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Air is about 78.% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules.
Part A: What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behaviorPart B: What is the partial pressure of Oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior
A graduated cylinder contains 131 mL of water. A 18.0 g piece of iron (density = 7.86 rm{g/cm^3}) and a 25.0 g piece of lead are added.
How many moles of atoms are in each of the following? 4.1*10^24 Pb atoms ,2.15*10^22 He atoms
How many moles of H2SO4 must be present to react completely with the NaOH delivered from the buret.
Calculate the half life of N2O5 and B. how long does it take for the N2O5 concentration to drop one tenth of its original value. * I believe the half life is 10,000 seconds for part A. But I am having trouble with part B.
Calculate the volume in, mililiters, of a 1.50M NaHCO3 solution that provides 28.0g NaHCO3, How many grams of H3PO4 is needed to prepare 550mL of a 0.31N solution?
A 44 sample of water absorbs 329 of heat If the water was initially at 21.7, what is its final temperature.
a. If a mint leaf is 12% methanol how much should be distilled? b. What temperature should the distillation take place-approximately?
Is the reaction spontaneous?
Choose the answer in which the three atoms and/or ions are listed in order of increasing EXPECTED size (smallest particle listed first) assuming that the simple shell model of the atom is correct.
The filter cake consists of K2CrO4 crystals and a solution that contains 36.36wt% K2CrO4. The crystals formed account for 95% of the mass of the total filter cake. The solution that passes through the filter, also 36.36wt% K2CrO4, is the recycle s..
When 1.0 g of snack cake is combusted in a constant-pressure bomb calorimeter with a heat capacity (including its water) of 10.0 kJ/°C, the temperature of the calorimeter rises by 2.24°C. How many nutritional calories (Calories) are in one serving..
What assumption is commonly used to simplify the process of finding the pH for a solution of a weak acid
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