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Consider the two containers below, labeled C and D, one with an ideal gas atom and one with ideal gas molecules, each at the same temperature. The gas molecule has more mass than the gas atom. one container has one molecule , and the otherone has 4. How do the pressures of the two containers compare? Why?
Calculate the pH during the titration of 32 mL of 1.149 x 10-1 M NaOH with 1.161 x 10-1 M HBr solution after the following additions of acid.
Calculate the empirical formula for a chemical compound which gives the following analysis: 65.2 g scandium and 34.8 g oxygen.
An oxide of phosphorus contains 56.4% oxygen and has a molar mass of 284 g/mol. What is the molecular formula for this compound?
The conditions of a gas change in a steady flow process from 20 degrees C and 1000 kPa to 60 degrees C and 100 kPa. Devise a reversible nonflow process
consider the following reaction. Mg+H3PO4 magnesium phosphate and hydrogen. what is the molecular formula for magnesium phosphate.
A gas mixture is made by combining 8.1 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 19.20 L. What is the molar mass of the unknown gas?
An 85.0g sample of iron requires 954 J of heat to raise its temperature 25.0C. What is the specific heat of the iron?
A 0.894-g sample of gas occupies 125 mL at 60. cm of Hg and 25C. What is the molar mass of the gas.
How much energy (in calories) is needed to heat 17cm^3 of fat from room temperature (25 C) to its melting point (35 C)?
calculate the heat energy released when 15.1g of liquid mercury at 25 degrees C is converted to solid mercury at its melting point
1 mole of a hydrocarbon of formula CnH2n was burned completely in oxygen producing carbon dioxide and water vapour only. It required 192 g of oxygen. Work out the formula of the hydrocarbon.
A saline solution contains 171 mEq/L each of Na+ and Cl-. how many moles of each of Na+ and Cl- are in 1.50 L of the saline solution.
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