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Katarina [22]
3 years ago
15

How many grams of hydrogen are needed to react with 1.40 g of nitrogen to produce ammonia?

Chemistry
1 answer:
vazorg [7]3 years ago
8 0

Answer:

Write a balanced chemical reaction:

N2 + 3H2 ==> 2NH3

Looking at the mole ratios in this balanced equation you can see it takes 3 moles H2 to make 2 moles NH3.  So, next calculate the moles of NH3 represented by 1.80 g and then convert to moles of H2 needed:

moles of NH3 = 1.80 g x 1 mole/17 g = 0.106 moles NH3

Moles H2 needed = 0.106 moles NH3 x 3 moles H2/2 moles NH3 = 0.159 moles H2 needed

Grams H2 needed = 0.159 moles x 2 g/mole = 0.318 grams H2 needed

Explanation:

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Answer:

a) ^{131}_{53} I

b) ^{192}_{77} Ir

c) ^{153}_{62} Sm

Explanation:

The symbols of the isotopes are written like

^{A}_{Z} X

where,

X is the element

A is the mass number (protons + neutrons)

Z is the atomic number (protons)

<em>a) Iodine-131</em>

The atomic number of iodine is 53. The mass number of this isotope is 131. The symbol is ^{131}_{53} I.

<em>b) Iridium-192</em>

The atomic number of iridium is 77. The mass number of this isotope is 192. The symbol is ^{192}_{77} Ir.

<em>c) Samarium-153</em>

The atomic number of samarium is 62. The mass number of this isotope is 153. The symbol is ^{153}_{62} Sm.

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Explanation:

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