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Rzqust [24]
3 years ago
11

How much heat is released as the temperature of 25.2 grams of iron is decreased from 72.1°C to 9.8°C? The specific heat of iron

is 0.444 J/g·°C.
Chemistry
1 answer:
prisoha [69]3 years ago
8 0

Answer:

Q=-697.06\ J

Negative sign says that release of heat.

Explanation:

The expression for the calculation of the heat released or absorbed of a process is shown below as:-

Q=m\times C\times \Delta T

Where,  

\Delta H  is the heat released or absorbed

m is the mass

C is the specific heat capacity

\Delta T  is the temperature change

Thus, given that:-

Mass = 25.2 g

Specific heat = 0.444 J/g°C

\Delta T=9.8-72.1\ ^0C=-62.3\ ^0C

So,  

Q=25.2\times 0.444\times -62.3\ J=-697.06\ J

Negative sign says that release of heat.

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<h3>Answer:</h3>

                  0.64 Moles of Propane

<h3>Explanation:</h3>

Data:

         Moles of Carbon  =  1.5 mol

         Conversion factor  =  7 mol C produces = 3 mol of Propane

Solution:

             As we know,

                7 moles of Carbon produces =  3 moles of Propane

Then,

            1.5 moles of Carbon will produce  =  X moles of Propane

Solving for X,

                     X =  (1.5 moles × 3 moles) ÷ 7 moles

                     X  =  0.6428571 moles of Propane

Or rounded to two significant figures,

                     X =  0.64 Moles of Propane

5 0
2 years ago
25 POINTS TO WHOEVER CAN FILL THIS OUT! Radioactivity Decay
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Answer:

how long?

Explanation:

3 0
3 years ago
What is the formula weight (amu) of the molecule H2O? Use atomic masses of H and O as 1.008 amu and 16.00 amu respectively. Repo
vaieri [72.5K]

Answer:

Formula weight of H₂O molecule is  18.02 amu.

Explanation:

Given data:

Formula weight of H₂O = ?

Atomic mass of H = 1.008 amu

Atomic mass of O = 16.00 amu

Solution:

Formula weight:

"It is the sum of all the atomic weight of atoms present in given formula"

Formula weight of H₂O = 2×1.008 amu + 1×16.00 amu

Formula weight of H₂O = 18.02 amu

Thus, formula weight of H₂O molecule is  18.02 amu.

6 0
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Solubility of a salt that has a general formula M3X (where M is the cation and X is the anion) is 0.0283 g/L of the solution. Th
egoroff_w [7]

ksp = 7.003 \times  {10}^{ - 16}  {mol}^{4}  {dm}^{ - 12}

6 0
3 years ago
A quantity of 0.225 g of a metal M (molar mass = 27.0 g/mol) liberated 0.303 L of molecular hydrogen (measured at 17°C and 741 m
Lana71 [14]

Answer:

Oxide of M is M_2O_3 and sulfate of M_2(SO_4)_3

Explanation:

0.303 L of molecular hydrogen gas measured at 17°C and 741 mmHg.

Let moles of hydrogen gas be n.

Temperature of the gas ,T= 17°C =290 K

Pressure of the gas ,P= 741 mmHg= 0.9633 atm

Volume occupied by gas , V = 0.303 L

Using an ideal gas equation:

PV=nRT

n=\frac{PV}{RT}=\frac{0.9633 atm\times 0.303 L}{0.0821 atm L/mol K\times 290 K}=0.01225 mol

Moles of hydrogen gas produced = 0.01225 mol

2M+2xHCl\rightarrow 2MCl_x+xH_2

Moles of metal =\frac{0.225 g}{27.0 g/mol}=8.3333 mol

So, 8.3333 mol of metal M gives 0.01225 mol of hydrogen gas.

\frac{8.3333}{0.01225 mol}=\frac{2}{x}

x = 2.9 ≈ 3

2M+6HCl\rightarrow 2MCl_3+3H_2

MCl_3\rightarrow M^{3+}+Cl^-

Formulas for the oxide and sulfate of M will be:

Oxide of M is M_2O_3 and sulfate of M_2(SO_4)_3.

3 0
3 years ago
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