Orbitals and Quantum number

What is the total number of p electrons in a single (ground state) P atom? Electron configuration of P is [Ne]3s2 3p3

calculate the mass of a substance when it is completely decomposed

sodium chloride is obtained when sodium carbonate is reacted with hydrochloric acid the equation for the reaction is; Na2CO3 = 2HCl ---> 2NaCl + CO2 + H20 Calculate the mass of sodium chloride that can be obtained when 53g of sodium carbonate is completely decomposed. (RAM = C=12, O=16, Na=23)

calculating the mass of sodium chloride that can be obtained from 53g of sodium carbonate is decomposed

sodium chloride is obtained when sodium carbonateis reacted with hydrochloric acid the equation for the reaction is' Na2CO3 = 2HCl --> 2NaCl + CO2 + H20 calculate the mass of sodium chloride that can be obtained when 5g of sodium carbonate is completely decomposed. (RAM = C=12, 0 = 16, Na = 23)

how mush heat is generated from burning butune

if enough butane is burned according to the following equation to produce210g or carbon dioxide, how much heat will be generated?? C4H10 = 13/2 O2 ---> 4CO2 + 5H2O

ideal gas equations

At STP, 0.280L of a gas weighs 0.400g. Calculate the molar mass of the gas.

Gas equations

Ozone molecules in the stratosphere absorb much of the harmful radiation from thr sun. the temp. and the pressure of ozone in the stratophere are 250 K and 1.0*10^-3atm. How many ozone molecules are present in 1.0 L of air under these conditions?

Calculate gas density

Calculate the density of HBr gas in grams per liter at 733 mm Hg and 46 degrees C.

gas stoichiometry

Calculate the mass in grams of Hydrogen chloride produced when 5.6 L of molecular hydrogen measured at STP react with an excess of molecular chlorine gas.

gas stoichiometry

C_2H_5OH burns in air: C_2H_5OH(l)+O_2->CO_2(g)+H_2O(l) balance the equation and determine the volume of air in liters at 35.0 C and 790 mmHg required to burn 227 g of ethanol. assume that air is 21.0 percent O_2 by volume.

daltons law of partial pressures

dry air near sea level has the following composition by volume: N_2, 78.08%; O_2 20.94%; Ar, 0.93%; CO_2 0.05%. the atmospheric pressure is 1.00 atm. calculate the partial pressure of each gas in atm and the concentration of each gas in moles per liter at 0degrees C.