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Chemical Reactions: Stoichiometry and Metals

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1. Calculate the molar mass of the following compounds:
a. sodium selenide
b. Palladium (II) hydroxide

2. Calculate the number of grams in each of the following compounds:
a. 4.0 moles of CaCl2(s)
b. 0.467 moles of (NH4)CO3(s), baking powder

3. Calulate the number of moles in each of the following compounds:
a. 150.0 g of NaBr (s)
b. 60.0g of ZnS(s)

4. Using the balanced chemical equation below, answer the following questions regarding mole relationships:
C3H8(g) + 5O2(g) -->3CO2(g) + 4H2O(g)
a.What are the mole-mole factors or molar rations of the following:
i. Propane to oxygen -->
ii. Water to carbon dioxide ->
iii. Carbon dioxide to oxygen -->
b.How many mole of oxygen gas are required to completely combust 7.0 moles of propane gas?
c.How many moles of carbon dioxide gas are produced from the burning of propane gas in the presence of 15.0 moles of oxygen gas?

5. Using the balanced chemical reaction below, answer the following questions regarding stoichiometry.

2K(s) + Zn(NO3)2(aq) --> Zn(s) + 2KNO3(aq)

a. Determine the mass of zinc metal produced from the reaction 6.0 moles of potassium metal in an excess solution of zinc nitrate.
b. Determine the number of moles of zinc nitrate solution required to react completely with 150.0g of potassium metal.
c. What mass of zinc metal will be produced from the reaction of 300.0 g of Zn(NO3)2 with an excess of potassium metal?

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https://brainmass.com/chemistry/stoichiometry/chemical-reactions-stoichiometry-and-metals-363342

Solution Summary

The following problem helps with various physical chemistry problems. Concepts covered involve molar mass, stoichiometry and metals.

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Stoichiometry worksheet

Question 1

What is the molar mass of propane (C3H8)? Use the average molar masses on the periodic table. Do not include units. Round to two decimal places.

Question 2

What is the percent composition of carbon in sodium carbonate (Na2CO3)? Use the average molar masses on the periodic chart, do not include units, round to two decimal places. Do not include the percent sign.

Question 3

Chemical species on the left of the arrow are called while those on the right of the arrow are called.

Question 4

Chemical species that are dissolved in water are called _____________ solutions.

Question 5

When the following equation is balanced, the coefficient for oxygen is____? Use a number, not a word.
____KCl + ___ O2 --> ___ KClO3

Question 6

Balance the following equations. Use whole numbers. If the coefficient is 1, you must put it in.
C4H10 + O2 --> CO2 + H2O
N2 + H2 --> NH3
Na + Cl2 --> NaCl

Question 7

a. Calculate the number of atoms in 3.4 moles of Ne. Use the format 6.02E+23 for 6.02 x1023.
b. Calculate the number of atoms in 3.4 g of Ne. Use the molar mass to two decimal places.Use the format 6.02E+23 for 6.02 x1023.

Question 8

How many moles of carbon are present in 81.5 g of carbon. Use the molar mass found on the periodic table in the front of your text. Round your answer to two decimal places, do not include units in your answer.

Question 9

How many grams of water (H2O) are found in 1.9 moles of water?Use the molar mass found on the periodic
table in the front of your text. Round your answer to two decimal places, do not include units in your answer.

Question 10

a. How many atoms of hydrogen are in 25.0 g of ammonia (NH3)? Use the format 6.02E+23 for 6.02 x 1023
b. How many atoms of nitrogen are in the same amount of ammonia? Use the molar mass to two decimal places found on the periodic table in the front of your text.

Question 11

A compound with a percent composition by mass of 87.5% N and 12.5% H was recently discovered. What is the empirical formula of this compound?

Question 12

Calculate the percent composition by mass of nitrogen in ammonium nitrate (NH4NO3)

Question 13

What mass of copper(II) nitrate would be produced from the complete reaction of 52.7 g of copper, according to the chemical reaction shown below?
Cu + 2 AgNO3 ----> Cu(NO3)2 + 2 Ag
Use the masses to two decimal places using the periodic chart. Round your answer to two decimal places, do not include units.

Question 14

Anhydrous aluminum oxide can be reduced to aluminum according to thisa chemical equation: 2 Al2O3 (s) ---> 4 Al (l) + 3 O2 (g) Calculate the mass of aluminum oxide reacted if 63.9 g of Al was produced and the percent yield was found to be 89.3%

Question 15

Solid magnesium metal reacts with chlorine gas according to the following equation:
Mg + Cl2 --> MgCl2
What mass of magnesium chloride is formed in the reaction between 7.8 g of Mg and 6.9 g of Cl2
use the masses to two decimal places on the chart. Round your answer to two decimal places, do not include units.

Question 16

Predict the products for the following reactions. Use the format CO2 for CO2. You will also need to balance the equation when finished. Retype the entire balanced equation with products.
a. C2H6 + O2 -->
b. KCl -->

See attached for question 17

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