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Chemistry: An Atoms First Approach

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 10ALQ

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Question

nar vest completes the statement or answers the question.
1) How many grams of N2 are produced when 125 g of NH3 reacts as shown in the following
balanced equation?
4NH3+6NO5N2+6H20
boobihou
D) 257 g
E) 165 g
B) 145 g
C) 7.35 g
A) 206 g

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Phosphine gas reacts with oxygen according to the following equation: 4PH3(g)+8O2(g)P4O10(s)+6H2O(g) Calculate (a) the mass of tetraphosphorus decaoxide produced from 12.43 mol of phosphine. (b) the mass of PH3 required to form 0.739 mol of steam. (c) the mass of oxygen gas that yields 1.000 g of steam. (d) the mass of oxygen required to react with 20.50 g of hosphine.
The coefficients in the chemical reaction 2A+3B products give us a relationship between which of the following: a. grams of A and grams of B b. density of A and density of B c. moles of A and moles of B
Consider the equation 2A + B . A2B. If you mix 1.0 mole of A with 1.0 mole of B, what amount (moles) of A2B can be produced?
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l)+O2(g)CO2(g)+H2O(l) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
In an actual experiment, 9.0 moles of H2 and 2.0 moles of N2 are consumed, and 0.50 moles of NH3 are produced. What is the percent yield of this experiment? N2(g) + 3H2(g) → 2NH3 (g)
How many moles of H3PO4 are produced when 78.5 g P4O10 reacts completely to form H3PO4?
48.0 g of solid aluminum (Al) is combined with 150.0 grams of iron (III) oxide to form 85.0 grams of aluminum oxide and some amount of iron as shown in the equation below. Calculate the percent yield of aluminum oxide. 2Al + Fe2O3 -> Al2O3 + 2Fe
How many grams of H2 are required to produce 7.50 grams of ammonia NH3? Use the balanced equation (this time the equation is already balanced): N2(g)+3H2(g)⟶2NH3(g)N2g+3H2g⟶2NH3(g)
Using the equation below, calculate the number of grams of N2 that are formed from the reaction of 21 grams of NH3. 4NH3 + 3O2 --> 2N2 + 6H2O
Propane gas, C3H8(g) , is used for barbeques. If 12.3 g of propane is combusted completely in a sufficient supply of oxygen gas, what mass of carbon dioxide gas is produced? C3H8(g) +5 O2(g) --> 3 CO2(g) +4H2O(g)
When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. Condition #1: C(s) + O2 (g) --> CO2 (g) However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. Condition #2: 2 C(s) + O2 (g) -->2 CO (g) What mass of CO (g) and CO2 (g) is expected when a 5.00 gram sample of pure carbon is burned under each of these two conditions listed above? Condition #1: Condition #2:
Using the balanced equation from Question #8, how many grams of lead will be produced if 2.54 grams ofPbS is burned with 1.88 g of O2? Express your answer to the correct number of significant figures and youmust show all work in the form of dimensional analysis as shown in Lesson 4. (Hint: be sure to work theproblem with both PbS and O2). Grams of lead II sulfide to mol of lead II sulfide. Compare lead sulfide to lead and calculate grams of lead.

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