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How many L. of N2 gas are produced at STP when the airbag inflates if the airbag contains 132 g. of Sodium Nitride?
Sulfuric acid (H2SO4) is a very strong diprotic acid. If 0.066 moles of sulfuric acid is mixed with water to make 192 mililiter of solution, what is the molarity of H+?
A gas occupies 672 mL at 785 mmHg. What volume would it occupy at 453 mmHg at constant temp??
A system absorbs 192 kj of heat and the surroundings do 120 kj of work on the system. what is the change in internal energy of the system
Supppose that a 2 L solution is made from 178 mg of citric acid (C6H8O7). What is the molar mass of C6H8O7
How many moles of CF4 can be produced when 5.00 mol C react with 8.00 mol F2?
Calculate E when 900.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
an An automobile gasoline tank holds 42 kg of gasoline. When the gasoline burns , 168 kg of oxygen are consumed and carbon dioxide and water are produced. What is the total combined mass of carbon dioxide and water that is produced
Fundamentals of chemistry - The conditions under which gases behave most ideally and Under the Bronsted?Lowry definition a base
Explain the use of nuclear isotope in medical field and Write a paragraph expaining what nuclear isotope can be used for medical purpose
You are given the following data. S(s) + 3/2 O2(g) → SO3(g) ΔH = -395.2 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH = -198.2 kJ Calculate ΔH
When NH3 is prepared from 28 g N2 and excess H2 the theoretical yield of NH3 is 34 g. When this reaction is carried out in a given experiment, only 30. g is produced.
Using a solution containing 0.302 grams of an antibiotic has an osmotic pressure of 8.34 mmHg At 23.6°C, 0.500 L. calculate its molecular mass.
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