constant of 4.2 ×10−3atm s−1. If 2.00 atm of HBr are
Dennis_Churaev [7]

Answer:

7,94 minutes

Explanation:

If the descomposition of HBr(gr) into elemental species have a rate constant, then this reaction belongs to a zero-order reaction kinetics, where the r<em>eaction rate does not depend on the concentration of the reactants. </em>

For the zero-order reactions, concentration-time equation can be written as follows:

                                          [A] = - Kt + [Ao]

where:

  • [A]: concentration of the reactant A at the <em>t </em>time,
  • [A]o: initial concentration of the reactant A,
  • K: rate constant,
  • t: elapsed time of the reaction

<u>To solve the problem, we just replace our data in the concentration-time equation, and we clear the value of t.</u>

Data:

K = 4.2 ×10−3atm/s,  

[A]o=[HBr]o= 2 atm,  

[A]=[HBr]=0 atm (all HBr(g) is gone)

<em>We clear the incognita :</em>

[A] = - Kt + [Ao]............. Kt =  [Ao] - [A]

                                        t  = ([Ao] - [A])/K

<em>We replace the numerical values:</em>

t = (2 atm - 0 atm)/4.2 ×10−3atm/s = 476,19 s = 7,94 minutes

So, we need 7,94 minutes to achieve complete conversion into elements ([HBr]=0).

6 0
3 years ago
The mass of sample A is 100.0 g, then removed it from a graduated
yan [13]

Answer: 25g/ml

Explanation:

Density = 100.0g/ 4.0mL = 25g/mL

3 0
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What is the molarity of 70.6 g C2H6O in 2.25 L of solution
myrzilka [38]

Hey there!

Molar mass C2H6O = 46.0684 g/mol

Number of moles:

n = mass of solute / molar mass

n = 70.6 / 46.0684

n = 1.532 moles

Therefore:

M = number of moles / volume ( L )

M = 1.532 / 2.25

= 0.680 M

Hope that helps!

7 0
3 years ago
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