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2 years ago

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1.36g H2 is allowed to react with 10.1g N2 producing 2.05g NH3 What is the theoretical yield in grams for this reaction under th

e given conditions?
Express your answer to three significant figures and include the appropriate units.

1 answer:

vladimir2022 [97]2 years ago

6 0

here's the answer to your question

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In solid NaCl, the equilibrium separation between neighboring Na+ and Cl- ions is 0.283 nm. Calculate the coulombic energy betwe

const2013 [10]

Explanation:

It is given that r = 0.283 nm. As 1 nm = $10^{-9} m$ .

Hence, 0.283 nm = $0.283 \times 10^{-9} m$

Formula for coulombic energy is as follows.

$U_{coulomb} = -1.748 \frac{e^{2}}{4 \pi \epsilon_{o} r}$

where, e = $1.6 \times 10^{-19}$ C

$\epsilon_{o}$ = $8.85 \times 10^{-12}$

$U_{coulomb} = -1.748 \frac{(1.6 \times 10^{-19}^{2}}{4 \times 3.14 \times 8.85 \times 10^{-12} \times 0.283 \times 10^{-9}}$

= $1.423 \times 10^{-18} J$

As 1 eV = $1.6 \times 10^{-19} J$

So, 1 J = $\frac{1 eV}{1.6 \times 10^{-19}}$

Hence, U = $\frac{1.423 \times 10^{-18} J}{1.6 \times 10^{-19} J}$

= 8.9 eV

Also, 1 J = $\frac{10^{-3} kJ}{6.022 \times 10^{23}mol}$

= $1.67 \times 10^{-27}$ kJ/mol

Therefore, U = $1.423 \times 10^{-18} J \times 1.67 \times 10^{-27}$ kJ/mol

= $2.37 \times 10^{-45} kJ/mol$

7 0

3 years ago

9. You have a mini bottle of pure maple syrup. The full container has a mass of 137

cupoosta [38]

Answer:

A

Explanation:EDGE

7 0

2 years ago

Consider the following balanced equation:

algol [13]

Moles of PF₃ : 4

<h3>Further explanation</h3>

A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.

Reaction

$\tt P_4(s)+6F_2(g)\rightarrow 4PF_3(g)$

1.25 moles of P₄(s) is reacted with 6 moles of F₂(g)

Limiting reactant : the smallest ratio (mol divide by coefficient)

P₄ : F₂ =

$\tt \dfrac{1.25}{1}\div \dfrac{6}{6}=1.25\div 1\rightarrow F_2~limiting~reactant(smallest~ratio)$

mol PF₃ based on mol of limiting reactant(F₂), so mol PF₃ :

$\tt \dfrac{4}{6}\times 6~moles=4~moles$

8 0

3 years ago

Chemistry check please... Thank you!

I am Lyosha [343]

1) We apply the ideal gas equation:
PV = nRT
n = (21300 x 3/1000) / (8.314 x 323)
n = 0.024
Your answer is correct.

2) Total pressure = Partial pressure of Hydrogen + Partial pressure of water
134.7 = 122.4 + Pw
Pw = 12.3 kPa
Your answer is correct

3) The molar fraction, volume fraction and pressure fraction of gasses are the same thing.
Thus, percentage pressure of Oxygen = 10%
Pressure of Oxygen = 2.04 x 10⁴ x 0.1
= 2.04 x 10³ kPa
Your answer is correct

Well done!

3 0

2 years ago

An oxygen atom has a mass of 2.66*10^-23 and a glass of water has a mass of 0.050 kg. What is the mass of 1 mole of oxygen atoms

Nutka1998 [239]

Answer:

16.0 g; 3.1 mol

Explanation:

(a) Mass of O atoms

Mass = 6.022 × 10^23 atoms × (2.66 × 10^-23 g/1 atom) = 16.0 g

(b) Moles of O atoms

0.050 kg = 50 g

Moles = 50 g × (1 mol/16.0 g) = 3.1 mol

4 0

2 years ago

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