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Nostrana [21]
3 years ago
15

How many moles of nitrogen are needed to completely convert 6.34 mol of hydrogen?

Physics
2 answers:
Sergeu [11.5K]3 years ago
5 0

Answer:

n = 2.11 moles

Explanation:

As we know by the reaction of hydrogen and nitrogen

N_2 + 3H_2 --> 2NH_3

so here from above equation we know that for complete conversion of 3 moles of hydrogen we need 1 mole of nitrogen

so here we know that 6.34 moles of hydrogen is available

so we require 1/3 times of moles of nitrogen for complete reaction

so number of moles of hydrogen will be

n = \frac{1}{3} \times 6.34

n = 2.11 moles

so here we can say it requires 2.11 moles of nitrogen for complete reaction of 6.34 moles of hydrogen

____ [38]3 years ago
4 0
If we use the equation:
N2 + 3H2 --> 2NH3
Then
1 mol of Nitrogen required 3 moles of Hydrogen
x mols : 6.34mols
X = 6.34/3
X = 2.11 moles of Nitrogen are required.
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The  kinetic energy is KE  =  7.59  *10^{10} \  J

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From the question we are told that

       The  radius of the orbit is  r =  2.3 *10^{4} \ km  = 2.3  *10^{7} \ m

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substituting this into the equation

      KE  =  \frac{ 1}{2} *\frac{GMm}{r}

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     KE  =  \frac{ 1}{2} *[\frac{GMm}{r^2}] * r

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3 years ago
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Answer:

See the answers below.

Explanation:

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E_{A}=E_{B}

The important thing about this problem is to identify the types of energy at each point. Let's take the reference level of potential energy at a height of zero meters. That is, at this point the potential energy is zero.

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E_{B}=m*g*h+\frac{1}{2}*m*v^{2}

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