I need a answer ASAP

Methane is gas that is found in small quantities in Earth's atmosphere. Methane is the simplest hydrocarbon, consisting of one c

tangare [24]

Answer:

A) Nonmetal carbon shares valence electrons with each nonmetal hydrogen forming four covalent bonds.

Explanation:

Methane is formed when nonmetal carbon shares valence electrons with each nonmetal hydrogen forming four covalent bonds. Nonmetals share electrons to form covalent bonds.

Good luck! :)

8 0

3 years ago

C₂H₄ + 3O₂ → 2CO₂ + 2H₂O If you start with 45.9 g of C₂H₄, and excess O₂, what mass of CO₂ will be produced?

hoa [83]

The mass of CO2 that would be produced is 144.03 g

From the equation of the reaction, the mole ratio of C2H4 input to CO2 produced is 1:2.

Recall that: mole = mass/molar mass

mole of 45.9 g C2H4 = 45.9/28.05

= 1.6364 moles

Thus: equivalent moles of CO2 = 1.6364 x 2

= 3.2727 moles

Mass of 3.2727 moles of CO2 = moles x molar mass

= 3.2727 x 44.01

= 144.03 g

More on stoichiometric calculations can be found here: brainly.com/question/8062886?referrer=searchResults

6 0

3 years ago

Which one A, B, C,D,E,F

Ivahew [28]

The component that runs the circuit is C the wire

8 0

3 years ago

How can you separate mixture of suphur, nacl and nh4cl

weqwewe [10]

Answer:

Ammonium chloride, iron ,Sulphur and salt mixed together... they can be separated in the following methods.

1. Ammonium chloride is separated by sublimination... NC4CI is sublimable. Heat the mixture in a china dish and collect the funds of NC4CI (sublimable substance)

2. Bring a magnet close to the remaining mixture. Iron is magnetic substance and thus, it will be attracted towards the magnet. Iron is separated.

3. Sulphur is insoluble in water and salt is soluble. Add water to the remaining mixture and then wait for sedimentation. Separate the sulphur by decantation.

4. Heat the filtered salt solution to obtain salt.

3 0

3 years ago

(1.) Using Beer's Law, How will the absorbance measured for the solutions change as the concentration of aspirin in solutions in

Vesnalui [34]

Answer:

(1) The absorbance of the aspirin in solutions will increase.

(2) [ASA]f = 3.79x10⁻⁴M

(3) [ASA]i = 3.79x10⁻³M

(4) m ASA = 0.171g

Explanation:

The Beer's Law is expressed by:

$A = \epsilon \cdot l \cdot C$ (1)

where A: is the absorbance of the species, ε: is the molar attenuation coefficient, l: is the pathlength and C: is the concentration of the species

(1) From equation (1), the relation between the absorbance of the species and its concentration is directly proportional, so if the aspirin concentration in solutions increases, the absorbance of the solutions will also increase.

(2) Starting in the given expression for the relationship between absorbance and concentration of ASA, we can calculate its concentration in the solution:

$A = 1061.5 \cdot [ASA]$

$[ASA] = \frac{A}{1061.5} = 3.79 \cdot 10^{-4}M$

Therefore, the aspirin concentration in the solution is 3.79x10⁻⁴ M

(3) To calculate the stock solution concentration, we can use the next equation:

$V_{i} [ASA]_{i} = V_{f} [ASA]_{f}$

where Vi: is the stock solution volume=10mL, Vf: is the solution diluted volume=100mL, [ASA]i: is the aspirin concentration of the stock solution and [ASA]f: is the aspirin concentration of the diluted solution

$[ASA]_{i} = \frac{V_{f} \cdot [ASA]_{f}}{V_{i}} = \frac {100mL \cdot 3.79\cdot 10^{-4} M}{10mL} = 3.79 \cdot 10^{-3} M$

Hence, the concentration of the stock solution is 3.79x10⁻³M

(4) To determine the aspirin mass in the tablet, we need to use the following equation:

$m_{ASA} = \eta_{ASA} \cdot M_{ASA} = [ASA]_{i} \cdot V_{0} \cdot M_{ASA}$

where η: is the aspirin moles = [ASA]i V₀, M: is the molar mass of aspirin=180.158g/mol, V₀: is the volume of the volumetric flask=250mL and [ASA]i: is the aspirin concentration in the volumetric flask which is equal to the stock solution=3.79x10⁻³M

$m_{ASA} = 3.79 \cdot 10^{-3} \frac{mol}{L} \cdot 0.250L \cdot 180.158 \frac{g}{mol} = 0.171 g$

Then, the aspirin mass in the tablet is 0.171 g.

I hope it helps you!

5 0

3 years ago