Principles of General Chemistry
3rd Edition
ISBN: 9780073402697
Author: SILBERBERG, Martin S.
Publisher: McGraw-Hill College
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Chapter 3, Problem 3.83P
(a)
Interpretation Introduction
Interpretation: Mass of
Concept introduction: The formula to convert mass in grams to moles is as follows:
For some stoichiometric balanced equation; the reactant that is present in the smallest amount is consumed completely to form the product and thus governs the product formation.This reactant is known as limiting reactant.On the basis of the stoichiometric ratio by which substrates combine, the moles of product formed from each reactant can be calculated.
The formula to convert moles to mass in grams is as follows:
(b)
Interpretation Introduction
Interpretation:Total moles of gaseous products formed are to be calculated.
Concept introduction: The formula to convert mass in grams to moles is as follows:
The formula to convert moles to mass in grams is as follows:
(c)
Interpretation Introduction
Interpretation:Molecules of water vapor formed is to be calculated.
Concept introduction: The formula to convert mass in grams to moles is as follows:
The formula to convert moles to mass in grams is as follows:
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Students have asked these similar questions
Consider the balanced chemical reaction shown below.
2 CHg(g) + 9 029) → 6 CO,(9) + 6 H20()
In a certain experiment, 6.773 g of CHg(g) reacts with 4.068 g of 0,(0).
(a) Which is the limiting reactant? (Example: type C3H6 for CHg(g))
is the limiting reactant.
(b) How many grams of CO,(9) form?
o of Co,(9) form.
(c) How many grams of H,O) form?
g of H20() form.
(d) How many grams of the excess reactant remains after the limiting reactant is completely consumed?
g of excess reactant remain.
The sample is analyzed and found to contain three elements, C, H and O. A 2.147 g sample of the compounds burns in O2(g) to produce 4.297 g of CO2(g) and 1.757 g of H2O(g).
(a) Calculate the moles of C in the sample.
(b) Calculate the moles of H in the sample.
(c) Calculate the moles of O in the sample.
(d) Determine the empirical formula for the compound.
1.
(a) For the double displacement reaction and find the mole ratio between the product and reactant for the constituents that contain the element: magnesium.
(b) Assume that you have 2.8 moles of the reactant that contains your element, how many moles of the product are created? (HINT: use the ratio above to find the moles of product)
(c) What is the average molar mass of the reactant and product that contains your element (g/mol)?
Reactant:
Product:
(d) Assume you have 100 grams of the reactant, how many moles does that represent. (HINT: use average molar mass above to convert the grams to moles)
2.
(a) How many moles of the product are created? (HINT: use the mole ratio above to convert the moles of reactant to moles of the product)
Moles of product:
(b) Convert the moles of the product to grams. (HINT: use the average molar mass of the product to convert the moles to grams)
Grams of product:
3.
Assume that a certain amount of the second reactant produced 4 moles of product that…
Chapter 3 Solutions
Principles of General Chemistry
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