Some basic concepts of chemistry class 11 ncert solutions 






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Answer: i 1 mole of C 2H 6 contains 2 moles of carbon atoms. It includes the basic concepts, formulas reactants, reagents, products, catalysts and all that will help to deal with chemistry in the simplest form.
The mass of a substance is constant whereas its weight may vary from one place to another due to change in gravity. The total significant figures are 3. L aw of Definite Proportions or Law of Constant Composition: This law was proposed by Louis Proust in 1799, which states that: 'A chemical compound always consists of the same elements combined together in the same ratio, irrespective of the method of preparation or the source from where it is taken'.
Answer: Molar mass of argon is the average molar mass and may be calculated as : Question 33. It states that matter can neither be created nor destroyed. In simple terms, molecular mass of a substance expressed in grams is called gram molecular mass. Convert the given quantities into basic units: i 29. How many significant figures should be present in the answer of the following calculations? An empirical formula represents the simplest whole number ratio of various atoms present in a compound whereas the molecular formula shows the exact number of different types of atoms present in a molecule of a compound. A 5 % solution of sodium chloride means that 5 g of NaCl is present in 100g of the solution. In such situations, one reactant is in excess over the other. Nowadays when you go inside a home, almost all the people inside the home will have a mobile phone individually. Calculate the molarity of a solution of ethanol in water in which mole fraction of ethanol is 0. Law of Conservation of Mass.
NCERT Solutions for Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry - We are not responsible for any type of mistake in data.
The percentage of different elements present can be calculated as : Question 3. Determine the empirical formula of an oxide of iron which has 69-9% iron and 30-1% oxygen by some basic concepts of chemistry class 11 ncert solutions. Writing the empirical formula of the compound. Calculate the amount of carbon dioxide that could be produced when i 1 mole of carbon is burnt in air. This means that dioxygen is in limited amount or-it is the limiting reactant. Molar mass of sodium acetate is 82. Calculate the concentration of nitric acid in moles per litre in a sample which has a density 1-41 g mL-1 and the mass per cent of nitric acid in it being 69%. How much copper can be obtained from 100 g of copper sulphate CuS0 4. Determine the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69. Calculate the average atomic mass of chlorine from the following data : Isotope % Natural Abundance Atomic mass Answer: Question 10. In three moles of ethane C 2H 6calculate the following : i No. What is the concentration of sugar C 12H 22O 11 in mol L -1 of some basic concepts of chemistry class 11 ncert solutions are dissolved in enough water to make final volume upto 2 L. Answer: The concentration in mol L -1 means molarity M. If the density of methanol is 0. Pressure is determined as force per unit area of the surface. It is equal to the mass of the proto type of the kilogram. It is infact, the mass of a platinum block stored at the international Bureau of Weights and Measurements in France. What do you understand by significant figures. Answer: We have seen that every measurement done in the laboratory involves same error or uncertainty depending upon the limitation of the measuring instrument. According to this, all digits repotted in a given data are certain except the last one which is uncertain or doubtful. For example, let us suppose that the reading as reported by a measuring scale is 11-64. It has four digits in all. Thus, the number may be reported as follows : Thus, the significant figures in any number are all certain digits plus one doubtful digit. It may be noted all digits reported in a number are significant. However, only the last digit is uncertain while the rest are certain. Thus, the number 11-64 has all the four digits as significant figures. Out of them 1, 1 and 6 are certain while 4 has some uncertainty about it. The level of contamination was 15 ppm by mass i Express this in percent by mass. How many significant figures are present in the following. Round up the following upto three significant figures : i 34. The following data is obtained when dinitrogen and dioxygen react together to form different compounds : Answer: By keeping 14 g as the fixed mass of dinitrogen N 2the ratios by mass of dioxygen O 2 combining with 14 g dinitrogen are : 16 : 32 : 16 : 40 or 2 : 4 : 2 : 5. Since this ratio is simple whole number, the data obeys the Law Multiple Proportions. If the speed of light is 3. Identify the limiting reactant if any in the following reaction mixtures. If yes, which one and what would be its mass. If 10 volumes of dihydrogen react with five volumes of dioxygen gas, how many volumes of water will be produced. Answer: 10 volumes of water vapours will be produced. Convert the following into basic units i 28. Which of the following has largest number of atoms. Calculate the molarity of a solution of ethanol in water in which mole fraction of ethanol is 0. In this case, the volume of solution is considered to be the same as that of the solvent i. What will be mass of one 12C in g. How many significant figures should be present in the answer of the following calculations. Answer: i The least precise figure 0. Therefore, the answer should have three significant figures. Therefore, the answer should be reported upto four significant figures. The exact figure 5 is not considered in this case. Therefore, the answer should be reported upto three significant figures. Use the data given in the following table to calculate the molar mass of naturally occurring argon. Answer: Molar mass of argon is the average molar mass and may be calculated as : Question 33. Calculate the number of atoms present in : i 52 moles of He ii 52 u of He iii 52 g of He. A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it in oxygen gives 3. Calculate i empirical formula ii molar mass and iii molecular formula of the gas. Calculation of mass percent of carbon and hydrogen. Determination of empirical formula of fuel gas. Calculation of molecular mass of fuel gas. Calculation of molecular formula of the gas.