How many grams of ammonia (nh3) are produced if 4 grams of hydrogen gas (h2) reacts with excess nitrogen gas (n2) according to the chemical equation below:

3 h2 + n2 à 2 nh3

2.43 g

4.86 g

11.33 g

22.66 g

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question 6

identify the limiting reactant if 5 g of n2 is allowed to react with 5 g of h2 according to the chemical equation given below. determine the theoretical yield of the product nh3.

3 h2 + n2 à 2 nh3

limiting reactant is h2 ; theoretical yield = 6.07 g of nh3

limiting reactant is h2 ; theoretical yield = 28.33 g of nh3

limiting reactant is n2 ; theoretical yield = 6.07 g of nh3

limiting reactant is n2 ; theoretical yield = 28.33 g of nh3

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question 7

for a given chemical reaction, the chemist determined the theoretical yield of product is equal to 15.1 grams. in the laboratory, the chemist only recovered 8.25 grams of product (the actual yield). calculate the percent yield.

32.7%

48.9%

54.6%

82.3%

Base from the chemical reaction :3 H2 + N2 à 2 NH3

Given 4 g H2

Mass NH3 = 4 g H2 ( 1 mole H2 / 2 g H2) ( 2 mol NH3 / 3 mol H2) ( 17 g NH3 / 1 mol NH3) 

mass NH3= 22.66 g NH3 produce from 4 g H2

the correct answer is answer a. a mixture

no other options make sense

hope this

have a great day : )

  - sprinkles

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.