8. If an atom has 35 protons in the nucleus, how many electrons will it have orbiting the nucleus?
1 answer:
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Answer:
1. 9.4 grams of methane produce<u> 25.85</u> grams of CO2
2.Grams of water produced = <u>11.81 grams</u>
3.Mass of Methane produced by 10.1 gram of O2 = <u>2.52 grams</u>
4.Amount of methane consumed = <u>46.9 grams</u>
5. Grams of Co2 produced =<u> 8.32 grams</u>
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Explanation:
Molar masses :
Methane = CH4 = mass of C + 4x (mass of H)
CH4 = 12 +4(1) = 16 grams
<u>1 mole of CH4 = 16 gram</u>
Oxygen O2 = 2 x (mass of O) = 2x(16) = 32 gram (1 mole of O2 =32 gram)
Carbon Dioxide =CO2 = mass of C + 2(mass of O)
= 12 + 2(16)
= 44 grams <u>(1 mole of CO2 = 44 gram )</u>
Water = H2O = 18 grams ( 1 mole of H2O = 18 gram)
1 mole of each molecule is equal to their molar masses
The balanced equation is :
According to Stoichiometry :
1 mole of CH4 = 2 Mole of O2 = 1 mole of CO2 = 2 mole of H2O
1. From the equation ,
1 mole of methane produce =1 mole of CO2
16 gram of methane = 44 gram of CO2
1 gram of methane =
gram of CO2
9.4 gram of CH4 =
gram of CO2
= 25 .85 gram of CO2
2.
2 mole of O2 produces = 2 mole of H2O(water)
1 mole of O2 produces = 1 mole of H2O
32 gram of O2 = 18 gram of water
1 gram of O2 =
21 gram of O2 =
11.81 gram of water
3. 1 mole of CH4 = 2 mole of O2
16 gram of CH4 = 2(32) = 64 grams of O2
64 gram of O2 needs = 16 grams of CH4
1 gram of O2 needs =
10.1 gram of O =
of CH4
= 2.52 gram
4.
1 mole of CO2 is produced from = 1 mole of CH4
44 gram of CO2 is produced from 16 gram of CH4
1 gram CO2 =
gram of CH4
129 gram of CO2 =
gram of CH4
= 46.90 grams
5.
2 mole of O2 produce = 1 mole of CO2
2x 32 gram of O2 = 44 gram of CO2
1 gram of O2 =
of CO2
12.1 gram of O2 produce=
of CO2
= 8.318 gram
Note : Write the quantity give on left side of "="
write the substance asked on right side of "="
An oxide of nitrogen contains 30.45 mass % N, if the molar mass is 90± 5 g/mol the molecular formula is N₂O₄.
<h3>What is molar mass?</h3>The molar mass of a chemical compound is determined by dividing its mass by the quantity of that compound, expressed as the number of moles in the sample, measured in moles. A substance's molar mass is one of its properties. The compound's molar mass is an average over numerous samples, which frequently have different masses because of isotopes.
<h3>How to find the molecular formula?</h3>The whole-number multiple is defined as follows.
Whole-number multiple =
The empirical formula mass is shown below.
Mw of empirical formula = Mw of N+ 2 x (Mw of O)
= 14.01 g/mol + 2 x (16.00 g/mol)
= 46.01 g/mol
With the given molar mass or the molecular formula mass, we can get the whole-number multiple for the compound.
Whole-number multiple = ≈ 2
Multiplying the subscripts of NO2 by 2, the molecular formula is N(1x2)O(2x2)= N2O4.
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