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A gas mixture of N2 and CO2 has a total pressure of 8.00 atm and contains 12.5 mol of gas. If the partial pressure of N2 is 3.69 atm, how many moles of CO2 are in the mixture?
Calculate the number of moles of gas in a 3.24 L basketball inflated to a total pressure of 24.3 psi (pounds per square inch) at room temperature (25 degrees Celsius).
Chlorine dioxide gas is used as a commercial bleaching agent. One method of preparing ClO2 is the reactiong of chlorine gas with sodium chlorite as:
What volume of gold would be equal in mass to a piece of copper with a volume of 140.0 mL? The density of gold is 19.3g/mL; the density of copper is 8.96 g/mL.
Oxalic acid dehydrate, H2C2O4. 2H2O (formula weight = 126.1 g/mol) is sometimes used to standardize NaOH solutions. How many grams of this acid will be required to titrate 45.0 mL of 0.18 M NaOH solution
How many moles of carbon monoxide are present in the product gas. How many moles of water vapor are present in the product gas. How many moles of oxygen are present in the product gas. How many moles of nitrogen are present in the product gas.
When the one ore lead (ii) sulfide burns in ixygen, the products are lead (ii) oxide and sulfur dioxide A. How many grams of oxygen are required to react with 0.126 mole lead (ii) sulfide?
the ternary compounds called chlorofluorocarbons, or Freons, have proved to be very valuable as refrigerants and as cleaning agents for circuit boards. Unfortunately, in the atmosphere these compounds produce chlorine atoms that catalyze the decom..
How many grams of sodium formate, NaCHO2, would have to be dissolved in 1.1 L of 0.20 M formic acid (pKa 3.74) to make the solution a buffer for pH 3.82
calculate the volume in mililiters (mL) of 6 M NaOH needed to make 500 mL of a 0.100 molar (M) NaOH solution.
You use 32.0 mL of NaOH to titrate 100. mL of HCl and 22.2 mL of NaOH to titrate 50.0 mL of 0.0836 M H2SO4. Find the unknown concentrations. NaOH HCl
HNO3 has 2 dissociating ions whereas Al(NO3)3 has 4, which should result in a higher conductance value. Would this have something to do with aluminum nitrate being paired with water as a solid?
Suppose that 1.02 of rubbing alcohol evaporates from a 75.0 aluminum block. If the aluminum block is initially at 25C, what is the final temperature of the block after the evaporation of the alcohol?
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