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Marianna [84]
3 years ago
5

For the reaction N2(g) + 3H2(g) <->2NH3(g), what will happen if hydrogen gas was removed from the mixture?

Chemistry
1 answer:
OlgaM077 [116]3 years ago
7 0
There will be a shift towards the reactants because the system will try to increase the amount of hydrogen. 
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Which statements accurately describe volume? Check all that apply. Volume is a physical property of an object. Volume is measure
Alex17521 [72]

Answer:

- Volume is a physical property of an object.

- One unit of volume is the milliliter.

- Liquids and solids have constant volumes.

Explanation:

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This body system is where oxygen gas and carbon dioxide gas are exchanged in our body. *
nexus9112 [7]

Answer:

The answer is the respiratory system

Explanation:

The function of the respiratory system is to move two gases. These two gases are called oxygen and carbon dioxide. Gas exchange takes place in the millions of alveoli in the lungs and the capillaries that envelop them.

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Use the given half reactions to "construct" an electrolytic cell. Zn^2+ + 2 e^---------&gt;Zn E°cell = -0.76 V Cu^2+ + 2 e^-----
Neko [114]

Answer:

See explanation and image attached

Explanation:

The standard cell potential at 298 K is given by;

E°cathode - E°anode

Hence;

E°cell = 0.34 V - (-0.76 V)

E°cell = 0.34 V + 0.76 V

E°cell = 1.1 V

To reduce Zn^2+ to Zn then Zn must be the cathode, hence;

E°cell = (-0.76 V) - 0.34 V

E°cell = -1.1 V

5 0
3 years ago
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al ( s ) + 6 HCl ( aq ) ⟶ 2 AlCl 3 ( aq )
Dovator [93]

Answer:

The volume of hydrogen gas produced at STP is 4.90 liters.

Explanation:

2Al (s) + 6 HCl (aq)\rightarrow 2 AlCl_3 (aq) + 3 H_2 (g)

Moles of aluminium =\frac{3.60 g}{27 g/mol}=0.1333 mol

According to reaction , 2 moles of aluminium gives 3 moles of hydrogen gas.

Then 0.1333 moles of aluminium will give:

\frac{3}{2}\times 0.1333 mol=0.2 moles of hydrogen gas

Volume of 0.2 moles of hydrogen gas at STP = V

Temperature at STP = T = 298.15 K

Pressure at STP = P = 1 atm

n = 0.2 mol

PV = nRT (Ideal gas equation)

V=\frac{nRT}{P}=\frac{0.2mol\times 0.0821 atm L/mol K\times 298.15 K}{1 atm}=4.8956 L\approx 4.90 L

The volume of hydrogen gas produced at STP is 4.90 liters.

4 0
3 years ago
The density of nitric oxide (NO) gas at 0.866 atm and 46.2 degrees celcius is ____ g/L
Artyom0805 [142]

Answer:

 d = 0.992 g/L

Explanation:

Data Given:

Pressure of nitric oxide (NO) = 0.866 atm

Temperature of a gas = 46.2° C

Convert the temperature to kelvin = 46.2° C + 273  

temperature in kelvin = 319.2 K

density of nitric oxide (NO) = ?

Solution:

Density of a gas can be calculated by

                       d = PM /RT

Where

d = density

P = Pressure

M = molar mass of gas

R = ideal gas constant  = 0.0821 L atm mol⁻¹ K⁻¹

T = temperature

So,

Molar mass of NO = 30 g/mol

Put values in the formula:

                        d = PM /RT

           d = 0.866 atm × 30 g/mol / 0.0821 L atm mol⁻¹ K⁻¹ × 319.2 K

           d = 25.98 atm. g/mol / 26.2 L atm mol⁻¹

           d = 0.992 g/L

8 0
3 years ago
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