11. What is the empirical formula of a compound that has the composition by mass

Question

11. What is the empirical formula of a compound that has the composition by mass of 29.5% N, 3.2%H, 12. Equal masses of the following elements were heated from 15°C to 90°C; copper (s-0.386 J/g°C, 13. Calorimetric analysis shows that for a certain substance, 1,020 calories is required to heat 78.6 grams of 14, A pure substance has a mass of 80.0 g and a specific heat equal to 0.385 Jg1.?". If this substance and 67.3% O? ( H304) ron (s 0.45 JIg°C, lead (s 0.128 J/g°C). Which one required the most energy? the substance from 85°C to 110°C? What is the specific heat of the substance? [0.5 cal/g°c absorbs 300. Joules of heat to become 78.2oC, what was its initial temperature? (68.5°C) 2. In the following reaction, what amount of water must react to absorb 852 kJ of energy? (0.0685 L) Zn(s) + H:0(g) > Zn0(s)+ H2(g) AHn 224 kJ 3. In the following reaction, if 4.0 moles of oxygen completely react, how much energy will be released? 1720 KJ) 4 NHs (g) + 502 (g) 4 NO (g) + 6H20 (g) ????:-904.8 kJ ATOMS 1. Write the ground state electron configuration for the following atoms: sulfur, ron, molybdenum, uranium. 2. For the elements listed in number 1 above, write the ground state orbital notation. 3. Which neutral atom has the same electron configuration as d. H What is the temperature of 5.00 moles of an ideal gas in a 2.8 L container pressurized to 4 240.°C] 4. .8 atm.?[ 5. What is the mass of xenon in a sealed container with a volume of 5.4L at STP? [32 gl 6. A rubber ball is filled with 5.4 L of air at 28°C and a pressure of 1.8 atm. If the ball is taken outside on a hot day whereby the temperature of the ball rises to 46°C and the volume increases to 6.2 L, what will be the pressure of the air in the ball? [1.7 atm] 7. If a rigid container that can withstand a total pressure of 4.9 atm is filled with 538 kg of pure oxygen at STP is heated to 593°C, will the container explode? Prove your answer. 8. If one has the same mass of the first five noble gases all at STP, which one would need the largest containar Drove vour answer

Explanation / Answer

Let the mass of compound be 100 g

So mass of Nitrogen will be : 29.5 g

Number of moles of N = 29.5 / 14 = 2.1 mol

Mass of hydrogen = 3.2 g

number of moles of H = 3.2 / 1.008 = 3.2 mol

Mass of oxygen = 67.3 g

Number of moles of O = 67.3 / 15.999 = 4.2

dividing the number of moles by a common values , we get the ratio as 2 : 3 : 4

So the empirical formula of the compound will be : N2H3O4

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