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hoa [83]
2 years ago
14

Acceleration always refers to a(n)

Chemistry
2 answers:
Harman [31]2 years ago
8 0
B, increase in speed
konstantin123 [22]2 years ago
6 0

Answer:

increase in speed

Step-by-step explanaton:

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Urea, CO(NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is th
Pachacha [2.7K]

Answer:

5.004kg

Explanation:

Combustion of carbon

C+O2=CO2

from the relationship of molar ratio

mass of carbon/molar mass of carbon=volume of CO2 produced\molar vol(22.4 dm3)

mass of carbon =1000kg

atomic mass of carbon =12

volume of CO2 produced=1000×22.4/12

volume of CO2 produced =1866.6dm3

from the combustion reaction equation provided

CO2 (g) + 2NH3 (g) ⟶ CO (NH2 )2 (s) + H2 O(l)

applying the same relationship of molar ratio

no of mole of CO2=no of mole of urea

therefore

vol of CO2\22.4=mass of urea/molar mass of urea

molar mass of urea=60.06g/mol

from the first calculation

vol of CO2=1866.6dm3

mass of urea=1866.6×60.06/22.4

mass of urea=5004.82kg

7 0
3 years ago
Read 2 more answers
The concentration of urea in a solution prepared by dissolving 16 g of urea in 20 g of H2OH2O is ________% by mass. The molar ma
Arada [10]

Answer:

44

Explanation:

Given that :

Mass of solute = Mass of urea = 16g

Mass of water = 20g

Mass of solution = (mass of solute + mass of solvent) = (mass of urea + mass of water) = (16g + 20g) = 36g

Percentage Mass = (mass of solute / mass of solution) * 100%

Percentage Mass = (16 / 36) * 100%

Percentage Mass = 0.4444444 x 100%

Percentage Mass = 44.44%

Percentage Mass = 44%

4 0
2 years ago
Calculate the density of nitrogen gas, in grams per liter, at stp.
lesantik [10]

Standard temperature is 273 K

Standard pressure is 1 atm

We use the ideal gas equation to find out density of nitrogen gas in g/L

Ideal gas equation:

PV = nRT\\  PV = (\frac{Mass}{Molar mass)}RT\\   P(Molar mass) = (\frac{Mass}{Volume})RT\\  \frac{Mass}{Volume}=\frac{P(molar mass)}{RT} \\  Density = \frac{P(Molar mass)}{RT}

Molar mass of N_{2} = 28 g/mol

Pressure = 1 atm

Temperature = 273 K

Density = \frac{(1atm)(28 g/mol)}{(0.08206 \frac{L.atm}{mol.K})(273 K)}

= 1.25 g/L

Therefore, density of nitrogen gas at STP is 1.25 g/L

4 0
3 years ago
A 3.5-g sample of colorado oil shale is burned in a bomb calorimeter, which causes the temperature of the calorimeter to increas
Lubov Fominskaja [6]
<span>q(rxn) = - [q(water)+q(bomb)] q(rxn) = -{[ (1000g)(4.184)(5.0)] + [ (5.0)(0.10)]} q(rxn) = - (20920 + 0.5) Now we divide 3.5g q(rxn)= - (20920)/(3.5g) q(rxn) = 5977.14 And final answer, change is to Kilo joule unit -q(rxn) = 5.23 KJ/unit</span>
3 0
2 years ago
Read 2 more answers
(08.02
bogdanovich [222]

Answer:

b. The molarity of the solution increases

Explanation:

The correct answer is option b, that is the molarity of the solution increases.

Because the molarity is the concentration of the solution and it is explained as the amount of solute in amount of solution.

Solution: is the solute dissolved in solvent.

So if we increases the amount of solute in solvent the concentration in terms of molarity of solution increases and if we increase amount of solvent or water then the concentration or molarity increases.

Suppose we have form a sugar solution of 1 L by adding 4 mole of sugar then what happen

Use the Molarity formula

Molarity = no. of moles / 1 L of solution

put values in the formula

Molarity = 4/ 1 L of solution = 4 M

So the molarity of solution is 4 now if we add 2 mole more sugar to the same amount of sugar and amount of solution remain the same

now the no. of moles of sugar = 6 mole

So,

Use the Molarity formula

Molarity = no. of moles / 1 L of solution

put values in the formula

Molarity = 6 mol / 1 L of solution = 6 M

So the correct option is b.

7 0
3 years ago
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