Concept explainers
a) How many molecules are in
b) How many atoms are in
c) How many atoms are in
d) What is the mass of
e) What is the mass of
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Chapter 7 Solutions
Introductory Chemistry: An Active Learning Approach
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- Two general chemistry students working together in the lab weigh out 0.832 g of CaCl2 2 H2O into a crucible. After heating the sample for a short time and allowing the crucible to cool, the students determine that the sample has a mass of 0.739 g. They then do a quick calculation. On the basis of this calculation, what should they do next? (a) Congratulate themselves on a job well done. (b) Assume the bottle of CaCl2 2 H2O was mislabeled; it actually contained something different. (c) Heat the crucible again, and then reweigh it.arrow_forwardYou have a pure sample of apholate, C12H24N9P3, a highly effective commercial insecticide. Calculate the molar mass of apholate. Calculate the mass of N in 100. g apholate. A sample containing 250.0 mg apholate is sprayed on an agricultural field. Calculate the mass of phosphorus in this sample of apholate; express your result in grams. Calculate the number of phosphorus atoms in this sample of apholate.arrow_forwardA compound R2O3 is 32.0% oxygen. What is the molar mass of R2O3? What is the element represented by R?arrow_forward
- Capsaicin, the compound that gives the hot taste to chili peppers, has the formula C18H27NO3. (a) Calculate its molar mass. (b) If you eat 55 mg of capsaicin, what amount (moles) have you consumed? (c) Calculate the mass percent of each element in the compound. (d) What mass of carbon (in milligrams) is there in 55 mg of capsaicin?arrow_forwardThe mass of 2.50 mol of a compound with the formula ECl4, in which E is a nonmetallic element, is 385 g. What is the molar mass of ECl4? What is the identity of E?arrow_forwardMorphine, a narcotic substance obtained from opium, has the molecular formula C17H19NO3. What is the mass percentage of each element in morphine (to three significant figures)?arrow_forward
- When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of FeO and Fe2O3. In a certain experiment, 20.00 g iron metal was reacted with 11.20 g oxygen gas. After the experiment, the iron was totally consumed, and 3.24 g oxygen gas remained. Calculate the amounts of FeO and Fe2O3 formed in this experiment.arrow_forward3.117 For the oxides of iron, FeO, Fe2O3, and Fe3O4, describe how you would determine which has the greatest percentage by mass of oxygen. Would you need to look up any information to solve this problem?arrow_forwardAtomic masses are relative masses. What does this mean?arrow_forward
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