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atroni [7]
3 years ago
11

20.0 g of Nitrogen is produced when oxygen gas reacts with NO gas. 29.8 L of oxygen is required at STP to produce this 20.0 g of

NO. A.yes B.false
Chemistry
1 answer:
Rainbow [258]3 years ago
3 0

Answer:

There will be produced 30.64 grams of nitrogen dioxide

The statement is false

Explanation:

Step 1: Data given

MAss of nitrogen produced = 20.0 grams

Molar mass of N2 = 28.0 g/mol

Mass of NO = 20.0 grams

Molar mass of NO = 30.01 g/mol

Volume of O2 at STP = 29.8 L

Step 2: the balanced equation

2NO + O2 → 2N02

Step 3: Calculate moles NO

Moles NO = mass NO / molar mas NO

Moles NO = 20.0 grams / 30.01 g/mol

Moles NO = 0.666 moles

Step 4: Calculate moles O2

1 mol O2 at STP = 22.4 L

29.8 L = 29.8/22.4 = 1.33 moles

Step 5: Calculate the limiting reactant

For 2 moles NO we need 1 mol O2 to produce 2 moles NO2

NO is the limiting reactant. IT will completely be consumed (0.666 moles).

O2 is in excess. There will react 0.666/2 = 0.333 moles O2

There will remain 1.333 - 0.333 = 0.997 moles O2

Step 6: Calculate moles NO2

For 2 moles NO we need 1 mol O2 to produce 2 moles NO2

For 0.666 moles NO we'll have 0.666 moles NO2

Step 7: Calculate mass NO2

Mass NO2 = moles NO2 * molar mass NO2

Mass NO2 = 0.666 moles * 46.0 g/mol

Mass NO2 = 30.64 grams

There will be produced 30.64 grams of nitrogen dioxide

The statement is false

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A chemical change is characterized of the formation of new substances or a chemical reaction. There are a number of observations that we can see if this type of change happens. One would be the formation of gas bubbles, this indicates that one of the products is a gas. Another observation would be a formation of a precipitate in the solution, it would indicate that the new solid formed is not soluble in the solution. A permanent color change in the solution would also indicate a chemical change because it may be that the new substance that is formed has its own distinct color when in solution. 
6 0
2 years ago
purification of chromium can be achieved by electrorefining chromium from an impure chromium anode onto a pure chromium cathode
stiv31 [10]

The chromium in the electrolytic solution is present as cr³⁺ will take 6.19 hours  will it take to plate 18.0 kg of chromium onto the cathode if the current passed through the cell is held constant at 45.0 A.

It is given that mass is 18 kg. Converting mass into grams

18 x (1000g / 1 kg)

= 18000 g

So, 18 kg = 18000 g

Now, calculate the number of moles

No. of moles = mass of Cr / molecular mass of Cr

No. of moles = 18000 / 52 g/mole

No. of moles = 346.15 mole

For , Cr³⁺, 3 moles of electrons are required

Hence,

3 x 346.15 mole

1038.45

As 96500 C of charge are present in 1 mole of electrons. As a result, the charge held by 1038.45 mole of electrons will be determined as follows.

= 1038.45mol x  96500 C / mole

= 10.02 x 10⁷ C

As, we know that relation between charge, current and time is as follows.

Q = I x T

Current is given as 45 A

Therefore, charge is calculated  

T = Q / I

T = 100.21 x 10⁶ / 45

T = 2.227 x 10⁶

As there are 3600 seconds in one 1 hour. Converting 2.227 x 10⁶ into hours are

= 2.227 x 10⁶ / 3600 sec/h

= 6.19 hours

Thus, if the current flowing through the cell is maintained constant at 45 A, we may estimate that it will take 6.19 hours to plate 18 kg of chromium onto the cathode.

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4 0
1 year ago
A gas cylinder is filled with argon at a pressure of 177 atm and 25°C. What is the gas pressure when the temperature of the cyli
Elena L [17]

277.79 atm is the calculated gas pressure.

The ideal gas is a fictitious concept used to study how real gases behave by comparing them to their deviations. The pressure-temperature rules are followed by an ideal gas.

177 atm is the initial pressure. The starting temperature is 298 K (25 °C = 25 + 273 °C).

195°C = 195+273

= 468K is the final temperature.

The pressure temperature relation illustrated below can be used to get the final pressure.

P1/T1 = P2/T1

= P1T2/T1

= 177 atm 468 K /298 K

= 277.97 atm

The final pressure is therefore 277.97 atm.

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5 0
1 year ago
Calculate the solubility (in g/L) of CaSO4(s) in 0.500 M Na2SO4(aq) at 25°C . The sp of CaSO4 is 4.93×10^−5 .
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7 0
3 years ago
Look at this balanced chemical reaction: N2 + 3H2 2NH3
stepladder [879]

Answer: A mass of 124457.96 g ammonia is produced by reacting a 450 L sample of nitrogen gas at a temperature of 450 K and a pressure of 300 atm.

Explanation:

Given: Volume = 450 L

Temperature = 450 K

Pressure = 300 atm

Using ideal gas equation, moles of nitrogen are calculated as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = tempertaure

Substitute values into the above formula as follows.

PV = nRT\\300 atm \times 450 L = n \times 0.0821 L atm/mol K \times 450 K\\n = \frac{135000}{36.945}\\= 3654.08 mol

According to the given equation, 1 mole of nitrogen forms 2 moles of ammonia. So, moles of ammonia formed by 3654.08 moles of nitrogen is as follows.

2 \times 3654.08 mol\\= 7308.16 mol

As moles is the mass of substance divided by its molar mass. So, mass of ammonia (molar mass = 17.03 g/mol) is as follows.

Moles = \frac{mass}{molar mass}\\7308.16 = \frac{mass}{17.03 g/mol}\\mass = 124457.96 g

Thus, we can conclude that a mass of 124457.96 g ammonia is produced by reacting a 450 L sample of nitrogen gas at a temperature of 450 K and a pressure of 300 atm.

8 0
3 years ago
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