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myrzilka [38]
3 years ago
10

How many molecules of carbon monoxide are in 10 mL at STP

Chemistry
1 answer:
mote1985 [20]3 years ago
7 0

 The number  of  carbon monoxide that  are in 10 ml at STP  is 2.68 x 10²⁰  molecules

<u><em>  calculation</em></u>

<u><em> </em></u>Step 1 :  convert 10 ml to L

convert 10 ml to L = 10/1000 =0.01 L

Step 2: find the moles of CO at STP

That is at STP  1  mole  = 22.4 L

                           ?moles = 0.01 L

by cross  multiplication

= {0.01 L x 1 mole)/22.4 L} =4.46 x 10⁻⁴  moles


Step 3 ; find the  number of   molecules of Co  using the Avogadro's law constant

that  according to Avogadro's  law  1  moles = 6.02 x 10²³

                                                  4.46 x 10⁻⁴ moles =? molecules

<em>by cross multiplication</em>

= {(4.46 x 10⁻⁴  moles) x( 6.02 x 10²³  molecules) / 1 mole}  =2.68 x 10²⁰  molecules


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Answer:

Latitude and longitude are imaginary lines that help us label every place on the surface of the earth. The most important line of latitude is the equator, which runs horizontally around the fattest part of the earth.

Explanation:

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3 years ago
How many molecules are in 68.0 g of H2S
Kryger [21]

The correct answer is 12.044 × 10²³ molecules.  

The molecular mass of H₂S is 34 gram per mole.  

Number of moles is determined by using the formula,  

Number of moles = mass/molecular mass

Given mass is 68 grams, so no of moles will be,  

68/34 = 2 moles

1 mole comprises 6.022 × 10²³ molecules, therefore, 2 moles will comprise = 6.022 × 10²³ × 2

= 12.044 × 10²³ molecules.  


3 0
3 years ago
A 2.00-mol sample of hydrogen gas is heated at constant pressure from 294 K to 414 K. (a) Calculate the energy transferred to th
Furkat [3]

Answer:

a) The energy transferred is 6.91 kJ

b) The internal energy is 4.90 kJ

c) The work done on the gas is - 2.01 kJ

Explanation:

Step 1: Data given

Number of moles of hydrogen gas = 2.00 moles

Pressure = constant

Temperature is heated from 294 K to 414 K

Molar heat capacity of hydrogen gas = 28.8 J/mol*K

Step 2: Calculate the energy transferred to the gas by heat.

Q = n* Cp * ΔT

⇒with Q =the energy transferred

⇒with n = the number of moles = 2.00 moles

⇒with Cp = the Molar heat capacity of hydrogen gas = 28.8 J/mol*K

⇒ with ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

Q = 2.00 * 28.8 * 120

Q = 6912 J = 6.91 kJ

Step 3: Calculate the increase in its internal energy.

ΔEint = n*Cv*ΔT

⇒with ΔEint = the increase in its internal energy.

⇒with n = the number of moles = 2.00 moles

⇒with Cv = The constant volume = 20.4 J/mol*K

⇒with  ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

ΔEint = 2.00 * 20.4 * 120

ΔEint =4896 J = 4.90 kJ

Step 4: Calculate the work done on the gas.

Work done on the gas = -Q + ΔEint

W = -6.91 kJ + 4.90 kJ

W = -2.01 kJ

6 0
3 years ago
Complete this equation for the dissociation of na2co3(aq). omit water from the equation because it is understood to be present.
Savatey [412]
Net overall dissociation:
Na2CO3 ---> 2Na(-) + CO3(2-)

*The ion charge is in parenthesis
6 0
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If I mix bleach and namona and throw it on a person what will happen​
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They have the chance to inhale toxic fumes secreted by the mixture.

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