Question 1: Select the best answer for the following questions? 1. Number of ions in 0.5 mole of Hg2Cl2 is equal to: A. 1.2x1024 B. 9.3x1023 C. 3.01x1023 D. 6.02 x1023 2. Mass of one sodium atom equal: А. 23 amu B. 3.8 x1023 С. 3.8 х1023 D. A and C are true 3. The density of chemical substances is classified as property: А. Intensive B. Extensive physical C. Chemical D. Intensive and chemical physical 4. When AGNO3 dissolved in water is an example on А. Chemical B. Physical Property C. Physical Change D. Chemical Property Change 5. Describe the accuracy and precision of the image: A. Accurate and B. Precise and not C. Accurate and D. Not accurate neither accurate. Precise. precise. not Precise. 6. Which is the product of these numbers, to the appropriate number of significant digits? (013.012 X 21.30) 7. 12 + (32. 15 – 25.063) A.45.49 B.46.0 C.45.5 D. 46.01 7. Which of the structures shown below represent isotopes? 238 Y 235 234 234 w 92 92 93 92 A. Z and W B. X and Y C. X and Z D. X, Y and Z 8. The best chemical formula that describes the ionic compound made from Barium and phosphate is: А. Вaз(РО4)2 В. Ва- (РО4) C. Ba3(PO4) D. Ba(PO4) 1

Question 1: Select the best answer for the following questions? 1. Number of ions in 0.5 mole of Hg2Cl2 is equal to: A. 1.2x1024 B. 9.3x1023 C. 3.01x1023 D. 6.02 x1023 2. Mass of one sodium atom equal: А. 23 amu B. 3.8 x1023 С. 3.8 х1023 D. A and C are true 3. The density of chemical substances is classified as property: А. Intensive B. Extensive physical C. Chemical D. Intensive and chemical physical 4. When AGNO3 dissolved in water is an example on А. Chemical B. Physical Property C. Physical Change D. Chemical Property Change 5. Describe the accuracy and precision of the image: A. Accurate and B. Precise and not C. Accurate and D. Not accurate neither accurate. Precise. precise. not Precise. 6. Which is the product of these numbers, to the appropriate number of significant digits? (013.012 X 21.30) 7. 12 + (32. 15 – 25.063) A.45.49 B.46.0 C.45.5 D. 46.01 7. Which of the structures shown below represent isotopes? 238 Y 235 234 234 w 92 92 93 92 A. Z and W B. X and Y C. X and Z D. X, Y and Z 8. The best chemical formula that describes the ionic compound made from Barium and phosphate is: А. Вaз(РО4)2 В. Ва- (РО4) C. Ba3(PO4) D. Ba(PO4) 1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How many molecules are in 98.70 grams of Ba (SO4)? A. 2.5 x 1023 molecules Ba (SO4) B. 0.6 x 1023 molecules Ba (SO4) C. 1.4 x 1024 molecules Ba (SO4) D. 3.7 x 1023 molecules Ba (SO4)
1. How many ATOMS of nitrogen are present in 6.28 grams of dinitrogen tetrafluoride ? atoms of nitrogen. 2. How many GRAMS of fluorine are present in 1.03x1023 molecules of dinitrogen tetrafluoride ? grams of fluorine.
1. Caffeine is a bitter stimulant drug and is found in varying quantities in seeds, leaves, and so on. Its formula is C8H10N4O2. Use the example above to answer the following questions. b) The number of mol of hydrogen in 4.1 mol of caffeine.
1 mole of carbon atoms correspond to ---- number of carbon atoms. Question 5 options: 12 6.02 x 1023 12 g 10.0 g
Element is Gold use 6.02 x 1023 for Avogadro's number or you may be counted wrong!!! 1. What is the symbol for your element? (Must be after Xe in Periodic Table). Au 2. What is the molar mass of your element? (include units). 197 g/mol 3. How many atoms are in a mole of your element? (No calculation needed) 4. If you have 2.15 x 1024 atoms of your element, how many moles is that? 5. If you have 2.15 x 1024 atoms of your element, how many grams is that? 6. Theoretically speaking, if your element was in the gas state at STP, how many liters is 56.87 grams of your element? (Most elements are not gases at STP so this question is just theoretical) You must solve this using CHM 130 knowledge only.
A sample of a compound has a total mass of 200.0 g. Phosphorus comprises 87.28 g of the sample while oxygen comprises 112.72 g. a. Find the percent mass of phosphorus and oxygen in the sample.b. Find the empirical formula of the compound. c. If the compound has a molar mass of 283.88 g/mol, what is the molecular formula?
Ibuprofen is an anti-inflammatory with the formula C13H18O2 A. What is the molar mass of ibuprofen? Express your answer using four significant figures. B. How many grams of ibuprofen are in 0.505 mole? Express your answer using three significant figures. C. How many moles of carbon are in 12.5 g of ibuprofen? Express your answer using three significant figures. D. How many moles of ibuprofen contain 1.42×1023 atoms of carbon? Express your answer using three significant figures. please solve all stepwise
1. Which quantity has the greater mass? a. 1 mol of Fe atoms or 1 mol of Sn atoms b. 1 mol of Si atoms or 1 mol of Ar atoms c. 1 mol of He atoms or 6.02x1023 H atoms d. 1 mol of Cl atoms or 1 mol of Cl2 molecules e. 1 mol of C₂H4 molecules or 3.01 x 1023 C₂H4 molecules 2. The average nicotine (C10H14N2) content of a Camel cigarette is 1.93 mg. Suppose an individual smokes one pack of 20 cigarettes a day. a. How many moles of nicotine are smoked in a day? b. How many molecules of nicotine are smoked in a day?
Which substance has the largest molar mass A. Water B. Carbon dioxide C. Methane (CH_4) D. Iodine (I_2) E. Hydrogen chloride (HCI)
a. Calculate the number of moles in 21.7 mg of nitrogen dioxide. mol b. Calculate the number of moles in 1.70 g of copper(II) nitrate. mol c. Calculate the number of moles in 2.46 g of carbon disulfide. mol
Consider 68.9 g of Pb(SO4)2 to answer the following questions. a. How many moles of Pb(SO4)2 is this? ____________________________ b. How many molecules of Pb(SO4)2 is this? ____________________________ c. What is the weight of one molecule of Pb(SO4)2 in amu? _________________ d. How many grams are 4.23 x 1022 molecules? __________________________
a. How many moles are in 8.5×10²² atoms Xe? b. How many moles are in 7.4×102 atoms Cu? 23 c. How many grams are in 6.8×10ª atoms Zn? d. How many grams are in 2.0×10“ atoms He? e. How many grams are in 2.75 moles Fe(NO2)3? f. How many grams are in 1.85 moles Ag,SO4? g. How many moles are in 34.2 g KCl? h. How many moles are in 14.8 g Zn(C,H3O2)2? i. How many atoms of oxygen are in 8.1 g CO2? j. How many atoms of hydrogen are in 5.0 g NH;?