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2 years ago

Assume that 8.5 L of iodine gas are produced at STP according to the following balanced equation:

2 answers:

3 0

Balanced chemical equation is as;

 2 Kl + Cl₂ → 2 KCl + I₂

1) Moles of I₂ produced;

22.4 L volume is occupied by = 1 mole of I₂ at STP
So,
8.5 L of I₂ will be occupied by = X mole of I₂ at STP

Solving for X,
X = (8.5 L × 1 mol) ÷ 22.4 L

X = 0.379 Moles of I₂

2) Moles of Cl₂ used;

22.4 L I₂ utilized = 1 mole of Cl₂ gas
So,
8.5 L of I₂ will utilize = X mole of Cl₂ gas

Solving for X,
X = (8.5 L × 1 mol) ÷ 22.4 L

X = 0.379 Moles of Cl₂

3) Grams of Cl₂ used;

As,
Moles = Mass / M.mass
Or,
Mass = Moles × M.mass

Mass = 0.379 mol × 70.90 g.mol⁻¹

Mass = 26.87 grams of Cl₂

Nat2105 [25]2 years ago

3 0

Answer:

0.38
0.38
27

Explanation:

right on edge

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Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpentina. It was first synthesized in 1956 by No

liraira [26]

Answer:

Molality = 0.066 m

Molar mass = 608.36 g/mol

Explanation:

It seems the question is incomplete. However a web search us shows this data:

" Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpentina. It was first synthesized in 1956 by Nobel Prize winner R. B. Woodward. It is used as a tranquilizer and sedative. When 1.00 g reserpine is dissolved in 25.0 g camphor, the freezing-point depression is 2.63 °C (Kf for camphor is 40 °C·kg/mol). Calculate the molality of the solution and the molar mass of reserpine. "

The freezing-point depression is expressed by:

ΔT=Kf * m

We put the data given by the problem and solve for m:

2.63 °C = 40°C·kg/mol * m

m = 0.06575 m

For the calculation of the molar mass: Molality is defined as moles of solute per kilogram of solvent:

0.06575 m = Moles reserpine / kg camphor

25.0 g camphor ⇒ 25.0/1000 = 0.025 kg camphor

We calculate moles of reserpine:

0.06575 m = Moles reserpine / 0.025 kg camphor

Moles reserpine = 1.64x10⁻³ mol

Finally we use the mass of reserpine and the moles to calculate the molar mass:

1.00 g reserpine / 1.64x10⁻³ mol = 608.36 g/mol

Keep in mind that if the data in your problem is different, the results will be different. But the solving method remains the same.

8 0

2 years ago

Question 17 In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas t

mars1129 [50]

Answer:

Explanation:

N₂ + 3H₂ = 2 NH₃

1 vol 2 vol

786 liters 1572 liters

786 liters of dinitrogen will result in the production of 1572 liters of ammonia

volume of ammonia V₁ = 1572 liters

temperature T₁ = 222 + 273 = 495 K

pressure = .35 atm

We shall find this volume at NTP

volume V₂ = ?

pressure = 1 atm

temperature T₂ = 273

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

$\frac{.35\times 1572}{495} =\frac{1\times V_2}{ 273 }$

$V_2 =303.44$ liter .

mol weight of ammonia = 17

At NTP mass of 22.4 liter of ammonia will have mass of 17 gm

mass of 303.44 liter of ammonia will be equal to (303.44 x 17) / 22.4 gm

= 230.28 gm

=.23 kg / sec .

Rate of production of ammonia = .23 kg /s .

5 0

2 years ago

Ron and Hermione begin with 1.50 g of the hydrate copper(II)sulfate ∙ x-hydrate (CuSO4 ∙ xH2O), where x is an integer. Part of t

Gwar [14]

Answer

Explanation:

We can go about this using the percentage compositions.

First, we calculate the percentage composition of the copper sulphate. This is obtainable by using the mass.

0.96/1.5 * 100 = 64%

Hence the percentage by mass of the water present is 36%

The molar mass of the anhydrous sulphate is 64 + 32 +4(16) = 160g/mol

The molar mass of the water is 2(1) + 16 = 18g/mol

Not forgetting that it is in multiples of x, the total molar mass of the water is 18x moles

The total mass of the copper sulphate hydrate is 160+ 18x

Now how do we get x? Like it is said earlier, the percentage composition is constant.

Hence, 64/100 * (160 + 18x) = 160

16000 = 64(160 + 18x)

16000 = 10,240 + 1152x

16,000 - 10,240 = 1152x

1152x = 5760

x = 5760/1152

x = 5

7 0

2 years ago

A sample of pure iron has a mass of 5.00 g. Calculate its volume.

olga55 [171]

It's volume is 0.48 cm3Specific

3 0

2 years ago

When 1.365 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the

luda_lava [24]

<h3>The enthalpy of combustion per mole of anthracene : 7064 kj/mol(- sign=exothermic)</h3><h3>Further explanation </h3>

The law of conservation of energy can be applied to heat changes, i.e. the heat received/absorbed is the same as the heat released

Q in = Q out

Heat can be calculated using the formula:

Q = mc∆T

Heat released by anthracene= Heat absorbed by water

Heat absorbed by water =

$\tt Q=500\times 4.18\times 25.89=54110.1~J$

mol of anthracene (MW=178,23 g/mol)

$\tt \dfrac{1.365}{178.23}=0.00766$

The enthalpy of combustion per mole of anthracene :

$\tt \Delta H=-\dfrac{Q}{n}=\dfrac{54110.1}{0.00766}=-7063981.7~J/mol\approx -7064~kJ/mol$

8 0

2 years ago