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valina [46]
3 years ago
13

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a flas

k with of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be . Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to significant digits.
Chemistry
1 answer:
marishachu [46]3 years ago
4 0

Answer:

Kp = 2.2 x 10-2

Explanation:

The equation for the decomposition of NH3 is as follows:

2NH3(g) <-------------> N2(g) + 3H2(g)

Initially only NH3 present

PNH3 = 2.3 atm

at equilibroum

PH2 = 3 x PN2 = 0.69 atm;

Therefore;

PN2 = 0.69 atm/3

= 0.23 aatm

PNH3 = 2.3 - 2(0.23) = 1.84 atm

Kp = (PN2) (PH2)3 / (PNH3)2

Kp = (0.23) (0.69)3 / (1.84)2

Kp = (0.23) (0.33) / (3.39)

Kp = 0.6912 / 1.44

Kp = 0.0224

Kp = 2.2 x 10-2

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If 0.100 moles of AgNO₃ react with 0.155 moles of H₂SO₄ according to this UNBALANCED equation below, what is the mass in grams o
AlekseyPX

Answer:

15.6g Ag2SO4

Explanation:

2AgNO3 + H2SO4 --> Ag2SO4 + 2HNO3

-2x              -x

0.1-2x.       0.155-x

x=0.05      x=0.155

0.05mol Ag2SO4 x 311.78g = 15.6g Ag2SO4

4 0
3 years ago
What is the function of the load in<br> an electric circuit?
mezya [45]

Answer:

The source side of the circuit includes all parts of the circuit between the positive side battery post and the load. The load is any device in the circuit that produces light, heat, sound or electrical movement when current is flowing. A load always has resistance and consumes voltage only when current is flowing.

Explanation:

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8 0
2 years ago
Read 2 more answers
How many moles of dipyrithione contain 6.3×1024  atoms of nitrogen?
chubhunter [2.5K]

Answer:

5.23 moles of C₁₀H₈N₂O₂S₂

Explanation:

In order to find the moles of dipyrithione we need to know its formula:

C₁₀H₈N₂O₂S₂

1 mol of N contains 6.02×10²³ atoms

We need to find out the moles of 6.3×10²⁴ atoms of N

6.3×10²⁴ atoms . 1 mol /6.02×10²³ atoms = 10.4 moles of N

Therefore, we know that 1 mol of dipyrithione has 2 moles of N, so we need to make this rule of three:

2 moles of N are contained in 1 mol of C₁₀H₈N₂O₂S₂

10.4 moles of N must be contained in (10.4 . 1) /2 = 5.23 moles of C₁₀H₈N₂O₂S₂

7 0
3 years ago
Read 2 more answers
The molar mass of element X is 42.3 grams per mol and the molar mass for
Drupady [299]

Answer:

X5Y2

Explanation:

% composition of X = 52.2%

% composition of Y = (100 - 52.2) = 47.8%

This means that there are 52.2g of X and 47.8g of Y in the compound

To calculate the empirical formula of the compound, we first convert the gram value to mole value by dividing by their molar masses.

X = 52.2g/42.3g/mol = 1.234mol

Y = 47.8g/96.7g/mol = 0.494mol

Next, we divide each mole value by the smallest value (0.494mol)

X = 1.234mol ÷ 0.494mol = 2.49

Y = 0.494mol ÷ 0.494mol = 1

We multiply each value by 2

X = 2.49 × 2 = 4.98

Y = 1 × 2 = 2

The simple ratio of X:Y is 5:2, hence, their empirical formula is X5Y2.

7 0
3 years ago
Gaseous chlorine dioxide (ClO2) is used in bleaching flour and municipal water treatment in
trapecia [35]

Taking into account the ideal gas law, the pressure is 2.52 atm.

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas are related by a simple formula called the ideal gas law. This equation relates the three variables if the amount of substance, number of moles n, remains constant. The universal constant of ideal gases R has the same value for all gaseous substances. The numerical value of R will depend on the units in which the other properties are worked.

P×V = n×R×T

In this case, you know:

  • P=?
  • V= 500 L
  • n= 52.1 moles
  • R= 0.082\frac{atmL}{molK}
  • T= 22 C= 295 K (being 0 C=273 K)

Replacing in the ideal gas law:

P×500 L = 52.1 moles ×0.082 \frac{atmL}{molK} ×295 K

Solving:

P= (52.1 moles ×0.082 \frac{atmL}{molK} ×295 K)÷ 500 L

<u><em>P= 2.52 atm</em></u>

Finally, the pressure is 2.52 atm.

Learn more about ideal gas law:

  • brainly.com/question/4147359?referrer=searchResults
5 0
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