1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Paul [167]
3 years ago
14

How do you do this? very confused

Chemistry
1 answer:
Vlad [161]3 years ago
4 0
The problem you have written you almost have it solved.  Take the moles that you have calculated and multiply that by the molecular weight to get the grams.

The STP problem:
use the moles you calculated along with 1 atm for Pressure, and 273 for the temperature and plug into the PV = nRT equation.  (also use 0.0821 for R)

From there you can solve for the volume

Hope this helps!
You might be interested in
Problem PageQuestion While ethanol is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synt
OverLord2011 [107]

Question: The question is incomplete. Below is the complete question and the answer;

While ethanol (CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 50.0 L tank at 22. °C with 24. mol of ethylene gas and 24. mol of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 15.4 mol of ethylene gas and 15.4 mol of water vapor The engineer then adds another 12. mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.

Answer:

Number of moles of ethanol = 11 mol

Explanation:

SEE THE ATTACHED FILE FOR THE CALCULATION

4 0
3 years ago
Which type of bonds do polar covalent bonds break down in chemical reactions?
Vlada [557]

Answer:

(C) im pretty sure is the answer

Explanation:

3 0
3 years ago
A compound contains only nitrogen and oxygen and is 30.5% nitrogen by mass. A gaseous sample of the compound has a density of 3.
MariettaO [177]

Answer : The molecular formula of the compound will be, NO_4

Explanation:

First we have to calculate the mass of nitrogen and oxygen.

As we are given that 30.5 % nitrogen by mass that means 30.5 g of nitrogen present in 100 g of solution.

Mass of nitrogen = 30.5 g

Mass of oxygen = Mass of solution - Mass of nitrogen

Mass of oxygen = 100 g - 30.5 g

Mass of oxygen = 69.5 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of N =\frac{\text{Given mass of N}}{\text{Molar mass of N}}=\frac{30.5g}{28g/mole}=1.09moles

Moles of O = \frac{\text{Given mass of O}}{\text{Molar mass of O}}=\frac{69.5g}{16g/mole}=4.34moles

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 1.09 moles.

For N = \frac{1.09}{1.09}=1

For O = \frac{4.34}{1.09}=3.98\approx 4

Step 3: Taking the mole ratio as their subscripts.

The ratio of N : O = 1 : 4

Hence, the empirical formula for the given compound is NO_4

The empirical mass of given compound is NO_4  = 1(28) + 4(16) = 92 g/eq

To calculate the molecular mass of compound we are using ideal gas equation:

PV=nRT\\\\PV=\frac{w}{M}RT\\\\P=\frac{w}{V}\\times \frac{RT}{M}\\\\P=\rho \frac{RT}{M}

where,

P = pressure of gas = 924 torr = 1.216 atm

Conversion used : (1 atm = 760 torr)

T = temperature of gas = 105^oC=273+105=378K

R = gas constant = 0.0821 L.atm/mole.K

\rho = density of gas = 3.61 g/L

M = molar mass of gas = ?

Now put all the given values in the ideal gas equation, we get:

(1.216atm)=3.61g/L\times \frac{(0.0821L.atm/mole.K)\times (378K)}{M}

M=92.1g/mol

Now we have to calculate the molecular formula of the compound.

The equation used to calculate the valency is :

n=\frac{\text{molecular mass}}{\text{empirical mass}}

n=\frac{92.1}{92}=1

Molecular formula = (NO_4)_n=(NO_4)_1=NO_4

Thus, the molecular formula of the compound will be, NO_4

4 0
3 years ago
How many grams would 3.98 x 10^24 atoms of oxygen weigh
Semenov [28]

Answer:

a little bit

Explanation:

i think

4 0
3 years ago
Read 2 more answers
The presence of hydrogen bond in most molecules is responsible for the following except
-Dominant- [34]
That answer is either 3 or 4, but I truly forgot which of the two.
5 0
3 years ago
Read 2 more answers
Other questions:
  • How many liters of O2 will form at STP if 22.5 g H2O2 react?
    6·1 answer
  • Considering all types of aerosols, what is their net effect on the climate system:
    7·2 answers
  • What Structure keeps harmful chemicals out of the animal cells
    13·2 answers
  • Describe and explain how electrical conductivity occurs in mercury bromide and mercury, in both solid and molten states.
    9·1 answer
  • How many moles of sodium atoms in 255 grams of na2so4
    7·1 answer
  • How can substitution mutation affect a person’s traits?
    11·1 answer
  • Anyone know the answer to this one?
    15·1 answer
  • Gallium (, ) is a metalloid obtained from its salts during the smelting of ores of other elements, like Zinc. has broad applicab
    7·1 answer
  • When was that one moment when you laughed the hardest
    11·2 answers
  • How much aluminum oxide in grams is produced from the reaction of 3.5 moles of oxygen with 4.5 moles of aluminum?
    11·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!