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leonid [27]
3 years ago
8

Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below.

Chemistry
2 answers:
Andreas93 [3]3 years ago
8 0

Answer:

15.63 moles of HgO are needed to produce 250.0 g of O_{2}

Explanation:

According to given balanced equation, 1 mole of O_{2} is produced from 2 moles of HgO.

Number of moles =\frac{mass}{molar mass}

So 250 g of O_{2} =\frac{250}{32}moles O_{2}

So moles of HgO needed =2\times \frac{250}{32}moles HgO

                                                   =15.63 moles HgO

____ [38]3 years ago
5 0
The answer to the question is C. 15.63
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You wish to construct a buffer of pH=7.0. Which of the following weak acids (w/ corresponding conjugate base) would you select?
Alex17521 [72]

Answer:

C.) HOCl Ka=3.5x10^-8

Explanation:

In order to a construct a buffer of pH= 7.0 we need to find the pKa values of all the acids given below

we Know that

pKa= -log(Ka)

therefore

A) pKa of  HClO2 = -log(1.2 x 10^-2)

=1.9208

B) similarly PKa of HF= -log(7.2 x 1 0^-4)= 2.7644

C)  pKa of HOCl= -log(3.5 x 1 0^-8)= 7.45

D) pKa of HCN = -log(4 x 1 0^-10)=  9.3979

If we consider the  Henderson- Hasselbalch equation for the calculation of the pH of the buffer solution

The weak acid for making the buffer must have a pKa value near to the desired pH of the weak acid.

So, near to value, pH=7.0. , the only option is HOCl whose pKa value is 7.45.

Hence, HOCl will be chosen for buffer construction.

3 0
3 years ago
Which reaction type is the following: AgF + CaCl2 --> AgCl + CaF2
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Explanation:

{\small{\underline{\bf{\red{answer...}}}}} \\  \\

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6 0
3 years ago
A particular exosolar system has five planets in total: A, B, C, D, and E. The table lists the orbital periods of these planets
sveta [45]

Answer:

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Explanation:

8 0
3 years ago
What mass of nitrous oxide gas (N2O) is contained in 20.0 L balloon at a pressure of 110.0 kPa and a temperature of 25 C?
likoan [24]

Answer:

40.94 g

Explanation:

Given data:

Mass of NO₂ = ?

Volume = 20.0 L

Pressure = 110.0 Pka

Temperature = 25°C

Solution:

Pressure = 110.0 KPa (110/101 = 1.1 atm)

Temperature = 25°C (25+273 = 298.15 K)

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

n = PV/RT

n = 1.1 atm × 20.0 L / 0.0821 atm.L/ mol.K ×298.15 K

n = 22 / 24.5 /mol

n= 0.89 mol

Mass of NO₂:

Mass = number of moles × molar mass

Mass = 0.89 mol × 46 g/mol

Mass = 40.94 g

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3 years ago
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