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2 years ago

If you are needing at least 100. grams of HCI to be produced, how many

Chemistry

1 answer:

Charra [1.4K]2 years ago

8 0

Answer:

116.4 g of SiCl4

Explanation:

SiCl4(l) +2H2O(l) -------> SiO2 (s) + 4HCl(aq)

Given this balanced reaction equation which will serve as a guide for our work, we can now look at the stoichiometry of the reaction.

Number of moles of HCl needed = mass of HCl/ molar mass of HCl

Molar mass of HCl= 36.46 g/mol

Number of moles of HCl= 100/36.46 g/mol= 2.74 moles

From the balanced reaction equation;

1 mole of SiCl4 yields 4 moles of HCl

x moles of SiCl4 will yield 2.74 moles of HCl

x= 2.74/4 = 0.685 moles of SiCl4

Therefore mass of SiCl4= number of moles of SiCl4 × molar mass of SiCl4

Mass of SiCl4= 0.685× 169.9 g/mol = 116.4 g of SiCl4

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Which of the following represents a chemical change? A.Souring of milk B.Melting of chocolate C.Condensation of water D.Breaking

leonid [27]

Chemical changes occur when a substance combines with another to form a new substance, called chemical synthesis or, alternatively, chemical decomposition into two or more different substances.

So which one do you think is the answer?

8 0

3 years ago

Read 2 more answers

How many moles are in 2.00g of H2O

gavmur [86]

n = m/M = 2/18 = 1/9 ~0,1 mol

4 0

2 years ago

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I need help can someone please do so?

larisa86 [58]

Answer:

0.296 J/g°C

Explanation:

Step 1:

Data obtained from the question.

Mass (M) =35g

Heat Absorbed (Q) = 1606 J

Initial temperature (T1) = 10°C

Final temperature (T2) = 165°C

Change in temperature (ΔT) = T2 – T1 = 165°C – 10°C = 155°C

Specific heat capacity (C) =..?

Step 2:

Determination of the specific heat capacity of iron.

Q = MCΔT

C = Q/MΔT

C = 1606 / (35 x 155)

C = 0.296 J/g°C

Therefore, the specific heat capacity of iron is 0.296 J/g°C

8 0

3 years ago

Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and the energy of a single photon of this r

denis23 [38]

Answer :

(1) The frequency of photon is, $3\times 10^{10}Hz$

(2) The energy of a single photon of this radiation is $1.988\times 10^{-23}J/photon$

(3) The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol

Explanation : Given,

Wavelength of photon = $1.0cm=0.01m$ (1 m = 100 cm)

(1) Now we have to calculate the frequency of photon.

Formula used :

$\nu=\frac{c}{\lambda}$

where,

$\nu$ = frequency of photon

$\lambda$ = wavelength of photon

c = speed of light = $3\times 10^8m/s$

Now put all the given values in the above formula, we get:

$\nu=\frac{3\times 10^8m/s}{0.01m}$

$\nu=3\times 10^{10}s^{-1}=3\times 10^{10}Hz$ $(1Hz=1s^{-1})$

The frequency of photon is, $3\times 10^{10}Hz$

(2) Now we have to calculate the energy of photon.

Formula used :

$E=h\times \nu$

where,

$\nu$ = frequency of photon

h = Planck's constant = $6.626\times 10^{-34}Js$

Now put all the given values in the above formula, we get:

$E=(6.626\times 10^{-34}Js)\times (3\times 10^{10}s^{-1})$

$E=1.988\times 10^{-23}J/photon$

The energy of a single photon of this radiation is $1.988\times 10^{-23}J/photon$

(3) Now we have to calculate the energy in J/mol.

$E=1.988\times 10^{-23}J/photon$

$E=(1.988\times 10^{-23}J/photon)\times (6.022\times 10^{23}photon/mol)$

$E=11.97J/mol$

The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol

3 0

3 years ago

Read 2 more answers

Given 16.2 grams of substance Y, if the substance absorbs 2722 joules of energy and the specific heat of the substance is 9.22 J

snow_tiger [21]

Since the substance absorbs heat, it is expected that the temperature will rise. The formula for the internal energy of a substance is given by the equation:

ΔU = mCpΔT

where:

ΔU = internal energy
m = mass of substance
Cp = specific heat capacity of substance
ΔT = change in temperature

ΔU = 2722 Joules = 16.2 grams (9.22 J/g-°C) (Tf - 26°C)

This gives a final temperature of Tf = 44.22 °C

4 0

2 years ago