1 N₂ + 3 H₂ = 2 NH₃
Mole ratio <span> of hydrogen to ammonia :
3 moles H</span>₂ : 2 moles NH₃ or 3 : 2
hope this helps!
I don’t understand the question sorry
Answer: -
C. The hydrogen at 10 °C has slower-moving molecules than the sample at 350 K.
Explanation: -
The kinetic energy of gas molecules increase with the increase in the temperature of the gas. With the increase in kinetic energy, the gas molecules also move faster. Thus with the increase of temperature, the speed of the molecules increase.
Temperature of first hydrogen gas sample is 10 °C.
10 °C means 273+10 = 283 K
Thus first sample temperature = 283 K
The second sample temperature of the hydrogen gas is 350 K.
Thus the temperature is increased.
So both the kinetic energy and speed of molecules is more for the hydrogen gas sample at 350 K.
Thus the hydrogen at 10 °C has slower-moving molecules than the sample at 350 K.
Hence the answer is C.
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The volume increases and the final volume is 2.1 L
<h3>Why volume increases?</h3>
The volume of a gas is directly related to the heat and pressure. If temperature increases, volume increases.
If pressure increases, volume decreases
Based on Boyle's law,
The absolute temperature of a gas is directly proportional to the volume of the gas.
As the balloon change increases its temperature, the volume increases
The Boyle's equation is:
V₁T₂ = V₂T₁
Where,
- V is volume
- T is absolute temperature of 1, initial state and 2, final state of the gas.
Replacing :
V₁ = 2.0L
T₂ = 35°C + 273.15 = 308.15K
V₂ = ?
T₁ = 25°C + 273.15 = 298.15 K
2.0L x 308.15 K = V₂ x 298.15 K
2.1 L = V₂
Final volume is 2.1L
Hence, The volume increases and the final volume is 2.1 L
Learn more about gas laws here ;
brainly.com/question/12669509
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